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Studocu is not sponsored or endorsed by any college or university Tutorial Book Physical Chemistry Mechanical Design (Florida State University Panama City) Studocu is not sponsored or endorsed by any college or university Tutorial Book Physical Chemistry Mechanical Design (Florida State University Panama City) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
1 SCHM002 Chemistry 2 Tutorial Booklet Physical Chemistry Name:_________________________ ______________ Subject Coordinator: Ali Hunt Email: Ali.Hunt@utscollege.edu.au Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
1 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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3 In this tutorial you will be required to perform basic titration calculations, reflect upon your progress through Chemistry 1 and plan your goals for Chemistry 2. This tutorial covers four activities. YOU ARE EXPECTED TO COMPLETE THE PRE-WORK BEFORE YOUR SCHEUDLED CLASS. • Report review to build on report writing skills developed in your first semester (PRE-WORK) › In this activity, you will be provided with an experimental report and asked to grade the reports and pull out important information. This pre-work allows you to engage with the marking criteria that will be used for your report later in the semester. • Reflection on your understanding of content from Chemistry 1, and your goals for Chemistry 2 › In this activity, you will be given a series of short questions in class, and asked to reflect on your time in Chemistry 1, as well as your plans for Chemistry 2. This will be completed ONLINE, so please bring a suitable smart device (such as a mobile phone, laptop, tablet, ipod etc.) • Dry lab to demonstrate your understanding of content from Chemistry 1 › In this activity, you will revise prior knowledge learned in Chemistry 1. You will be given a laboratory situation and asked to apply previous knowledge to perform certain calculations/questions. You will need to be able to carry these skills into the Chemistry 2 labs. • Plan to achieve your goals for this semester and Chemistry 2 (POST-WORK) › In this activity, you will prepare a timetable plan for the semester. The aim of this activity is for you to develop your time management by preparing a plan early on in the semester that reflects your study commitments for the semester. Tutorial 1 Science Chemistry 2 SCHM002 TUTORIAL 1: INTRODUCTION ACTIVITY AND REVISION Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
4 PRE-WORK 1. Briefly outline the purpose, as well as any conventions used in the following sections in reporting scientific information: Introduction: Method: Results: Discussion: Conclusion: References: 2. Using your experience from semester one, what are the similarities and differences with laboratory reports and journal articles? (which of the conventions in the table above do they both have?) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
5 For the remaining pre-work you are required to read through the Method and Discussion sections of a lab report, available on Canvas, and answer the following questions (the Introduction section is provided to you for background) . You can find the report under the Week 1 module, Tutorial 1: Pre- work SUP MATERIAL, along with the marking rubric. For each section, read the report, check off the list with a tick (if included) or a cross (if missing, or lacking), and then answer the questions. 3. Method: - Written in paragraph form - Method is detailed - Method is concise (no unnecessary information) Do you think that sufficient detail was provided so that you could duplicate the method? Was there any detail that was not needed? 4. Results/Discussion: - Results are professionally presented - All Tables/Figures have appropriate labels - All results are discussed (rate law, rate constant and order) - Trends are explained - Plausible future recommendations are included - Conclusion relates back to aim How could the results have been presented more professionally? What do we mean when we ask for plausible future recommendations? 5. What overall grade would you give this report? (Use your ticks and compare them to the rubric) Please read through the following experimental method, the results will be completed in class. Confidence rating: 1 2 3 4 Guessing.. Not confident Slightly confident Very confident 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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6 ANALYSIS OF AN ASPIRIN TABLET INTRODUCTION Early Greeks and Romans were aware that the bark of the willow tree was useful in reducing fever and in relieving pain. It has been found that this pain-relieving ingredient is a compound called salicin, which consists of a sugar molecule attached to salicylic acid. It is the salicylic acid that is responsible for the analgesic (pain-reducing) and anti-pyretic (fever-reducing) effects of the willow bark. Although salicylic acid produces these desired effects, salicylic acid itself is quite toxic and produces severe irritation of the stomach lining. To make salicylic acid more useful, it is reacted with acetic acid to form an ester, acetylsalicylic acid, which we commonly call “aspirin”. Acetylsalicylic acid usually does not irritate the stomach lining to a significant extent but once it is absorbed from the stomach it passes to the liver where it is hydrolysed back to salicylic acid. Aspirin is a weak monoprotic acid, and consequently it can be estimated in a titration reaction with the strong base, NaOH. That is, The NaOH solution supplied for this experiment is not a standard solution and it must be standardised with standard HCl solution, which is supplied. The aim of this experiment is to determine the mass of aspirin present in commercially available aspirin tablets. COOH OH salicylic acid COOH OCCH 3 O acetylsalicylic acid (aspirin) + OH - CO 2 - OCCH 3 O + H 2 O COOH OCCH 3 O C 9 H 8 O 4 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
7 EXPERIMENTAL Part A: Titration of unknown NaOH with standard HCl The aim of this experiment is to determine the concentration of an unknown NaOH solution. 1. Collect 75 mL of the approximately 1M NaOH solution. Using a 50.00 mL pipette carefully dilute 50 mL to 500.0 in a volumetric flask. You will use the diluted NaOH solution you have prepared, in the titrations. 2. Collect no more than 150 mL of the standard HCl solution in a clean, dry beaker. Record the concentration of this solution in the Results section. 3. Fill a burette with the NaOH solution. Record the initial burette reading in the Results section. 4. Pipette 25.00 mL of the standard HCl solution into a conical flask. 5. Add two drops of the indicator phenolphthalein to the HCl in the conical flask. The indicator is colourless in acidic solution. 6. Titrate the HCl solution with the NaOH solution. The end-point is the first sign of a permanent colour change in the indicator. The change will be from colourless to a pale pink colour. Record the burette reading in the Results section. 7. Repeat the titration two or three times with further 25.00 mL samples of the HCl solution. Record all your burette readings in the Results section. 8. Retain your diluted NaOH solution in the volumetric flask for Part B. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
8 Part B: Determination of aspirin in a tablet The aim of this experiment is to determine the average number of grams of aspirin in a commercially available tablet. 1. Collect three aspirin tablets and weigh them together on the top-loading balance. Record the total weight and determine the average tablet weight. Place one tablet in each of three 250 mL conical flasks. Add about 30 mL of de-ionised water and 5 mL of ethanol (this helps the aspirin to dissolve) to each conical flask and gently warm the solutions over a Bunsen for about 10 minutes. The aspirin in a tablet will dissolve but some of the tablet (filler and binder) will remain undissolved. Do NOT boil the solution. Cool the solutions to room temperature before proceeding with Step 2. 2. Add two drops of phenolphthalein indicator to each aspirin solution and titrate one of the solutions with the standardised NaOH solution until an end-point is indicated. Record this titration reading in the Results section. 3. Repeat the titration of Step 2 for each of the other two aspirin solutions. You can save time by adding the NaOH solution rapidly to within about 2 mL of the rough titre, and then the NaOH solution should be added dropwise and with constant swirling of the conical flask until the end-point is reached. Record all titration readings in the Results section. 4. Calculate the average number of grams of aspirin in a tablet. 5. Determine the average % by weight of aspirin in an aspirin tablet. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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9 IN-CLASS / WEEKLY WORK The following table lists key learning outcomes that you should develop for this topic. Please complete the Yes/No column before the tutorial. In the following week, you should look back on those topics that you are not confident with, and complete the Notes column to describe what you have done to resolve any issues. Please write down what you have found and how. For example, you may ask your tutor in class, use the drop-in session, google, review the lecture notes, discuss with a peer. Points of Confusion (POC) Can you: Confident (Yes/No) Notes (What you learned and how) • Calculate FM Example: NO Revised Chem 1 lecture notes – calculate formula mass (FM) by adding the relative atomic masses of each atom in the formula using the periodic table • Calculate mass, moles and FM using n = m/M Y N • Write net ionic equations Y N • Calculate moles, concentration and volume using c = n/v Y N • Use titration data to calculate concentration Y N • Calculate dilutions Y N • Use mass to work out limiting reactants and hence theoretical yields Y N • Calculate percentage yields Y N • Report answers to the correct sig fig with correct units Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
10 Results Part A: Titration of unknown NaOH with standard HCl Exact concentration of standard HCl solution = ------------------- Volume of standard HCl solution used in a titration = ------------------- Volume of NaOH used in a titration: Rough titration Titration 1 Titration 2 Titration 3 Volume of NaOH used (mL) Mean volume of NaOH used in a titration = ------------------- Calculations In this section you will calculate the concentration of the diluted NaOH solution. Record your working in the spaces provided below. Remember units and significant figures! 1. Write a balanced net ionic equation for this reaction. 2. Calculate the moles of HCl used in the titration. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
11 3. Hence, calculate the moles of diluted NaOH. 4. Calculate the concentration of the diluted NaOH solution (this concentration will be used in Part B). Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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12 Part B: Determination of aspirin in a tablet Total mass of three tablets = ------------------- Average mass of one tablet = ------------------- Concentration of the diluted NaOH solution from Part A = ------------------- Volume of NaOH used in a Titration: Titration 1 Titration 2 Titration 3 Volume of NaOH used (mL) Mean volume of NaOH used in a titration = ------------------- Calculations In this section you will calculate the percentage mass of aspirin in an aspirin tablet. Record your working in the spaces provided below. Use the following equation for your calculations: 1. Calculate the average moles of NaOH required. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
13 2. Hence, calculate the average moles of aspirin present in a tablet. 3. Calculate the formula mass of aspirin (acetylsalicylic acid, C 9 H 8 O 4 ). 4. Hence, calculate the mass of aspirin in a tablet. 5. Determine the average % by weight of aspirin per tablet. Completed? Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
14 PRACTICE QUIZ – REVISION 1. What is the concentration of a solution that was prepared by diluting 50.0 mL of a 0.546 M into 250 mL volumetric flask? (1 mark) 2. In a titration, 25.00 mL of a 0.1009 M HCl solution was neutralised by 15.90 mL of a NaOH solution. a) Write a net ionic equation to represent the titration equation . (1 mark) b) Calculate the precise concentration of NaOH . (3 marks) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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15 3. Aspirin (C 9 H 8 O 4 ) can be prepared by reacting salicylic acid (C 7 H 6 O 3 ) with acetic anhydride (C 4 H 6 O 3 ) according to the following stoichiometric equation: 2 C 7 H 6 O 3(s) + C 4 H 6 O 3(l) → 2 C 9 H 8 O 4(s) + H 2 O (l) A sample of aspirin was prepared from 100 grams of salicylic acid and 250 g of acetic anhydride. a) Calculate the moles of each reactant. Which is the limiting reactant? (3 marks) b) Hence, what is the theoretical mass of aspirin that could be obtained? (1 mark) c) If the actual yield of aspirin obtained was 75.0 grams, what was the % yield? (1 mark) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
16 REVIEW QUESTIONS Refer to the experiment and questions answered in class. 1. Can you suggest a reason why three aspirin tablets were used in the method? 2. Would you have expected the % weight of aspirin per tablet to be 100%? Explain. 3. The method did not include any details about the correct method for rinsing the glassware. Fill out the table below by drawing a brief sketch of the following titration glassware, and list the correct way to rinse the glassware before use. Pipette Volumetric flask Burette Conical flask Sketch Rinsing method Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
17 4. A 25.00 mL aliquot of an aqueous sodium carbonate solution was titrated using 0.9420 M HCl. At the endpoint of the titration, the volume of HCl used was 17.05 mL. What is the concentration of the sodium carbonate solution? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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18 5. A 3.80 g sample of magnesium nitride was reacted with 4.20 g water according to the following equation: Mg 3 N 2(s) + 3H 2 O (l) → 2NH 3(g) + 3MgO (s) The actual yield of MgO obtained was 3.60 g. What was the percent yield of this reaction? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
19 This tutorial contains problems and calculations to do with solubility equilibria. You are expected to attempt the pre-work questions BEFORE your scheduled tutorial class. In class we will review K SP and can spend time going through questions that you may be having troubles with. Please bring a calculator! Before coming to this tutorial, you should: Revise the Equilibrium and K SP lecture notes Attempt the pre-work that follows Make sure the POC table from last week is completed Make a list of any questions that you have regarding this topic, so they can be discussed in class. Tutorial 2 Science Chemistry 2 SCHM002 TUTORIAL 2: K SP Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
20 PRE-WORK 1. Match the following terms to the correct definition: Common ion effect; Ion product (Q), (analogous to reaction quotient); Molar solubility; Saturated solution; Solubility; Solubility product constant (K SP ) a) An equilibrium constant, that describes the equilibrium of the dissolution of a sparingly soluble salt (how much the solid is likely to dissolve – a low value = very insoluble), unitless b) Quantity of solid that can be dissolved per litre of solution before the solution becomes saturated (referring to the concentration of solid that will dissolve), units generally in mol/L or g/L. c) Concentration of the ions in solution, units generally in mol/L or g/L. Analogous to the molar solubility, use mole ratio to determine solubility of ions. d) Describes the effect on equilibrium that occurs on addition of a common ion. The solubility of a sparingly soluble salt is reduced in a solution that contains a common ion. e) Product of the concentration of the ions in a salt solution raised to the same powers as K SP , i.e. describes salt solutions that are not at equilibrium. Can be used to predict if precipitation will occur. f) A solution where the solid has reached equilibrium with the dissolved ions, containing the maximum amount of solid that can dissolve. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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21 2. Write the expression for the solubility-product constant (K SP ) for the following saturated solutions. a) CuSO 4 (s) ⇌ Cu 2+ (aq) + SO 4 2 – (aq) b) Fe(OH) 2 (s) ⇌ Fe 2+ (aq) + 2OH – (aq) c) Cu 3 (PO 4 ) 2 (s) ⇌ 3Cu 2+ (aq) + 2PO 4 3 – (aq) 3. In a saturated solution of calcium fluoride at 25 °C, the concentration of calcium ions was found to be 1.24 x10 – 3 M. a) Write an equation to represent the equilibrium present in a saturated solution of calcium fluoride. b) What is the molar solubility of CaF 2 at this temperature? c) What is the concentration of [F – ]? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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22 d) Write the K SP expression. e) Calculate the value of K SP. 4. Which of the following salts has a greater solubility at 25 o C? PbCl 2 (K SP PbCl 2 = 1.7 x10 – 5 ) or PbF 2 (K SP = 3.6 x10 – 8 ) Confidence rating: 1 2 3 4 Guessing.. Not confident Slightly confident Very confident 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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23 IN-CLASS / WEEKLY WORK Points of Confusion (POC) Can you: Confident (Yes/No) Notes (What you learned and how) • Understand the terms relating to solubility equilibria – such as solubility, solubility product, molar solubility Y N • Given the name of a salt, write the formula Y N • Given a sparingly soluble salt, write the equilibrium equation Y N • Write the K SP expression for a sparingly soluble salt Y N • Solve associated K SP calculations, such as calculate the K SP, molar solubility and solubility of ions Y N • Recognise the effect of common ions and pH on solubility Y N • Solve associated calculations with a common ion Y N • Use K SP to predict if a precipitate will occur on mixing solutions Y N • Use K SP to predict and calculate selective precipitation Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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24 Lynn Turner Case: ▪ Antifreeze is a common poison ▪ It contains ethylene glycol, which is metabolised in the body ▪ Two of the major (toxic) metabolites are glycolic acid and oxalic acid ▪ Oxalic acid binds with calcium to form calcium oxalate crystals, which can damage the kidneys, brain, heart and lungs (kidney stones) Let’s take a closer look at calcium oxalate: Calcium oxalate is a sparingly soluble salt 1. Write an equation to show the equilibrium of a saturated solution of calcium oxalate (CaC 2 O 4 ). 2. Write the K SP expression for calcium oxalate. 3. Calculate the K SP of a saturated solution of calcium oxalate if concentration of oxalate ions was found to be 1.40 x10 -4 M at 25 O C. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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25 Extension Question 4. The normal amount of Ca 2+ (aq) in blood is 100 mg / 1L. Using the K SP calculated above, predict the minimum concentration of oxalate ions required to result in the precipitation of calcium oxalate (assume temperature is 25 0 C). Note that this situation is not a saturated solution at equilibrium…. Relate to Q. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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26 Using solubility to solve for K SP 5. Given that the concentration of silver ions in a saturated solution of silver chromate (Ag 2 CrO 4 ) is 1.26 x10 -4 M, calculate the K SP for this solution. Using K SP to find solubility 6. Calculate the molar solubility of lead(II) fluoride, and the concentration of lead ions and fluoride ions, in a saturated solution of lead(II) fluoride at 25 O C. K SP (PbF 2 ) = 3.6 x10 -8 @ 25 O C Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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27 Common ion effect 7. Calculate the molar solubility of iron(II) hydroxide, and the concentration of hydroxide ions, in a saturated solution of iron(II) hydroxide in: K SP (Fe(OH) 2 ) = 4.8 x10 -20 @ 25 O C a) pure water at 25 O C. b) A solution that contains 0.010 M of Fe(NO 3 ) 2 at 25 O C. c) Explain the difference in the solubilities and K SP between these two solutions Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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28 Extension Question Barium sulfate, BaSO 4 , is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A barium sulfate solution, sometimes called a cocktail, is ingested by the patient, whose stomach and intestines can then be visualized via X-ray imaging. If a patient ingests 380 mL of a saturated barium sulfate solution, how much toxic Ba 2+ (in grams) ion has the patient consumed? The solubility product K SP of BaSO 4 is 1.1 x10 -10 . Completed? Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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29 PRACTICE QUIZ – K SP (QUIZ WILL BE IN NEXT WEEK ’ S TUTORIAL) Silver carbonate is a sparingly soluble salt. 1. Write an equation to represent the equilibrium in a saturated solution of Ag 2 CO 3. (2 marks) 2. Write the K SP expression for this equilibrium. (1 mark) 3. The silver ion concentration in a saturated silver carbonate solution was found to be 2.5 x10 − 4 M. Determine the following, showing your working: a) [CO 3 2 – ] (1 mark) b) the value of K sp (2 marks) c) the molar solubility of Ag 2 CO 3 (1 mark) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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30 4. Use your value for K SP to calculate the molar solubility of Ag 2 CO 3 in a solution of 0.10 M AgNO 3 . (2 marks) 5. How does the molar solubility you calculated in Q4 compare to that calculated in Q3 c) ? Explain the difference. (1 mark) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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31 REVIEW QUESTIONS 1. What is the solubility product (K SP ) for PbBr 2 if the molar solubility of a saturated solution of PbBr 2 was found to be 0.010 M? 2. What is the molar solubility of barium carbonate if the K SP for BaCO 3 is 5.0 x10 – 9 ? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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32 3. The K SP of copper hydroxide is 4.8 x10 – 20 . What would be the [Cu 2+ ] and [OH – ] in a saturated solution of Cu(OH) 2 ? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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33 4. Calculate the molar solubility of AgBr in the following solutions: (K SP = 5.0 x10 – 13 ) a) Pure water b) 3.0 x10 – 2 M AgNO 3 solution c) 0.10 NaBr solution d) In which of these solutions is the solubility of AgBr the lowest? Why? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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34 5. Using the K SP (PbF 2 ) = 3.6 x10 -8 , will a precipitate form if: a) 500.0 mL of 0.0030 M lead nitrate, and 800.0 mL of 0.0040 M sodium fluoride are mixed? b) 500.0 mL of 0.0030 M lead nitrate, and 800.0 mL of 0.0400 M sodium fluoride are mixed? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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35 6. A solution contains 1.0 x10 -4 M Cu + and 2.0 x10 -3 M Pb 2+ . a) If a source of I - is added gradually to this solution, will PbI 2 (K SP = 1.4 x10 -8 ) or CuI (K SP = 5.3 x10 -12 ) precipitate first? b) What concentration of I - is required to start this precipitation? 7. A solution consists of 0.050 M Mg 2+ and 0.020 M Cu 2+ . a) Which ion will precipitate first as OH - is added to the solution? Mg(OH) 2 (K SP = 1.8 x10 -11 ) and Cu(OH) 2 (K SP = 2.2 x10 -20 ). b) What concentration of OH - is necessary to begin the precipitation of each cation? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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36 8. Calcium ions trigger clotting of blood. Therefore, when blood is donated the receiving bag sometimes contain oxalate salt (such as sodium oxalate) to precipitate the Ca 2+ , and thus prevent clotting. Typically, blood contains 9.7 x10 -5 g Ca 2+ /mL. What concentration of Na 2 C 2 O 4 does a medical technologist need to add to a 100 mL blood sample in order for CaC 2 O 2 to precipitate (and hence avoid blood clotting)? (K SP for calcium oxalate = 2.6 x10 -9 ) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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37 9. The normal amount of Ca 2+ (aq) in urine is 300 mg / 1L. What is the minimum concentration of oxalate ions required to result in the precipitation of calcium oxalate kidney stones? Assume that the K SP of calcium oxalate at standard body temperature is 2.6 x10 -9 . Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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38 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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39 This tutorial contains questions and calculations associated with acid-base chemistry, focusing on buffers, pH titrations and indicators. You are expected to attempt the pre-work questions BEFORE your scheduled tutorial class. In class we will review the acid-base content and can spend time going through questions that you may be having troubles with. There will be a quiz on K SP (see practice quiz in last week’s tutorial notes – page 29). Please bring a calculator! Before coming to this tutorial, you should: Revise the Acid-Base, buffer and pH titrations lecture notes Attempt the pre-work that follows Make sure the POC table from last week is completed Make a list of any questions that you have regarding this topic, so they can be discussed in class. Tutorial 3 Science Chemistry 2 SCHM002 TUTORIAL 3: ACID-BASE CHEMISTRY Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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40 PRE-WORK 1. Write the hydrolysis reaction of the following, and indicate if the solution is acidic or basic. Hydrolysis reaction Acidic or Basic? HCl (aq) NaOH (aq) HCN (aq) NH 3(aq) NH 4 + (aq) CH 3 COO – (aq) 2. (Revision) Calculate the pH of the following aqueous solutions, and indicate if the solution is acidic, basic or neutral: a) [H + ] = 0.047 M b) 1.0 x10 – 7 M OH – c) pOH = 5.33 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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41 3. Identify the conjugate acid base pairs in the following acid-base reactions a) HCl + NH 3 → NH 4 + + Cl – b) OH – + HCN → H 2 O + CN – c) PO 4 3 – + HNO 3 → NO 3 – + HPO 4 2 – 4. Calculate the pH of a buffer that is 0.120 M NaHCO 3 and 0.105 M Na 2 CO 3 . pK a (HCO 3 – ) = 10.3 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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42 5. Describe the following pH curves (e.g. strong acid added to a strong base): a) b) c) 6. For each of the titration curves above in Q5 a), b) and c), would the following indicators be a suitable choice? a) Methyl red (pKa = 5.0) b) Cresol red (pKa = 8.3) c) Bromothymol blue (pKa = 7.0) Confidence rating: 1 2 3 4 Guessing.. Not confident Slightly confident Very confident 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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43 IN-CLASS / WEEKLY WORK Points of Confusion (POC) Can you: Confident (Yes/No) Notes (What you learned and how) • Perform pH calculations to solve for pH, pOH, [H + ] and [OH - ] Y N • Identify conjugate acid- base pairs Y N • Identify the acid-base properties of anions and cations Y N • Explain what a buffer is and how it works Y N • Perform buffer calculations using the Hendersen- Hasselbalch equation Y N • Recognise acid/base titration pH curves and explain their shape Y N • Determine equivalence of an acid/base titration using a pH curve Y N • Explain why equivalence points occur at pH = 7, <7, >7 Y N • Estimate pK a of weak acids or bases using pH curves Y N • Explain how indicators work Y N • Choose an appropriate indicator for particular titrations Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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44 Buffers a) The HCO 3 – /H 2 CO 3 system is a major buffer in blood. With the help of an equation, describe how it acts as a buffer when acid (H + ) is released into the bloodstream. b) A person suffering from anxiety begins breathing rapidly and as a results suffers alkalosis, an increase in blood pH. Explain how rapid breathing can cause the pH of blood to increase. c) One cure for this problem is breathing into a paper bag. Why does this produce lower blood pH? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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45 d) The pK a1 of H 2 CO 3 = 6.1. What is the ratio of HCO 3 – to H 2 CO 3 in: Normal blood at pH = 7.4? e) An exhausted marathon runner whose blood pH is 7.1? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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46 Extension buffer question: A buffer, consisting of H 2 PO 4 - and HPO 4 2- , helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major ingredients are 6.50 g of NaH 2 PO 4 and 8.00 g of Na 2 HPO 4 per 355 mL of solution? The Ka of H 2 PO 4 - is 6.20 x10 -8 . Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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47 pH titrations a) This diagram represents a titration of a weak acid, HA, with a strong base, OH – . Match each picture below, which represents the species present at various points in the titration, to the correct part of the pH curve (1-4) and briefly justify your choice. Use slides to visualise colour. (Water removed for simplicity) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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48 Indicators Refer to the indictor colour on the ppt to answer the following questions: Methyl red a) What is the HIn colour and In – colour (acid and base forms) of this indicator? b) Estimate the pKa. c) Use the pKa to predict the range that you would expect the colour change to occur over. d) What types of titrations would this be a suitable indicator? (think about pH at equivalence) Thymol Blue a) What is the HIn colour and In – colour (acid and base forms) of this indicator? b) Estimate the pKa. c) Use the pKa to predict the range that you would expect the colour change to occur over? d) What types of titrations would this be a suitable indicator? (think about pH at equivalence) Completed? Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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49 0.0 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.0 9.0 10.0 11.0 12.0 13.0 14.0 15.0 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 50.00 pH vol added (mL ) Titration Curve PRACTICE QUIZ – PH TITRATIONS AND BUFFERS Use this pH titration curve, to answer the following questions: 1. What type of titration is shown in the plot above? (1 mark) (a) a strong acid (flask) is being titrated with a strong base (burette) (b) a weak base (flask) is being titrated with a strong acid (burette) (c) a weak acid (flask) is being titrated with a strong base (burette) (d) a strong base (flask) is being titrated with a weak acid (burette) 2. What is the equivalence volume? (1 mark) 3. What is the pH at equivalence? (1 mark) 4. What is the approximate pK a of the acid being titrated? (1 mark) (a) 2.6 (b) 5.2 (c) 9.0 (d) 13.8 5. Which one of the following reactions explains why pH > 7 at the equivalence point of the pictured titration? (“HA” is an acid like CH 3 COOH, and “B” is a base, like NH 3 ). (1 mark) (a) HA + OH − → A − + H 2 O (b) BH + ⇌ B + H + (c) A − + H 2 O ⇌ HA + OH − (d) B + H + → BH + Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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50 6. Which one of the following indicators would be the most suitable for the titration pictured above? (1 mark) (a) methyl yellow (p K a = 3.1) (b) bromocresel purple (p K a = 6.3) (c) bromothymol blue (p K a = 7.0) (d) cresol red (p K a = 8.3) 7. Consider a buffer that is prepared with 0.120 M NaHCO 3 and 0.100 M of Na 2 CO 3 . a) Explain why this solution can act as a buffer. (1 mark) b) Calclaute the pH of this buffer if the pK a of NaHCO 3 = 10.3. (2 marks) c) Which of the following represents the buffer after 0.0300 moles of base has been added? Why? (1 mark) (a) (b) (c) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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51 REVIEW QUESTIONS 1. (Revision) Calculate the pH of the following: a) A 5.0 x10 – 4 M HCl solution. b) A 0.00316 M NaOH solution. c) A 0.20 M solution of HCN. K a = 4.9 x10 – 10 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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52 2. If a buffer solution is prepared by mixing 0.10 moles of CH 3 COOH with 0.050 moles of CH 3 COO – in 1.0 L flask, calculate: a) The pH of the buffer (pk a of CH 3 COOH = 4.76). b) The pH after 0.020 moles of OH – is added to the buffer. Assume volume doesn’t change. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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53 3. What concentration of sodium ethanoate is required to give a buffer solution of pH = 5.7, if mixed with 0.50 M ethanoic acid? Use K a of CH 3 COOH (ethanoic acid) = 1.8 x10 – 5 . 4. A buffer solution contains 0.12 moles of propanoic acid (HC 3 H 5 O 2 ) and 0.10 moles of sodium propanoate (NaC 3 H 5 O 2 ) in a 1.5 L flask. The K a of propanoic acid is 1.3 x10 -5 . a) Calculate the pH of this buffer. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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54 b) Calculate the pH after 100 mL of 0.500 M of HI is added to this buffer. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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55 5. The graph below represents a pH curve obtained in a titration of a NH 3 solution with a 0.10 M solution of HCl. a) What is the equivalence volume? b) What is the pH at equivalence volume? Explain why this pH is acidic. c) What part of the titration curve can be used to estimate the pK a of NH 4 + ? Briefly explain. Hence estimate the pK a of NH 4 + . Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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56 d) For each of indicators listed below, explain if they could be used as colour indicators for this titration? Methyl violet: pK a = 0.8 Ethyl red: pK a = 5.4 Phenolphthalein: pK a = 9.5 6. Resazurin is a indicator that can be used for redox titrations. Use the following observations to estimate: a) the HIn colour b) the In – colour c) the pKa of resazurin. pH Colour 2.1 Orange 3.8 Orange 6.4 Purple 8.8 Purple 0.0 1.0 2.0 3.0 4.0 5.0 6.0 7.0 8.0 9.0 10.0 11.0 12.0 13.0 0.00 20.00 40.00 60.00 pH vol added (mL) Titration Curve Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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57 Integrated question 7. What is the pH of a saturated solution of magensium hydroxide at 25 °C. K SP of Mg(OH) 2 = 1.6 x10 -12 . Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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58 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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59 This tutorial contains problems and calculations associated with the kinetics content. You are expected to attempt the pre-work questions BEFORE your scheduled tutorial class. In class we can spend time going through the questions that you may be having troubles with. There will be a quiz on pH titrations and buffers (see practice quiz in last week’s tutorial notes – page 49). Please bring a calculator! Before coming to this tutorial, you should: Revise the kinetics lecture notes Attempt the pre-work that follows Make sure the POC table from last week is completed Make a list of any questions that you have regarding this topic, so they can be discussed in class. Tutorial 4 Science Chemistry 2 SCHM002 TUTORIAL 4: KINETICS Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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60 PRE-WORK Factors that affect reaction rates 1. Reactions can proceed at different rates. List an example (can be a chemical reaction or an everyday example) of a fast reaction and a slow reaction. 2. List 4 factors that can have an effect on the reaction rate. For each, list the factor, describe how it affects the rate and give an example (can be a chemical reaction or an everyday example). 3. What is the collision theory? How is it related to the rate of reactions? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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61 Rates of reaction 4. It was found in an investigation of the reaction: CH 3 CHO (g) → CH 4(g) + CO (g), that the concentration of CH 3 CHO changed from 2.55 x10 -2 mol/L to 2.37 x10 -2 mol/L in 6 minutes. What is the average rate of reaction with respect to CH 3 CHO over that period? 5. Write the rate expressions for the following reactions to show the relationship between the disappearance of the reactants and the appearance of products: a) I - (aq) + OCl - (aq) → Cl - (aq) + OI - (aq) b) 3O 2(g) → 2O 3(g) c) 4NH 3(g) + 5O 2(g) → 4NO (g) + 6H 2 O (g) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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62 Relating rates of reactions 6. Consider the following reaction: C 3 H 8(g) + 5O 2(g) → 3CO 2(g) + 4H 2 O (g) . If, at a given moment, C 3 H 8 is reacting at a rate of 0.400 molL -1 s -1 , what is: a) The rate of formation of CO 2 ? b) The rate of formation of H 2 O? c) The rate at which O 2 is reacting? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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63 Rate laws 7. For the reaction A + 2B → C + D The rate of appearance of product C can be monitored using the following rate law expression: ?[?] ?? = k[A][B] 2 Explain each of the components of the rate law: a) ?[?] ?? b) k c) [A] d) [B] 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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64 k 1 k 2 Mechanisms 8. What is the molecularity of each of the following elementary reactions? a) Cl 2(g) → 2Cl (g) b) OCl - (g) + H 2 O (g) → HOCl (g) + OH - (g) c) 2Br . (aq) → Br 2(aq) 9. The net reaction H 2 + 2ICI → I 2 + 2HCl Proceeds via the following mechanism: H 2 + ICI → HI + HCl SLOW HI + ICI → I 2 + HCl FAST a) Write the rate law for the net reaction. b) What species (if any) is an intermediate? Confidence rating: 1 2 3 4 Guessing.. Not confident Slightly confident Very confident 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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65 IN-CLASS / WEEKLY WORK Points of Confusion (POC) Can you: Confident (Yes/No) Notes (What you learned and how) • Calculate the average rate Y N • Relate reaction stoichiometry to relative reaction rates of reactants and products Y N • Describe factors that affect rate and relate to collision theory Y N • Understand catalyst work by providing an alternate reaction mechanism Y N • Write rate law expressions and define all associated terms Y N • Use the initial rate method to determine reaction orders and rate constants from experimental data Y N • Use integrated rate laws to calculate the order of a reaction, calculate k and write the rate law expression Y N • Give units for k, depending on the order of the reaction Y N • Calculate the half-life of first order reactions Y N • Describe the molecularity of a reaction Y N • Choose a mechanism of reaction based on experimentally derived rate laws Y N • Use Arrhenius equation Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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66 Relating rates of reactions Rate laws 1. A reaction, A + B + C → products, was found to have the following rate law rate = k[A] 2 [B] a) What is the order of the reaction with respect to reactant A? What effect will doubling the concentration of A have on the rate? b) What is the order of the reaction with respect to reactant B? What effect will doubling the concentration of B have on the rate? c) What is the order of the reaction with respect to reactant C? What effect will doubling the concentration of C have on the rate? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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67 2. An eye irritant in smog is formaldehyde, HCHO, formed by the reaction of ozone with ethene: C 2 H 4(g) + O 3(g) → 2HCHO (g) + ½O 2(g) The following data was obtained by varying the initial concentrations of the reactants: Initial Concentrations Rate [C 2 H 4 ] (molL -1 ) [O 3 ] (molL -1 ) + ?[????] ?? (molL -1 s -1 ) (1) 1.0 x10 -4 0.50 x10 -5 1.0 x10 -10 (2) 1.0 x10 -4 1.5 x10 -5 3.0 x10 -10 (3) 2.0 x10 -4 0.50 x10 -5 4.0 x10 -10 a) Determine the rate law for this reaction using the above data. Give your reasoning. b) Calculate the rate constant for this reaction at this temperature. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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68 3. The following data were collected for the decomposition of nitrous oxide (“laughing gas”) on a gold catalyst at 900 °C. The data was plotted to give the following graphs: 2N 2 O (g) → 2N 2(g) + O 2(g) Time (min) [N 2 O] (mol/L) ln [N 2 O] 1 / [N 2 O] (L/mol) 0 0.0999 -2.30 10.0 15 0.0835 -2.48 12.0 30 0.0680 -2.69 14.7 80 0.0350 -3.35 28.6 120 0.0220 -3.82 45.5 y = 0.0999e -0.013x 0.0000 0.0500 0.1000 0.1500 0 20 40 60 80 100 120 [N 2 O] (mol/L) time (min) [N 2 O] vs t y = -0.0128x - 2.3037 -5.00 -4.00 -3.00 -2.00 -1.00 0.00 0 20 40 60 80 100 120 ln [N 2 O] time (min) ln [N 2 O] vs t y = 10.011e 0.0128x 0.0 10.0 20.0 30.0 40.0 50.0 0 20 40 60 80 100 120 1 / [N 2 O] (L/mol) time (min) 1 / [N 2 O] vs t Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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69 a) What is the order of the reaction with respect to N 2 O? Give your reasoning. b) Give the rate law expression. c) What is the rate constant for this reaction? d) Estimate the half-life of N 2 O. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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70 4. The radioactive isotope 51 Cr is used to evaluate the lifetime of red blood cells. It ’ s t ½ = 27.7 days. A hospital laboratory has 80.0 mg of 51 Cr. How much of the 51 Cr is left after 85 days? Arrhenius question (Extension) 5. The activation energy of popping popcorn is 53.8 kJ/mol. How many times faster will the reaction occur at 250°C then 210 °C ? Completed? Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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71 PRACTICE QUIZ – KINETICS 1. The following data were collected for the following reaction at a particular temperature. A + B ⟶ C Experiment Initial [A] (M) Initial [B] (M) Initial Rate of Formation of C (molL -1 min -1 ) 1 0.10 0.10 4.0 x10 -4 2 0.10 0.20 1.6 x10 -3 3 0.20 0.20 3.2 x10 -3 a) What is the order of the reaction w.r.t [A]? Give your reasoning. (3 marks) b) What is the order of the reaction w.r.t [B]? Give your reasoning. (in above) c) Write the overall rate law expression for this reaction and give the rate constant. (3 marks) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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72 0 2 4 6 8 0 5 10 15 20 25 1/[NaN 3 ] time (min) 1/[NaN 3 ] -2 -1.5 -1 -0.5 0 0 5 10 15 20 25 ln [NaN 3 ] time (min) ln [NaN 3 ] 2. The following data was collected for the decomposition of sodium azide to nitrogen gas, which is the reaction used to inflate airbags. 2 NaN 3(s) → 2 Na (s) + 3 N 2(g) Time (min) [NaN 3 ] (molL -1 ) 0 0.500 1 0.473 5 0.378 10 0.286 15 0.216 20 0.163 a) What is the order of this reaction? Give your reasoning. (1 mark) b) Hence, write the rate law expression for this decomposition. (1 mark) c) What is the value for k? (remember units). (2 marks) y = 0.2009x + 1.7961 y = -0.056x - 0.6926 0 0.1 0.2 0.3 0.4 0.5 0.6 0 5 10 15 20 25 [ NaN 3 ] time (min) [NaN 3 ] y = -0.017x + 0.4809 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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73 REVIEW QUESTIONS 1. The rate of disappearance of HCl was measured for the following reaction: CH 3 OH (aq) + HCl (aq) → CH 3 Cl (aq) + H 2 O (l) . Time (hours) [HCl] (mol/L) 0.0 1.85 1.8 1.36 7.2 0.580 Calculate the average rate of reaction between the 1.8 hours to 7.2 hours interval. 2. Consider the following combustion: 2H 2(g) + O 2(g) → 2H 2 O (g) . If hydrogen is burning at a rate of 0.85 mol/s, what is the rate of consumption of oxygen? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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74 3. The decomposition of N 2 O 5 in carbon tetrachloride proceeds as follows: 2 N 2 O 5 → 4NO 2 + O 2 The rate law is first order with respect to N 2 O 5 . At 64 °C the rate constant is 4.82 x10 -3 s -1 . a) Write an expression for the rate law for the reaction. b) What is the rate of reaction when [N 2 O 5 ] = 0.0240 M? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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75 4. The following data were obtained at 650 K for the reaction: 2NO (g) + O 2(g) → 2NO 2(g) Initial Concentrations Rate [NO] (molL -1 ) [O 2 ] (molL -1 ) – ?[NO] ?t (molL -1 s -1 ) (1) 0.020 0.010 2.0 x10 -4 (2) 0.040 0.010 8.0 x10 -4 (3) 0.020 0.040 8.0 x10 -4 a) Deduce the rate law for the reaction. Give your reasoning. b) Calculate the rate constant. c) Using the rate constant from b) , calculate the rate of appearance of NO AND the rate of disappearance of O 2 at the instant when [NO] = 0.030 M and [O 2 ] = 0.020 M. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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76 5. The gas-phase decomposition of NO 2 at 383 °C gives NO and O 2 according the equation: 2NO 2(g) → 2NO (g) + O 2(g) The following data was obtained experimentally: Time (s) [NO 2 ] (mol/L) ln [NO 2 ] 1 / [NO 2 ] (L/mol) 0 0.1000 -2.303 10.00 5 0.01700 -4.075 58.82 10 0.009000 -4.711 111.1 15 0.006200 -5.083 161.3 20 0.004700 -5.360 212.8 a) What does this graph (In [NO 2 ] vs t) reveal about the order with respect to NO 2 ? -6.000 -5.000 -4.000 -3.000 -2.000 -1.000 0.000 0 5 10 15 20 ln [NO2] time (s) ln [NO 2 ] vs t 0.0000 0.0200 0.0400 0.0600 0.0800 0.1000 0.1200 0 5 10 15 20 [NO 2 ] (mol/L) time (s) [NO 2 ] vs t Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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77 b) What does this graph (1 / [NO 2 ] vs t) reveal about the order with respect to NO 2 ? c) Hence write the rate law expression for this reaction. d) What is the value (with correct units) for the rate constant at this temperature? y = 10.16x + 9.1984 0.00 50.00 100.00 150.00 200.00 250.00 0 5 10 15 20 1 / [NO 2 ] (L/mol) time (s) 1 / [NO 2 ] vs t Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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78 6. At 500 ° C, the first order conversion of cyclopropane to propylene has a rate constant of 1.16 x10 -6 s -1 . If the initial concentration of cyclopropane is 1.00 x10 -2 mol/L at 500 ° C, what will its concentration be 24.0 hours after the reaction begins? 7. The reaction, SO 2 Cl 2(g) → SO 2(g) + Cl 2(g) is first order with k = 2.2 x10 -5 s -1 at 320 °C .What percentage of SO 2 Cl 2 is decomposed on heating at 320 °C for 90 minutes? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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79 8. Urea (NH 2 CONH 2 ) is the end product in protein metabolism in animals. The decomposition of urea in 0.1 M HCl occurs according to the reaction: NH 2 CONH 2(aq) + H + (aq) + 2H 2 O (l) → 2NH 4 + (aq) + HCO 3 - (aq) The reaction is first order with respect to urea and first order overall. When [NH 2 CONH 2 ] = 0.200 M, the rate of the reaction at 61 ° C is 8.56 x10 -5 molL -1 s -1 . a) What is the value for the rate constant at this temperature? b) What is the concentration of urea after in this solution after 4.00 x10 3 seconds, if the starting concentration is 0.500 M? c) Estimate the value for the half-life of this reaction. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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80 k 1 k 2 Mechanisms 9. A possible mechanism for the reaction, 2A + B → C + D, is: (1) A + A ⇌ A 2 slow, equilibrium (2) A 2 + A → A 3 fast (3) A 3 + B → A + C + D fast According to the mechanism, the rate law will be (select answer): (a) Rate = k[A] 2 (b) Rate = k[A][B] (c) Rate = k[A] 2 [B] (d) Rate = k[A] 3 10. Ozone reacts with nitrogen dioxide to produce dinitrogen pentoxide and oxygen: O 3(g) + 2NO 2(g) → N 2 O 5(g) + O 2(g) The reaction is believed to occur is two steps: O 3(g) + NO 2(g) → NO 3(g) + O 2(g) NO 3(g) + NO 2(g) → N 2 O 5 (g) The experimental rate law is rate = k[O 3 ][NO 2 ]. What can you say about the relative rates of the two steps of the mechanism? (i.e. which step is the rate determining step?) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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81 Arrhenius equation 11. The gas-phase decomposition of HI into H 2 and I 2 is found to have E a = 182 kJ/mol. The rate constant at 700 °C is 1.57 x10 -5 Lmol -1 s -1 . What is value of k at 800 °C? 12. Understanding the high temperature behaviour of nitrogen oxides is essential for controlling pollution generated in vehicle engines. The decomposition of nitric oxide (NO) to N 2 and O 2 is second order with a rate constant of 0.0796 Lmol -1 s -1 at 737 °C and 0.0815 Lmol -1 s -1 at 947 °C. Calculate the activation energy for the reaction. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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82 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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83 This tutorial contains problems and calculations associated with electrochemistry and thermochemistry. You are expected to attempt the pre-work questions BEFORE your scheduled tutorial class. In class we can spend time going through the questions that you may be having troubles with. There will be a quiz on kinetics (see practice quiz in last week’s tutorial notes – page 71). Please bring a calculator! Before coming to this tutorial, you should: Revise the electrochemistry and thermochemistry lecture notes Attempt the pre-work that follows Make sure the POC table from last week is completed Make a list of any questions that you have regarding this topic, so they can be discussed in class. Tutorial 5 Science Chemistry 2 SCHM002 TUTORIAL 5: ELECTROCHEMISTRY AND THERMOCHEMISTRY Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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84 PRE-WORK Electrochemistry 1. A galvanic cell is to be constructed using the following couples: Fe 3+ / Fe 2+ E° = 0.77 V Sn 4+ / Sn 2+ E° = 0.15 V Will there be a spontaneous reaction between the following pairs? Note there is only one combination that will give a spontaneous reaction . Justify your answers and calculate the standard cell potential (E° cell ) for the combination that gives a spontaneous reaction. a) Sn 2+ and Fe 2+ b) Sn 2+ and Fe 3+ c) Sn 4+ and Fe 2+ d) Sn 4+ and Fe 3+ Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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85 2. Explain how zinc gives sacrificial protection to steel. Fe 2+ / Fe E° = + 0.44 V Zn 2+ / Zn E° = - 0.76 V 3. Explain why aluminium metal cannot be produced by the electrolysis of aqueous solutions of aluminium salts. H 2 O / H 2 E° = - 0.83 V Al 3+ / Al E° = - 1.66 V Thermochemistry 1. What is the specific heat capacity? Give the equation that uses the specific heat capacity to find the quantity of heat (q) involved in a reaction. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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86 2. Define the following terms, give the formula used to calculate, AND give the units generally used to report these values: a) ΔH b) ΔS c) ΔG 3. Gibbs free energy can used to predict the spontaneity of a reaction. Which of the following scenarios leads to a spontaneous reaction? ΔG < 0 ΔG = 0 ΔG > 0 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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87 4. Predict which substances have a higher entropy: a) Gas H 2 O or Water H 2 O b) 1 mol of Pb (s) or 1 mol of Pb (l) c) During Greek empire Now Confidence rating: 1 2 3 4 Guessing.. Not confident Slightly confident Very confident 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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88 IN-CLASS / WEEKLY WORK Points of Confusion (POC) Can you: Confident (Yes/No) Notes (What you learned and how) • Identify species as an oxidant and a reductant Y N • Balance redox reaction using half-equations in acidic conditions Y N • Construct galvanic cells, showing all components Y N • Use Tables of Standard Reduction Potentials Y N • Predict if a spontaneous reaction will occur with given species, predict anode/cathode components and calculate cell potential Y N • Use the Nernst equation to determine spontaneity and cell potential Y N • Identify redox reactions occurring in corrosion Y N • Identify electrolysis and the processes occurring in electrolysis and predict products formed Y N • Predict how the entropy will change through phase changes Y N • Calculate standard entropy and enthalpy values Y N • Calculate Gibbs free energy and use it predict the spontaneity or a reaction Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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89 1. A galvanic cell is constructed using the following couples: Cu 2+ (aq) / Cu (s) E° = + 0.34 V Zn 2+ (aq) / Zn (s) E° = - 0.76 V Calculate the E cell when the galvanic cell is constructed with [Cu 2+ ] = 1.0 M, [Zn 2+ ] = 0.010 M, at a temperature of 25°C. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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90 2. (Extension) On the diagram below, show how you would construct a galvanic cell using the following couples: MnO 4 – (aq) , H + / MnO 2(s) E° = + 1.68 V Zn 2+ (aq) / Zn (s) E° = - 0.76 V Clearly show the following on the diagram: a) Which half cell is the cathode and which is the anode b) What metal/material each electrode would be made of c) What solutions should be in the beakers d) The direction that the electrons would flow through the wire e) Assuming the salt bridge contains NaNO 3 as an electrolyte, show the directions Na + and NO 3 – ions would migrate in the salt bridge when the cell is operating f) Write the relevant balanced half-equations underneath each cell, and the overall redox equation g) Calculate the E 0 cell h) Calculate the E cell when the galvanic cell is constructed with [MnO 4 - ] = 8.0 x10 -2 M, [Zn 2+ ] = 2.0 x10 -4 M, at a pH of 3.8 and a temperature of 25°C. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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91 3. If 200 grams of water is to be heated from 24.0°C to 100.0°C to make a cup of tea, how much heat must be added? The specific heat of water is 4.18 J/g∙C 4. An aluminum skillet weighing 1.58 kg is heated on a stove to 173 o C. Suppose the skillet is cooled to room temperature, 23.9 o C. How much heat / energy must be removed to cause this cooling? The specific heat of aluminum is 0.901 J/g o C. 5. Calculate the temperature change when 10.0 kg of water loses 232 kJ of heat. The specific heat of water is 4.18 J/g∙C 6. What is the final temperature of a sample of copper if 1.96 kJ of heat are added to 500. g of copper initially at 20.0°C. The heat capacity of copper is 0.572 J/g∙C. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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92 7. The following reaction shows the decomposition of calcium carbonate. CaCO 3(s) → CaO (s) + CO 2(g) H f o (kJmol -1 ) S o (JK -1 mol -1 ) CaCO 3(s) -1207 92.9 CaO (s) -635 398 CO 2(g) -393.5 213 a) Determine the standard enthalpy change for the decomposition of one mole of solid calcium carbonate. b) Determine the standard entropy change for the decomposition of one mole of solid calcium carbonate. c) Calculate ∆G° for the reaction at 25.0°C. Is this reaction spontaneous? d) At what temperature would reaction become spontaneous? Completed? Y N Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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93 PRACTICE QUIZ – ELECTRO AND THERMO CHEM Consider a galvanic cell constructed that uses the following equation: Pb 2+ (aq) + Cd (s) → Pb (s) + Cd 2+ (aq) Useful data: Pb 2+ / Pb E° = - 0.126 V Cd 2+ / Cd E° = - 0.403 V E cell = E° - ?? ?? ln Q R = 8.314 JK -1 mol -1 F = 96500 Cmol -1 1. Calculate the cell potential of a galvanic cell that runs at 25.0°C where [Cd 2+ ] = 0.0200 M and [Pb 2+ ] = 0.200 M. (6 marks) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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94 2. What is the final temperature of a 250 g sample of ethanol, initially at 22 °C, if 32.4 kJ of heat is added in process of making mulled wine. The heat capacity of ethanol is 2.44 J/g∙C . (2 marks) 3. Calculate ∆ S° for the synthesis of ammonia at 25°C, and account for the sign of ∆S°: (2 marks) N 2 (g) + 3H 2 (g) → 2 NH 3 (g) ∆ S°( N 2 ) = 191.5 J/mol.K ; ∆ S°( H 2 ) = 130.6 J/mol.K; ∆ S°( NH 3 ) = 192.5 J/mol.K. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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95 REVIEW QUESTIONS 1. A galvanic cell is constructed that uses the following reaction and operates at 298 K: Zn (s) + Ni 2+ (aq) → Zn 2+ (aq) + Ni (s) Ni 2+ / Ni E° = - 0.28 V Zn 2+ / Zn E° = - 0.76 V What is the cell potential of this cell when [Ni 2+ ] = 0.200 M and [Zn 2+ ] = 0.900 M Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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96 2. A galvanic cell is constructed that uses the following reaction and operates at 298 K: 2Al (s) + 3I 2(s) → 2Al 3+ (aq) + 6I – (aq) I 2 / I - E° = + 0.54 V Al 3+ / Al E° = - 1.66 V What is the cell potential of this cell when [Al 3+ ] = 4.0 x10 -3 M and [I – ] = 0.010 M? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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97 3. A galvanic cell uses the following reaction: Al (s) + 3Ag + (aq) → Al 3+ (aq) + 3Ag (s) What is the effect on the cell voltage when: a) More Al 3+ ions are added to the anode (without increasing volume) b) The size of the aluminium electrode in increased c) Water is added to the anode compartment, diluting the solution 4. A ship’s hull can be protected from corrosion using a sacrificial anode. Assuming the hull is composed of iron, which of the following could be used to protect the hull from corrosion. Explain your answer. Zn, Cu, Ni Cu 2+ / Cu E° = + 0.34 V Ni 2+ / Ni E° = - 0.28 V Fe 2+ / Fe E° = - 0.44 V Zn 2+ / Zn E° = - 0.76 V Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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98 5. If the following salts are electrolysed, what products would form at the cathode and at the anode? You can refer to a S.R.P table (Canvas) to see the half equations. a) Molten MgBr 2 b) Molten AlCl 3 c) Molten NaCl d) Aqueous NaCl (concentrated – this favours oxidation of Cl in preference to water ) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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99 6. In your backyard, you have a swimming pool that contains 5.19 x10 3 kg of water. How many kJ are required to raise the temperature of this water from 7.2 °C to 25.0 °C? 7. How many grams of water would require 2200 joules of heat to raise its temperature from 34°C to 100°C? The specific heat of water is 4.18 J/g∙C 8. Determine the specific heat of a certain metal if a 450 gram sample of it loses 34 500 Joules of heat as its temperature drops by 97 o C. 9. A system at 776.5 K undergoes a change in enthalpy of – 5.711 kJ/mol. If the free energy value is 6.771 kJ/mol, what is the change in entropy? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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100 10. Consider the following reaction: N 2 (g) + O 2 (g) → 2 NO (g) Δ H f o (kJmol -1 ) Δ S o (JK -1 mol -1 ) N 2 (g 0 191.4 O 2 (g) 0 204.9 NO (g) 90.4 210.5 a) Determine the standard enthalpy change. b) Determine the standard entropy change. c) Calculate ∆G° for the reaction. Is this reaction spontaneous? d) At what temperature would you need to increase/decrease to, for the reaction to become spontaneous? Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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101 This tutorial is related to preparing for your upcoming mid-semester test, covering all the physical chemistry content. If time permits, we will also peer review drafts of the practical report, so please make sure to have your draft on hand. You are expected to attempt the pre-work BEFORE your scheduled tutorial class. In class we can spend time going through typical test questions as a way to revise the physical chemistry content. There will be a quiz on electrochemistry and thermochemistry (see practice quiz in last week’s tutorial notes – page 93). Please bring a calculator! Before coming to this tutorial, you should: Revise the physical chemistry lecture notes Attempt the pre-work that follows Make a list of any questions that you have regarding any topic from the lectures, labs or tutorials, so they can be discussed in class. Tutorial 6 Science Chemistry 2 SCHM002 TUTORIAL 6: PHYSICAL CHEMISRTY REVISION Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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102 PRE-WORK 1. Please draft a version of your handwritten, A4 page of notes that you will bring into the test. Bring this page of notes with you to the tutorial class . It will help you to answer the questions. It will also help to bring your lecture notes to class. Some tips on creating exam notes: https://www.universitysurvival.com/student-topics/preparing-a-cheat-sheet-2/ https://www.seventeen.com/life/school/a43503/students-who-made-the-most- out-of-their-cheat-sheet/ 2. In class, we will go through a multiple-choice paper. Please attempt the questions on the following pages , so we can spend time in class with ones that you may require help with. Although your paper will also involve short answer questions, these questions will prepare you for the types of questions you may see in the mid-semester test. We will not have time to complete all questions in class. 0 1 2 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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103 IN-CLASS / WEEKLY WORK MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1. Consider the following table of Ksp values. Which compound listed below has the smallest molar solubility in water? (a) Cd(OH) 2 (b) CaF 2 (c) AgI (d) ZnCO 3 (e) CdCO 3 2. The solubility of lead (II) chloride (PbCl 2 ) is 1.6 × 10 -2 M. What is the Ksp of PbCl 2 ? (a) 1.6 × 10 -5 (b) 1.6 × 10 -2 (c) 5.0 × 10 -4 (d) 3.1 × 10 -7 (e) 4.1 × 10 -6 3. What is the molar solubility of magnesium carbonate ( MgCO 3 ) in water? The solubility-product constant for MgCO 3 is 3.5 × 10 -8 at 25 °C. (a) 2.6 × 10 -4 (b) 1.9 × 10 -4 (c) 1.8 × 10 -8 (d) 7.0 × 10 -8 (e) 7.46 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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104 4. Of the substances below, ________ will decrease the solubility of Pb(OH) 2 in a saturated solution. (a) H 2 O 2 (b) NaNO 3 (c) Pb(NO 3 ) 2 (d) NaCl (e) HNO 3 5. Which of the following ions will act as a weak base in water? (a) Cl – (b) NO 3 – (c) OH – (d) ClO – (e) None of the above will act as a weak base in water. 6. A solution is prepared by dissolving 0.23 mol of hypochlorous acid and 0.27 mol of sodium hypochlorite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The K a of hypochlorous acid is 1.36 × 10 -3 at 25 °C. (a) H 2 O (b) Hypochlorous acid (c) H 3 O + (d) Hypochlorite ion (e) This is a buffer solution: the pH does not change upon addition of acid or base. 7. What is the pH of a buffer solution that is 0.150 M in lactic acid and 0.110 M in sodium lactate? The K a of lactic acid is 1.4 × 10 -4 at 25 °C. (a) 3.98 (b) 5.64 (c) 3.72 (d) 14.13 (e) 10.28 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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105 8. A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve below was obtained. Which of the following indicators would be best for this titration? (a) phenolpthalein (b) methyl orange (c) bromothymol blue (d) methyl red (e) bromocresol purple 9. Which one of the following is not a valid expression for the rate of the reaction below? 4NH 3(g) + 7O 2 (g) → 4NO 2 (g) + 6H 2 O (g) (a) – 1 4 Δ NH 3 Δt (b) – 1 7 Δ O 2 Δt (c) – 1 4 Δ NO 2 Δt (d) + 1 6 Δ H 2 O Δt (e) All of the above are valid expressions of the reaction rate. 10. The rate law of a reaction is rate = k[D][X]. The units of the rate constant are ________. (a) mol 2 L -2 s -1 (b) L mol -1 s -1 (c) mol L -1 s -2 (d) mol L -1 s -1 (e) L 2 mol -2 s -1 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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106 11. The data in the table below were obtained for the reaction: 2 ClO 2(aq) + 2 OH – (aq) → ClO 3 – (aq) + ClO 2 – (aq) + H 2 O (l) The rate constant for this reaction is ________M -2 s -1 ? (a) 115 (b) 1.15 × 10 4 (c) 230 (d) 4.6 (e) 713 12. For a first-order reaction, a plot of ________ versus ________ is linear. (a) 1 [A] t , t (b) ??[?] ? , t (c) t , 1 [A] t (d) [?] ? , t (e) ??[?] ? , 1 ? 13. A compound decomposes by a first-order process. If 17.0% of the compound decomposes in 60.0 minutes, the half-life of the compound is ________. (a) 198 minutes (b) 223 minutes (c) 141 minutes (d) 325 minutes (e) 181 minutes Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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107 14. A particular first-order reaction has a rate constant of 1.35 × 10 2 s -1 at 25.0 °C. What is the magnitude of k at 80.0 °C if Ea = 55.5 kJ/mol? (a) 2.26 × 10 -4 (b) 0.243 (c) 4.12 (d) 4.43 × 10 3 (e) 135.5 15. The mechanism for formation of the product X is: The intermediate reactant in the reaction is ________. (a) A (b) B (c) C (d) D (e) X 16. The standard cell potential (E°cell) for the reaction below is +0.63 V. The cell potential for this reaction is ________ V at 25 °C when [ Zn 2+ ] = 1.5 M and [Pb 2+ ] = 2.0 × 10 -4 M. Pb 2+ (aq) + Zn (s) → Zn 2+ (aq) + Pb (s) (a) 0.41 (b) 0.74 (c) 0.63 (d) 0.52 (e) 0.85 17. Which of the following metals could be used as a sacrificial anode to provide cathodic protection to a zinc pipe? E° zinc = – 0.76 V. (a) Nickel (E° = – 0.26 V) (b) Iron (E° = – 0.46 V) (c) Lithium (E° = – 3.04 V) (d) Copper (E° = + 0.34 V) (e) Lead (E° = – 0.13 V) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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108 18. A sample of calcium carbonate absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1 °C to 28.5 °C. If the specific heat of calcium carbonate is 0.82 J/g·K, what is the mass (in grams) of the sample? (a) 5.0 (b) 3.7 (c) 7.5 (d) 5.0 × 10 3 (e) 410 19. Which one of the following processes produces a decrease in the entropy of the system? (a) mixing of two gases into one container (b) melting ice to form water (c) boiling water to form steam (d) freezing water to form ice (e) dissolution of solid KCl in water 20. Consider the reaction: NH 3(g) + HCl (g) → NH 4 Cl (s) Given the following table of thermodynamic data, determine the temperature (in °C) above which the reaction is nonspontaneous. (a) This reaction is spontaneous at all temperatures. (b) 1235 (c) 432.8 (d) 618.1 (e) 345.0 Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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109 Answer Key: 1. (c) 2. (a) 3. (b) 4. (c) 5. (d) 6. (d) 7. (c) 8. (c) 9. (c) 10. (b) 11. (c) 12. (b) 13. (b) 14. (d) 15. (d) 16. (d) 17. (c) 18. (c) 19. (d) 20. (e) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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110 REVIEW QUESTIONS There are additional past papers and study notes available on Canvas. For review, please complete the questions at the end of each of the physical chemistry tutorials and lectures. There are additional questions for each topic at the end of each Module in Canvas, under the Extra Resources page. Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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DATA AND FORMULAS R = 8.314 JK -1 mol -1 F = 9.65 x 10 4 JV -1 mol -1 pH = – log[H + ] pH = pK a + log [A - ] [HA] E = E° – RT nF lnQ q = mC S Δ T Δ G° = Δ H° – T Δ S° t ½ = In 2 k [A] t = [A] 0 e − kt ln[A] t − ln[A] 0 = − kt ? [?] ? − ? [?] ? = kt k = Ae – (Ea/RT) ln ?? ?? = ?? ? ( ? ?? – ? ?? ) Downloaded by Timothy Handoko (hantimo210@gmail.com) lOMoARcPSD|23633319
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Course Home openvellum.ecollege.com/course.html?courseld=16921657&OpenVellumHMAC=3296af0fdfd0081ea26215c9d534a898#10001 YouTube N Netflix Khan ) Turnitin O Zoom N Canvas Pearson Sign In E Reading List ... CHEM-341 Fall 2021 Hi, Jarrett Sign Out Help Mastering Chemistry Course Home My Courses Syllabus Part A Scores eТext List the following compounds from highest boiling to lowest boiling: Rank the compounds from highest boiling to lowest boiling. To rank items as equivalent, overlap them. Document Sharing Reset Help User Settings Course Tools > OH N- ОН `N' H NH2 highest boiling lowest boiling The correct ranking cannot be determined.
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Safari File Edit View History Bookmarks Develop Window Help Not Secure - a5.chem.binghamton.edu o E LON-CAPA t30p04a O [엘소드/KR Elswrod] 범… MC Kimetsu no Yaiba - Di. As you work on the questions, have your lab manual and text book handy. If you have questions go to one of the office hours and remember, do not leave it for the last minute! In the titration of 25.00 mL of a water sample, it took 19.090 mL of 3.165x 10-3 M EDTA solution to reach the endpoint. Calculate the number of moles of EDTA required to titrate the water sample. (enter your answer with 3 significant figures) 6.04x10-5 You are correct. Your receipt no. is 151-9969 ? Previous Tries The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures) 6.04x10-5 You are…
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ter 9- CHEM A054 520 2 x Question 12 - Chapter 9 part 2 X с Chapter 9 part 2 Homework i 12 1 points ezto.mheducation.com/ext/map/index.html?_con=con&external_browser=0&launchUrl=https%253A%252F%25 8 01:46:13 eBook Hint Print References Mc Graw Hill CH6_Chem103 - Kenai Peninsu X + °C Determine the freezing point of an aqueous solution that is 0.584 m sucrose. Saved DU
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MISSED THIS? Watch IWE: Half-Reaction Method of Balancing Aqueous Redox Equations in Acidic Solution ; Read Section 20.2. You can click on the Review link to access the section in your e Text. Balance each of the following redox reactions occurring in acidic aqueous solution. K(s) + Cr³+ (aq) → Cr(s) + K+ (aq) Express your answer as a chemical equation including phases. ► View Available Hint(s) Submit ΑΣΦ A chemical reaction does not occur for this question. Part B ? Al(s) + Fe²+ (aq) → A1³+ (aq) + Fe(s) Express your answer as a chemical equation including phases.
Homework AX /6920146#/6920146/16/2 Macmillan Learning Web 2.0 scientific calculator Williston Forge Jero... Assignment Score: Question 17 of 21 > mass: Home Page - myAl... OO TOOLS ×10% 91.5% X + HUAWEI P30 LEICA TRIPLE CAMERA T Synonyms and Ant... Home Page - myAl.. Resources e Ex Give Up? SOAP2DAY Essayaibot: Free Ess... Hint Hydrogen gas holds promise as an alternative fuel to gasoline. Calculate the mass of H₂ gas in a 38.3 L fuel tank at a pressu 2.42 x 104 mmHg and a temperature of 17.4 °C. Paraphrasing Toof Check Answer Attempt 4 C
2. MF= C12H160 QE-300 20 200 180 160 140 120 100 80 60 40 20 2 2 3. 2 11 10 9 8 7 6 5 4 3 1
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Dashboard | myPSU M Inbox (1,777) - dmatias2@p x S Link to Modified Mastering X Course Home X A holodeck Dashboard | myPSU e CH10 X A https://openvellum.ecollege.com/course.html?courseld=170447208&OpenVellumHMAC=75234cdfe17835d8fd3833695fbb2f14#10001 A Syllabus enzyme B catalyzed enzyme A catalyzed uncatalyzed reaction Scores Pearson eText Document Sharing Submit Previous Answers User Settings Course Tools > v Correct Enzymes lower the activation energy of a chemical reaction. This means that the reaction is more likely to proceed, and results in faster formation of products. Part B Complete this vocabulary exercise relating to enzymes. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. • View Available Hint(s) Reset Help cofactor 1. A substrate binds to an enzyme at the where the reaction occurs. substrate 2. A small organic molecule necessary for the function of some enzymes…
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Provided are spectra for a compound with molecular formula CgH100 Part A) Give the degrees of unsaturation Part B) Identify the peaks that are associated with specific bonds of the structure and list the corresponding functional groups that the specific bonds belong to. Re- create the example table below that organizes this information. Use the wavenumbers that are already labeled on the spectra. Example table: wavenumber (cm-1) Corresponding Bond Type Corresponding Functional Group C(sp3)-H N-H 2978 3300 Part C) Draw the structure and clearly indicate which hydrogens correspond to which signals in the HNMR spectrum ONLY. The signals are already labeled A-D on the HNMR spectrum. Match the hydrogen labeling (HA, HB, etc.) on your drawn structure to the signal labeling provided. 4300 3320-2872 2951 3006 3003 2001 alkyl amine 1613 1510 1000
Edit View History Bookmarks. Profiles Tab Window Help ALEKS ||| ALEKS - Tiffany Te-L-Peng - L X + www-awu.aleks.com/alekscgi/x/Isl.exe/10_u-IgNslkr7j8P3jH-liGBdp5ulp5VqUnMDyPOVaX6q0CRPLZSQ5NeEtFRBekLt6yRztwY O SUBSTITUTION REACTIONS Predicting the effect of carbocation stability on the rate of... For each pair of substrates below, choose the one that will react faster in a substitution reaction, assuming that: 1. the rate law for the substitution reaction has a first-order dependence on the concentration of the alkyl halide, and 2. doesn't depend on the concentration of the other reactant at all. Substrate A age Explanation CI Check Br B Substrate B CI Faster Rate (Choose one) (Choose one) Choose one) MacBook Pro ▼ ▼ ▼ US X 3 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms
marks People Tab Window Help * 令 100% 47 linois State University : CHE 1 X * MindTap - Cengage Learning G so3 molecular geometry - Goo X i/evo/index.html?deploymentld355750828934189288909969212&elSBN=9781305657571&snapshotld=2199898&id=1.. MINDTAP nd Quick Prep Use the References to access important values if needed for this question. Orbitals which result from solving the Schrodinger Wave Equation can be represented by electron "cloud" pictures. The shapes of the orbitals are distinguished by their nodes, places where the electron density equals zero. Erwin Schrödinger Based upon the number of spherical and angular nodes, label the orbitals below as 1s, 2p, etc. Specify the value of n and I for each: This is a orbital This is a orbital This is a orbital n = and I= n = and / n and I Submit Answer 5 question attempts remaining
← Murray McKinz X M 8 Ways to Mak X с ✰ openvellum.ecollege.com/course.html?courseld=17588559&OpenVellumHMAC=ab1d8844bb4e9e48eff60bc535d90c0c#10001 Mastering Chemistry Course Home My Courses Course Home Syllabus Scores eText Document Sharing User Settings Course Tools ● 50°F Sunny In-Text Citation X Canvas at ECU X Chem 1120: Intro to Gen Chem for the Allied Health Sciences.
01-5a Match the generic formula to its generic name. CnH2n+2 [Select] CnH2n-2 [Select] C6H6 [Select] соно CnH2n [Select] <
K Haylee Scott - cp Zoom meeting lin com/web/viewer.html?state%=D%7B'ids %3A%5B"1zOflgo1GoQFrdviJ6PWx8L3h2j4uav5n"%5D%2C"action"%3A'open C Clever | Portal A Classroom https://sso.theleam. M Oro Grande Elemen. W Yearbook Aven ue Period 5 Scien. Haylee Scott - cprr061.pdf Building Vocabulary From the list below, choose the term that best completes each sentence. matter physical change endothermic reaction chemical change chemistry precipitate exothermic reaction 7. Any change that alters a substance without changing it into another substance is a(n) 8. is anything that has mass and takes up space. 9. A reaction that releases energy in the form of heat is called a(n) 10. A(n) absorbed. 11. A chemical reaction is also referred to as a(n) is a reaction in which energy is 12. A(n) a chemical reaction. is a solid formed from a solution during 13. is the study of the properties of matter and how matter changes. OPearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved…
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口 A docs.google.com Classroom | Google for Education Alchemy Lesson 20 & 21 Worksheet Andres Carrill Andres Carrillo - Alchemy Lessons 20 & 21 Worksheet Update Apple ID S Some account servi available until you sig File Edit View Insert Format Tools Add-ons Help Last edit was 2 days ago 100% Normal text Arial 11 BIUA E = E = EE E - E E X 1 2 3 4 .. 6 I 7 O 8 1 IC 5 AIV-20: Getting Connected (Writing lonic Compounds) Part 1: Putting together lonic Compounds lonic compound Metal Number of cation nonmetal number of anion total total charge = 0 valence valence number of electrons electrons valence electrons NaF, sodium fluoride Na Na + (+1)+(-1) = 0 F- 8. MgO, magnesium oxide Mg 02- (+2) + (-2) = 0 MgCl2, magnesium chloride Mg CI 7 16 (+2) + 2(-1) = 0 Ne, neon Ne 8 BeF2, beryllium fluoride Be MgS, magnesium sulfide CaCl,, calcium chloride Na Br K Se Al Al203, aluminum oxide Al Al F
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