CHEMISTRY THE CENTRAL SCIENCE >EBOOK<
14th Edition
ISBN: 9780136873891
Author: Brown
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 4, Problem 83E
Some sulfuric acid is spilled on a lab bench You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to 2 NaHCO3(s) + H2SO4(aq) Na2SO4(aq) + 2 H2O(l) + 2 CO2(g)
Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
When HCl(aq) is added to calclum carbonate solid, carbon dioxide gas, liquid water and aqueous calcium chloride form: Caco,(s) + 2HCI(aq) - CO,lg) • CaCl, faq) + H,00) This reaction is used by geologists to confirm the presence of limestone (calcium carbonate) in minerals. In this experiment you are trying to determine the effect of concentration of HCI(aq) on the production of carbon dioxide. a. Based upon the information above, come up with a question to answer. (C:1) You can use the following equipment to answer this question: calcium carbonate chips, 1.90 molL HClaq). pH meter (measures hydrogen ion concentration), beaker, timer, apparatus to measure gas produced b. Based upon the equipment provided above, design a procedure to answer your question. Ensure you provide numbered steps. (1:3, C:2) c. Hypothesize an answer to your question. (I:1) Give reasons for your hypothesis. Ensure you are very specific. (A3) From your experiment, you collect the following data: Reactant…
One mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form b) AgCl precipitate will form c) NaNO3 precipitate will form d) both AgCl and NaNO3 precipitates will form
30. The following reaction takes place. A,B(s) = 2A(ac) + B(ag) + heat. If 1.80 moles of A,B is added into a 1.00
L container, it is found that 30.0% of the reactant dissociates to reach equilibrium. Find the solubility
product constant, Ksp, for this reaction. Note: Your answer must include an ICE table.
(aq),
Chapter 4 Solutions
CHEMISTRY THE CENTRAL SCIENCE >EBOOK<
Ch. 4.1 - If you have an aqueous solution that contains 1.5...Ch. 4.1 - If you were to draw diagrams representing aqueous...Ch. 4.2 - Prob. 4.2.1PECh. 4.2 - Classify the following compounds as soluble or...Ch. 4.2 - Yes or No: Will a precipitate form when solutions...Ch. 4.2 - a. What compound precipitates when aqueous...Ch. 4.2 - What happens when you mix an aqueous solution of...Ch. 4.2 -
Write the net ionic equation for the...Ch. 4.3 - Prob. 4.5.1PECh. 4.3 -
Imagine a diagram showing 10 Na + ions and 10 OH-...
Ch. 4.3 -
Which of these substances, when dissolved in...Ch. 4.3 - Consider solutions in which 0.1 mol of each of the...Ch. 4.3 -
Which is the correct ionic equation for the...Ch. 4.3 - For the reaction of phosphorous acid (H3PO3) and...Ch. 4.4 - Prob. 4.8.1PECh. 4.4 - What is the oxidation state of the boldfaced...Ch. 4.4 - Which of the following statements is true about...Ch. 4.4 - Prob. 4.9.2PECh. 4.4 - Which of these metals is the easiest to oxidize?...Ch. 4.4 - Which of the following metals will be oxidized by...Ch. 4.5 - Prob. 4.11.1PECh. 4.5 - Calculate the molarity of a solution made by...Ch. 4.5 - Prob. 4.12.1PECh. 4.5 - What is the molar concentration of K+ions in a...Ch. 4.5 - Prob. 4.13.1PECh. 4.5 -
How many grams of Na2SO4 are there in 15 mL of...Ch. 4.5 - Prob. 4.14.1PECh. 4.5 - What volume of 2.50 M lead(II) nitrate solution...Ch. 4.6 - How many milligrams of sodium sulfide are needed...Ch. 4.6 -
How many grams of NaOH are needed to neutralize...Ch. 4.6 - Prob. 4.16.1PECh. 4.6 - Prob. 4.16.2PECh. 4.6 - Practice Exercise 1 A mysterious white powder is...Ch. 4.6 - Prob. 4.17.2PECh. 4 - Prob. 1DECh. 4 - Prob. 1ECh. 4 - Aqueous solutions of three different substances,...Ch. 4 -
4 3 Use the molecular representations shown here...Ch. 4 - The concept of chemical equilibrium is very...Ch. 4 -
4 5 You are presented with a white solid and told...Ch. 4 - Which of the following ions will always be a...Ch. 4 - The labels have fallen off three bottles...Ch. 4 - Explain how a redox reaction involves electrons in...Ch. 4 - Prob. 9ECh. 4 - Prob. 10ECh. 4 -
4.11 Which data set, of the two graphed here,...Ch. 4 - You are titrating an acidic solution with a basic...Ch. 4 - State whether each of the following statements is...Ch. 4 - State whether each of the following statements is...Ch. 4 -
4.15 We have learned in this chapter that many...Ch. 4 - Prob. 16ECh. 4 -
4.17 Specify what ions are present in solution...Ch. 4 - Prob. 18ECh. 4 - Prob. 19ECh. 4 - Acetone. CH3COCH3, is a nonelectrolyte;...Ch. 4 -
4.21 Using solubility guidelines, predict whether...Ch. 4 - Prob. 22ECh. 4 - Prob. 23ECh. 4 - Prob. 24ECh. 4 - Which ions remain in solution, unreacted, after...Ch. 4 - Write balanced net ionic equations for the...Ch. 4 -
4.27 Separate samples of a solution of an unknown...Ch. 4 - Prob. 28ECh. 4 - Prob. 29ECh. 4 - Prob. 30ECh. 4 - Prob. 31ECh. 4 - Prob. 32ECh. 4 - State whether each of the following statements is...Ch. 4 - State whether each of the following statements is...Ch. 4 -
4.35 Label each of the following substances as an...Ch. 4 - An aqueous solution of an unknown solute is tested...Ch. 4 - Prob. 37ECh. 4 - Classify each of the following aqueous solutions...Ch. 4 - Complete and balance the following molecular...Ch. 4 - Write the balanced molecular and net ionic...Ch. 4 - Write balanced molecular and net ionic equations...Ch. 4 -
4.42 Because the oxide ion is basic, metal oxides...Ch. 4 -
4.43 Magnesium carbonate, magnesium oxide, and...Ch. 4 -
4.44 As K20 dissolves in water, the oxide ion...Ch. 4 - True or false: If a substance is oxidized, it is...Ch. 4 - Prob. 46ECh. 4 - Which region of the periodic table shown here...Ch. 4 - Determine the oxidation number of sulfur in each...Ch. 4 - Determine the oxidation number for the indicated...Ch. 4 - Determine the oxidation number for the indicated...Ch. 4 - Which element is oxidized, and which is reduced in...Ch. 4 - Which of the following are redox reactions? For...Ch. 4 -
4.53 Write balanced molecular and net ionic...Ch. 4 - Write balanced molecular and net ionic equations...Ch. 4 - Using the activity series (Table 4.5), write...Ch. 4 - Using the activity series (Table 4.5), write...Ch. 4 - The metal cadmium tends to form Cd2+ ions. The...Ch. 4 -
4.58 The following reactions (note that the...Ch. 4 - Is the concentration of a solution an intensive or...Ch. 4 - Prob. 60ECh. 4 - Calculate the molarity of a solution that contains...Ch. 4 -
4.62
Calculate the molarity of a solution made by...Ch. 4 - Prob. 63ECh. 4 - Prob. 64ECh. 4 - Prob. 65ECh. 4 -
4.66 The average adult male has a total blood...Ch. 4 -
4.67
How many grams of ethanol, CH2CH2OH should...Ch. 4 - Prob. 68ECh. 4 - Which will have the highest concentration of...Ch. 4 - Prob. 70ECh. 4 - Prob. 71ECh. 4 - Prob. 72ECh. 4 - Prob. 73ECh. 4 - Prob. 74ECh. 4 - Prob. 75ECh. 4 - Prob. 76ECh. 4 - Prob. 77ECh. 4 - Prob. 78ECh. 4 - Prob. 79ECh. 4 - Prob. 80ECh. 4 - Prob. 81ECh. 4 - Prob. 82ECh. 4 - Some sulfuric acid is spilled on a lab bench You...Ch. 4 -
4.84 The distinctive odor of vinegar is due to...Ch. 4 - A 4.36-g sample of an unknown alkali metal...Ch. 4 -
4.86 An 8.65-g sample of an unknown group 2A...Ch. 4 - A solution of 100.0 mL of 0.200 M KOH is mixed...Ch. 4 -
4.88 A solution is made by mixing 15.0 g of...Ch. 4 - Prob. 89ECh. 4 - A 1.248-9 sample of limestone rock is pulverized...Ch. 4 - 4.91 Uranium hexafluoride, UF6, is processed to...Ch. 4 - The accompanying photo shows the reaction between...Ch. 4 - Prob. 93AECh. 4 -
4.94 You choose to investigate some of the...Ch. 4 -
4 95 Antacids are often used to relieve pain and...Ch. 4 -
4 96 The commercial production of nitric acid...Ch. 4 - Consider the following reagents: zinc, copper,...Ch. 4 - 98 Bronze is a solid solution of Cu(s) and Sn(s);...Ch. 4 - Prob. 99AECh. 4 - Prob. 100AECh. 4 -
4.101 Hard water contains Ca2+ , Mg2 + , and Fe2+...Ch. 4 - Tartaric acid. H2C4H4O6, has two acidic hydrogens....Ch. 4 - Prob. 103AECh. 4 - A solid sample of Zn(OH)2 is added to 0.350 L of...Ch. 4 - Prob. 105IECh. 4 - Prob. 106IECh. 4 - Prob. 107IECh. 4 - A fertilizer railroad car carrying 34,300 gallons...Ch. 4 - Prob. 109IECh. 4 - Prob. 110IECh. 4 - Prob. 111IECh. 4 - Prob. 112IECh. 4 - Prob. 113IECh. 4 - Prob. 114IECh. 4 -
4.115 Federal regulations set an upper limit of...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Describe a nonchemical system that is not in equilibrium, and explain why equilibrium has not been achieved.arrow_forwardConsider a metal ion A2+ and its nitrate salt, In an experiment, 35.00 mL of a 0.217 M solution of A(NO3)2 is made to react with 25.00 mL of 0.195 M NaOH. A precipitate, A(OH)2, forms. Along with the precipitation, the temperature increases from 24.8C to 28.2C. What is H for the precipitation of A(OH)2? The following assumptions can be made. • The density of the solution is 1.00 g/mL. • Volumes are additive. • The specific heat of the solution is 4.18 J/g C.arrow_forwardSilver undergoes similar reactions as those shown for gold. Both metals react with cyanide ion in the presence of oxygen to form soluble complexes, and both are reduced by zinc. The reaction of Ag+ with cyanide ion may be viewed as two sequential steps: (1) Ag+(aq)+CN(aq)AgCN(s) (2) AgCN(s)+CN(aq)[Ag(CN)2](aq)Ag+(aq)+2CN(aq)[Ag(CN)2](aq)Kf=1.31021 a. Use the solubility product equilibrium constant (Appendix J) of AgCN(s) to determine the equilibrium constant for Step 1. b. Use the equilibrium constants from Step 1 and the overall reaction to determine the equilibrium constant for Step 2. c. Excess AgCN(s) is combined with 1.0 L of 0.0071 M CN (aq) and allowed to equilibrate. Calculate the equilibrium concentrations of CN and [Ag(CN)2] using the equilibrium constant for Step 2. Assume no change in volume occurs.arrow_forward
- Write the expression of the reaction quotient for the ionization of HOCN in water.arrow_forwardUse the solubility product constant from Appendix F to determine whether a precipitate will form if 10.0 mL of 1.0 106 M iron(II) chloride is added to 20.0 mL of 3.0 104 M barium hydroxide.arrow_forwardThe ore cinnabar (HgS) is an important source of mercury. Cinnabar is a red solid whose solubility in water is 5.5 X 10-2 mol L-1. Calculate its \p. What is its solubility' in grams per 100 g of water?arrow_forward
- Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25Carrow_forwardGiven that the Gf for Pb2+(aq) and Cl-(aq) is -24.3 kJ/mole and -131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).arrow_forwardMagnesite (magnesium carbonate, MgCO3) is a common magnesium mineral. From the solubility product constant, find the solubility of magnesium carbonate in grams per liter of water.arrow_forward
- 12.67 Hydrofluoric acid is a weak acid used in the building industry to etch patterns into glass for elegant windows. Because it dissolves glass, it is the only inorganic acid that must be stored in plastic containers. A 0.1 M solution of HF has a pH of 2.1. Calculate [Hj0"| in this solution.arrow_forwardGiven the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.arrow_forwardThe following is a thought experiment. Imagine that you put a little water in a test tube and add some NaF crystals. Immediately after you add NaF, you observe that the crystals begin dissolving. The quantity of solid NaF decreases, hut before long, it appears that no more NaF is dissolving. The solution is saturated. The equation for the dissolution of NaF in water is NaF(s) —* Na (aq) + F~(aq). As NaF dissolves, what do you think happens to the rate of dissolution? Describe w hat is occurring on the molecular level. Assume that the reverse reaction, Na+(aq) + F“(aq) —* NaF(s), also occurs as the crystal dissolves. In other words, both dissolution and precipitation are taking place. When it appears that there is no more change in the quantin’ of NaF dissolving (the solution is saturated), w hat has happened to the rates of the forward and reverse reactions? Explain your answer.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Acid-Base Equilibrium; Author: Bozeman Science;https://www.youtube.com/watch?v=l5fk7HPmo5g;License: Standard YouTube License, CC-BY
Introduction to Titrimetric analysis; Author: Vidya-mitra;https://www.youtube.com/watch?v=uykGVfn9q24;License: Standard Youtube License