Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
10th Edition
ISBN: 9781305957510
Author: ZUMDAHL, Steven S.; Zumdahl, Susan A.; DeCoste, Donald J.
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 15, Problem 20Q
Consider the following two acids:
pKa1 = 2.98; pKa2 = 13.40
HO2CCH2CH2CH2CH2CO2H
Adipic acid
pKa1 = 4.41; pKa2 = 5.28
In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
You are conducting a biochemical experiment with an enzyme that has optimal activity at pH = 6.50. You decide to use carbonate (pKa1 = 6.38, pKa2 = 10.30) as the buffer to keep the pH stable throughout the enzymatic reaction. (Recall that the formula for carbonic acid is H2CO3.) You prepare a 0.4 M solution of carbonate buffer at pH = 10.50. Calculate the concentrations of the major carbonate species in your solution. Show your calculations.
The concentration of Cl– in a 300.0-mL sample of water drawn from a fresh water acquifer suffering from encroachment of sea water, was determined by titrating with 0.0516 M Hg(NO3)2. The sample was acidified and titrated to the diphenylcarbazone end point, requiring 6.18 mL of the titrant. Report the concentration of Cl–in parts per million
30ml of 0.06M solution of protonated form of anion amino acid methionine (H2A+) is treated with0.09M NaOH.calculate pH after addition of 20 ml of base.pKa1=2.28 and pKa=9.2 please answer this question .with explanation
Chapter 15 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
Ch. 15 - What is meant by the presence of a common ion? How...Ch. 15 - Define a buffer solution. What makes up a buffer...Ch. 15 - One of the most challenging parts of solving...Ch. 15 - A good buffer generally contains relatively equal...Ch. 15 - Draw the general titration curve for a strong acid...Ch. 15 - Instead of the titration of a strong acid by a...Ch. 15 - Sketch the titration curve for a weak acid...Ch. 15 - Sketch the titration curve for a weak base...Ch. 15 - What is an acidbase indicator? Define the...Ch. 15 - Why does an indicator change from its acid color...
Ch. 15 - What are the major species in solution after...Ch. 15 - A friend asks the following: Consider a buffered...Ch. 15 - Mixing together solutions of acetic acid and...Ch. 15 - Sketch two pH curves, one for the titration of a...Ch. 15 - Sketch a pH curve for the titration of a weak acid...Ch. 15 - You have a solution of the weak acid HA and add...Ch. 15 - You have a solution of the weak acid HA and add...Ch. 15 - The common ion effect for weak acids is to...Ch. 15 - Prob. 12QCh. 15 - A best buffer has about equal quantities of weak...Ch. 15 - Consider the following pH curves for 100.0 mL of...Ch. 15 - An acid is titrated with NaOH. The following...Ch. 15 - Consider the following four titrations. i. 100.0...Ch. 15 - Figure 14-4 shows the pH curves for the titrations...Ch. 15 - Acidbase indicators mark the end point of...Ch. 15 - Consider the titration of 100.0 mL of 0.10 M...Ch. 15 - Consider the following two acids: pKa1 = 2.98;...Ch. 15 - How many of the following are buffered solutions?...Ch. 15 - Which of the following can be classified as buffer...Ch. 15 - A certain buffer is made by dissolving NaHCO3 and...Ch. 15 - A buffer is prepared by dissolving HONH2 and...Ch. 15 - Calculate the pH of each of the following...Ch. 15 - Calculate the pH of each of the following...Ch. 15 - Compare the percent dissociation of the acid in...Ch. 15 - Compare the percent ionization of the base in...Ch. 15 - Calculate the pH after 0.020 mole of HCl is added...Ch. 15 - Calculate the pH after 0.020 mole of HCl is added...Ch. 15 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 15 - Calculate the pH after 0.020 mole of NaOH is added...Ch. 15 - Which of the solutions in Exercise 21 shows the...Ch. 15 - Prob. 34ECh. 15 - Calculate the pH of a solution that is 1.00 M HNO2...Ch. 15 - Calculate the pH of a solution that is 0.60 M HF...Ch. 15 - Calculate the pH after 0.10 mole of NaOH is added...Ch. 15 - Calculate the pH after 0.10 mole of NaOH is added...Ch. 15 - Calculate the pH of each of the following buffered...Ch. 15 - Calculate the pH of each of the following buffered...Ch. 15 - Calculate the pH of a buffered solution prepared...Ch. 15 - A buffered solution is made by adding 50.0 g NH4Cl...Ch. 15 - Calculate the pH after 0.010 mole of gaseous HCl...Ch. 15 - Calculate the pH after 0.15 mole of solid NaOH is...Ch. 15 - Some K2SO3 and KHSO3 are dissolved in 250.0 mL of...Ch. 15 - An aqueous solution contains dissolved C6H5NH3Cl...Ch. 15 - Calculate the mass of sodium acetate that must be...Ch. 15 - What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must...Ch. 15 - Consider a solution that contains both C5H5N and...Ch. 15 - Calculate the ratio [NH3]/[NH4+] in...Ch. 15 - Carbonate buffers are important in regulating the...Ch. 15 - When a person exercises, muscle contractions...Ch. 15 - Consider the acids in Table 13-2. Which acid would...Ch. 15 - Consider the bases in Table 13-3. Which base would...Ch. 15 - Calculate the pH of a solution that is 0.40 M...Ch. 15 - Calculate the pH of a solution that is 0.20 M HOCl...Ch. 15 - Which of the following mixtures would result in...Ch. 15 - Which of the following mixtures would result in a...Ch. 15 - What quantity (moles) of NaOH must be added to 1.0...Ch. 15 - Calculate the number of moles of HCl(g) that must...Ch. 15 - Consider the titration of a generic weak acid HA...Ch. 15 - Sketch the titration curve for the titration of a...Ch. 15 - Consider the titration of 40.0 mL of 0.200 M HClO4...Ch. 15 - Consider the titration of 80.0 mL of 0.100 M...Ch. 15 - Consider the titration of 100.0 mL of 0.200 M...Ch. 15 - Consider the titration of 100.0 mL of 0.100 M...Ch. 15 - Lactic acid is a common by-product of cellular...Ch. 15 - Repeat the procedure in Exercise 61, but for the...Ch. 15 - Repeat the procedure in Exercise 61, but for the...Ch. 15 - Repeat the procedure in Exercise 61, but for the...Ch. 15 - Calculate the pH at the halfway point and at the...Ch. 15 - In the titration of 50.0 mL of 1.0 M methylamine,...Ch. 15 - You have 75.0 mL of 0.10 M HA. After adding 30.0...Ch. 15 - A student dissolves 0.0100 mole of an unknown weak...Ch. 15 - Two drops of indicator HIn (Ka = 1.0 109), where...Ch. 15 - Methyl red has the following structure: It...Ch. 15 - Potassium hydrogen phthalate, known as KHP (molar...Ch. 15 - A certain indicator HIn has a pKa of 3.00 and a...Ch. 15 - Which of the indicators in Fig. 14-8 could be used...Ch. 15 - Prob. 80ECh. 15 - Which of the indicators in Fig. 14-8 could be used...Ch. 15 - Prob. 82ECh. 15 - Estimate the pH of a solution in which bromcresol...Ch. 15 - Estimate the pH of a solution in which crystal...Ch. 15 - A solution has a pH of 7.0. What would be the...Ch. 15 - A solution has a pH of 4.5. What would be the...Ch. 15 - When a diprotic acid, H2A. is titrated with NaOH,...Ch. 15 - Consider die titration of 50.0 mL of 0.10 M H3A...Ch. 15 - Derive an equation analogous to the...Ch. 15 - a. Calculate the pH of a buffered solution that is...Ch. 15 - Tris(hydroxymethyl)aminomethane, commonly called...Ch. 15 - You make 1.00 L of a buffered solution (pH = 4.00)...Ch. 15 - You have the following reagents on hand: Solids...Ch. 15 - Prob. 94AECh. 15 - Phosphate buffers are important in regulating the...Ch. 15 - When a diprotic acid, H2A, is titrated with NaOH,...Ch. 15 - Consider the blood buffer system discussed in the...Ch. 15 - What quantity (moles) of HCl(g) must be added to...Ch. 15 - Prob. 99AECh. 15 - The following plot shows the pH curves for the...Ch. 15 - Calculate the volume of 1.50 102 M NaOH that must...Ch. 15 - Prob. 102AECh. 15 - A certain acetic acid solution has pH = 2.68....Ch. 15 - A 0.210-g sample of an acid (molar mass = 192...Ch. 15 - The active ingredient in aspirin is...Ch. 15 - One method for determining the purity of aspirin...Ch. 15 - A student intends to titrate a solution of a weak...Ch. 15 - A student titrates an unknown weak acid, HA, to a...Ch. 15 - A sample of a certain monoprotic weak acid was...Ch. 15 - The pigment cyanidin aglycone is one of the...Ch. 15 - Consider 1.0 L of a solution that is 0.85 M HOC6H5...Ch. 15 - What concentration of NH4Cl is necessary to buffer...Ch. 15 - Consider the following acids and bases: HCO2H Ka =...Ch. 15 - Consider a buffered solution containing CH3NH3Cl...Ch. 15 - Consider the titration of 150.0 mL of 0.100 M HI...Ch. 15 - Consider the titration of 100.0 mL of 0.100 M HCN...Ch. 15 - Consider the titration of 100.0 mL of 0.200 M...Ch. 15 - Consider the following four titrations (iiv): i....Ch. 15 - Another way to treat data from a pH titration is...Ch. 15 - A buffer is made using 45.0 mL of 0.750 M HC3H5O2...Ch. 15 - A 0.400-M solution of ammonia was titrated with...Ch. 15 - What volume of 0.0100 M NaOH must be added to 1.00...Ch. 15 - Consider a solution formed by mixing 50.0 mL of...Ch. 15 - Cacodylic acid, (CH3)2AsO2H, is a toxic compound...Ch. 15 - The titration of Na2CO3 with HCl bas the following...Ch. 15 - Consider the titration curve in Exercise 115 for...Ch. 15 - A few drops of each of the indicators shown in the...Ch. 15 - Malonic acid (HO2CCH2CO2H) is a diprotic acid. In...Ch. 15 - A buffer solution is prepared by mixing 75.0 mL of...Ch. 15 - A 10.00-g sample of the ionic compound NaA, where...Ch. 15 - Calculate the pH of a solution prepared by mixing...Ch. 15 - Consider a solution prepared by mixing the...
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
- Strong base is dissolved in 615 mL of 0.200 M weak acid (Ka = 3.46 x 10-5) to make a buffer with a pH of 3.97. Assume that the volume remains constant when the base is added. HA(aq) + OH(aq) → H₂O(l) + A¯(aq) Calculate the pKa value of the acid, and determine the number of moles of acid initially present. pK₁ = initial amount: mol HA When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A-] [HA] How many moles of strong base were initially added? amount added: O III 66°F O 1) mol OH J 5:55 PM 6/2/2022arrow_forwardAn analytical chemist is titrating 50.2 mL of a 0.5100M solution of trimethylamine ((CH3)N) with a 0.7400M solution of HNO3. The pk of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 38.0 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = Xarrow_forwardAn analytical chemist is titrating 236.4 mL of a 0.3500M solution of trimethylamine ((CH₂)₂N) with a 0.2300M solution of HNO3. The pK₂ of 3 trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 77.8 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X Śarrow_forward
- For an acid HA with a pKa of 5.2, what is the ratio of the concentration of the conjugate base to that of the acid at pH 7.2.arrow_forwardAscorbic acid, H2C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pKa1 is 4.10 and pKa2 is 11.79. When 125 mL of a solution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 3.64 g. Your answer is correct. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. 0.164 Hint Your answer is partially correct. What was the pH of the ascorbic acid solution before it was evaporated? pH = 2.44 What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i M Marrow_forward8. Calculate the pH and Ka for HC₂H3O2 if in a 1.0000 M solution of HC₂H3O2 in water there is 0.99600 M HC2H3O2. Use stoichiometry. (answers are pH = 2.398 and Ka 1.60 x 10-5) H3O+1 HC₂H3O2 + H₂O C₂H30₂¹ + 1.00000 M start: 0 0 equil: 0.99600 M 0.00400 Marrow_forward
- Sodium phosphate has 3 ionizable groups, with pKa’s of 2.2, 7.2, and 12.3. You have 250 mL of a 200 mM sodium phosphate solution at pH 6.8. You add 2.0 mL of 5.0 M sodium hydroxide to the solution. What’s the new pH?arrow_forwardCalculate the volume, in liters, of 1.681 M KOH that must be added to a 0.117 L solution containing 9.98 g of glutamic acid hydrochloride (H₂Glu+Cl¯, MW = 183.59 g/mol) to achieve a pH of 10.18. Glutamic acid (Glu) is an amino acid with pKa values of pKal = 2.23, pK₁2 = 4.42, and PK₂3 = 9.95. volume: L NH, CÌ HC-CH₂-CH₂-C-OH C= O OH Glutamic Acid Hydrochloridearrow_forwardDraw a titration curve for the amino acid lysine at the pKa's of 2.2, 9.0, and 10.0 for the ionizable groups of lysine. Label the buffering regions and equivalence points. Draw the structures for the primary species of lysine at all the buffering regions and equivalence points you include in your graph.arrow_forward
- Consider the titration of 50.00 ml of a solution of 0.2574 M of the fully protonated form of the diprotic amino acid glycine (pKa1 = 2.34, pKa2 = 9.60) with 0.3786 M KOH. What is the pH after the addition of 33.99 mL of the KOH solution?arrow_forwardA solution contains NaHCO3, Na2CO3, and NaOH, either alone or in permissible combination. Titration of a 40.0-mL portion to a phenolphthalein end point requires 24.1 mL of 0.100 M HCl. A second 40.0-mL aliquot requires 48.4 mL of the HCl when titrated to a bromocresol green end point. Deduce the composition and calculate the molar solute conc. of the original solutionarrow_forwardCalculate the Ka and Kb values for 1.0 M NaHSO4 and Na2CO3.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Acid-base Theories and Conjugate Acid-base Pairs; Author: Mindset;https://www.youtube.com/watch?v=hQLWYmAFo3E;License: Standard YouTube License, CC-BY
COMPLEXOMETRIC TITRATION; Author: Pikai Pharmacy;https://www.youtube.com/watch?v=EQxvY6a42Dw;License: Standard Youtube License