Explanation Given The concentration of each of the solution of HCOOH, CH 3 COOH, HCN, HCOONa, CH 3 COONa, and NaCN is 0.10 M . Three acids are available, HCOOH, CH 3 COOH and HCN . The acid dissociation constant ( K a ) of HCOOH is 1.8 × 10 − 4 (refer Appendix D from the textbook). The acid dissociation constant ( K a ) of CH 3 COOH is 1.8 × 10 − 5 (refer Appendix D from the textbook). The acid dissociation constant ( K a ) of HCN is 6.2 × 10 − 10 (refer Appendix D from the textbook). The p K a of HCOOH is calculated by the formula, p K a = − log ( K a ) Substitute the value of K a in the above formula. p K a = − log ( 1.8 × 10 − 4 ) = 3.75 The p K a of CH 3 COOH is calculated by the formula, p K a = − log ( K a ) Substitute the value of K a in the above formula. p K a = − log ( 1.8 × 10 − 5 ) = 4.75 The p K a of HCN is calculated by the formula, p K a = − log ( K a ) Substitute the value of K a in the above formula. p K a = − log ( 6.2 × 10 − 10 ) = 9.3 According to Henderson-Hasselbalch equation, pH = p K a + log [ Base ] [ Acid ] Here, [ Base ] is the concentration of the conjugate base. [ Acid ] is the concentration of the weak acid. Therefore, if the concentration of the conjugate base and the concentration of the weak acid is equal, pH becomes equal to p K a . The pH of the buffer should be 5.00 . Therefore, the value of p K a should be close to 5.00 . The p K a of CH 3 COOH is 4.75 , that is the closest value to 5.00 . Therefore, acetic acid is suitable to prepare the buffer solution of pH 5.00 . The reaction equilibrium of acetic acid is, CH 3 COOH ( a q ) ⇌ H + ( a q ) + CH 3 COO − ( a q ) The change in the concentration of CH 3 COOH is assumed to be x . The initial and the equilibrium concentrations of the species involved in the above reaction, CH 3 COOH ( a q ) ⇌ H + ( a q ) + CH 3 COO − ( a q ) Initial : 0

Chemistry the Central Science 13th Edition Custom for Lamar University

13th Edition

ISBN: 9781269962667

Author: Theodore L. Brown, H. Eugene LeMay Jr., Bruce E. Bursten, Batherine J. Murphy, Patrick M. Woodward, Matthew W. Stoltzfus

Publisher: Pearson Learning Center

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Chapter 3, Problem 19E

Interpretation Introduction

To determine: The solutions required and their correct volume to prepare approximately 1 L of a buffer solution of pH 5.00 .

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Chapter 3, Problem 18E

Chapter 3, Problem 20E

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Chapter 3 Solutions

Chemistry the Central Science 13th Edition Custom for Lamar University

Ch. 3.1 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 3.1 - Prob. 3.1.2PE Ch. 3.1 - Consider a saturated solution of the salt MA3, in...Ch. 3.1 - Prob. 3.2.2PE Ch. 3.2 - Prob. 3.3.1PE Ch. 3.2 - Prob. 3.3.2PE Ch. 3.2 - Prob. 3.4.1PE Ch. 3.2 - Prob. 3.4.2PE Ch. 3.3 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 3.3 - Does a precipitate form when 0.050 L of 2.0 × 10-2...

Ch. 3.3 - Under what conditions does an ionic compound...Ch. 3.3 - Prob. 3.6.2PE Ch. 3.4 - Prob. 3.7.1PE Ch. 3.4 - The following boxes represent aqueos solutions...Ch. 3.4 - Prob. 3.8.1PE Ch. 3.4 - Prob. 3.8.2PE Ch. 3.4 - Prob. 3.9.1PE Ch. 3.4 - Prob. 3.9.2PE Ch. 3.4 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 3.4 - Practice Exercise 2 Calculate the pH of a solution...Ch. 3.4 - Calculate the concentration of the lactate ion in...Ch. 3.4 - Practice Exercise 2 Calculate the format ion...Ch. 3.4 - Practice Exercise 1 If the pH of a buffer solution...Ch. 3.4 - Prob. 3.12.2PE Ch. 3.5 - Prob. 3.13.1PE Ch. 3.5 - Prob. 3.13.2PE Ch. 3.5 - Calculate the number of grams of ammonium chloride...Ch. 3.5 - Prob. 3.14.2PE Ch. 3.5 - Prob. 3.15.1PE Ch. 3.5 - Determine The pH of the original buffer described...Ch. 3.6 - An acid-base titration is performed: 250.0 mL of...Ch. 3.6 - Prob. 3.16.2PE Ch. 3.6 - Prob. 3.17.1PE Ch. 3.6 - Calculate the pH in the solution formed by adding...Ch. 3.7 - Prob. 3.18.1PE Ch. 3.7 - Prob. 3.18.2PE Ch. 3.7 - Prob. 3.19.1PE Ch. 3.7 - Prob. 3.19.2PE Ch. 3.7 - Prob. 3.20.1PE Ch. 3.7 - Prob. 3.20.2PE Ch. 3 - The accompanying graph shows the titration curves...Ch. 3 - Prob. 2E Ch. 3 - Prob. 3E Ch. 3 - Prob. 4E Ch. 3 - Prob. 5E Ch. 3 - Prob. 6E Ch. 3 - Prob. 7E Ch. 3 - Prob. 8E Ch. 3 - Prob. 9E Ch. 3 - Use information from Appendix D to calculate the...Ch. 3 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 3 - You are asked to prepare a pH = 3.00 buffer...Ch. 3 - You are asked to prepare an pH = 4.00 buffer...Ch. 3 - Prob. 14E Ch. 3 - Prob. 15E Ch. 3 - Prob. 16E Ch. 3 - Prob. 17E Ch. 3 - Prob. 18E Ch. 3 - Prob. 19E Ch. 3 - Prob. 20E Ch. 3 - 17.35 The samples of nitric and acetic acids shows...Ch. 3 - 17.36 Determine whether each of the following...Ch. 3 - Prob. 23E Ch. 3 - Prob. 24E Ch. 3 - Prob. 25E Ch. 3 - Assume that 30.0 mL of a M solution of a week base...Ch. 3 - Prob. 27E Ch. 3 - Prob. 28E Ch. 3 - Prob. 29E Ch. 3 - Prob. 30E Ch. 3 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 3 - Prob. 32E Ch. 3 - Prob. 33E Ch. 3 - Prob. 34E Ch. 3 - The solubility of two slighty soluble salts of...Ch. 3 - Prob. 36E Ch. 3 - 17.52 a. true or false: solubility and...Ch. 3 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 3 - Prob. 39E Ch. 3 - Prob. 40E Ch. 3 - using calculate the molar solubility of AgBr in a....Ch. 3 - calculate the solubility of LaF3 in grams per...Ch. 3 - Prob. 43E Ch. 3 - Consider a beaker containing a saturated solution...Ch. 3 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 3 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 3 - 17.63 Which of the following salts will be...Ch. 3 - For each of the following slightly soluble salts,...Ch. 3 - Prob. 49E Ch. 3 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 3 - Prob. 51E Ch. 3 - Prob. 52E Ch. 3 - Prob. 53E Ch. 3 - Calculate the minimum pH needed to precipitate Mn...Ch. 3 - Prob. 55E Ch. 3 - Prob. 56E Ch. 3 - Prob. 57E Ch. 3 - Prob. 58E Ch. 3 - Prob. 59E Ch. 3 - An unknown solid is entirely soluble in water. On...Ch. 3 - Prob. 61E Ch. 3 - Prob. 62E Ch. 3 - 17.81 Precipitation of the group 4 cautions of...Ch. 3 - Prob. 64E Ch. 3 - Prob. 65E Ch. 3 - Prob. 66E Ch. 3 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 3 - Prob. 68E Ch. 3 - Equal quantities of 0.010 M solution of an acid HA...Ch. 3 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 3 - (a) Define the terms limiting reactant and excess...Ch. 3 - Prob. 72E Ch. 3 - Prob. 73E Ch. 3 - Prob. 74E Ch. 3 - What is the pH of a solution made by mixing 0.30...Ch. 3 - Suppose you want to do a physiological experiment...Ch. 3 - Prob. 77E Ch. 3 - Prob. 78E Ch. 3 - For each pair of compounds, use Kap values to...Ch. 3 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 3 - Salts containing the phosphate ion are added to...Ch. 3 - Prob. 82E Ch. 3 - 17.103 The solubility –product constant for barium...Ch. 3 - Prob. 84E Ch. 3 - Prob. 85E Ch. 3 - A buffer of what pH is needed to give a Mg2+...Ch. 3 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 3 - Prob. 88AE Ch. 3 - Prob. 89AE Ch. 3 - Prob. 90AE Ch. 3 - Prob. 91AE Ch. 3 - Prob. 92AE Ch. 3 - Prob. 93AE Ch. 3 - Prob. 94AE Ch. 3 - Prob. 95AE Ch. 3 - A concentration of 10-100 parts per billion (by...Ch. 3 - Prob. 97AE Ch. 3 - Prob. 98AE Ch. 3 - In nonaqueous solvents, it is possible to react HF...Ch. 3 - Prob. 100AE Ch. 3 - Prob. 101AE Ch. 3 - Prob. 102AE Ch. 3 - 17.9 The following graphs represent the behavior...Ch. 3 - Prob. 104AE Ch. 3 - 17.11 The graph below shows the solubility of a...Ch. 3 - Prob. 106IE Ch. 3 - Prob. 107IE Ch. 3 - (a) If an automobile travels 225 mi with a gas...Ch. 3 - Prob. 109IE Ch. 3 - Prob. 110IE Ch. 3 - Hydrogen cyanide, HCN, is a poisonous gas. The...Ch. 3 - Prob. 112IE

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