Explanation In a weak acid-strong base titration , before reaching the equivalence point the addition of strong base keeps on neutralizing the acid that results in the formation of conjugate base of the weak acid. The graph of titration between a weak acid and strong base gives an idea about their concentrations. In the graph, at halfway to the equivalence point when half of the weak acid has been neutralized, the concentration of the weak acid and its conjugate base becomes equal and this is represented as, [ Base ] = [ Acid ] Where, [ Base ] is the concentration of the conjugate base of the weak acid. [ Acid ] is the concentration of the weak acid. The pH of the solution at that point is calculated by the formula, pH = p K a + log [ Base ]<

Chemistry: The Central Science Plus Mastering Chemistry with Pearson eText -- Access Card Package (14th Edition)

14th Edition

ISBN: 9780134292816

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Matthew E. Stoltzfus

Publisher: PEARSON

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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Chapter 17, Problem 92AE

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To determine: A mathematical proof for the fact that the pH at the halfway point of a titration of a weak acid with a strong base is equal to pKa of the acid.

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Chapter 17, Problem 91AE

Chapter 17, Problem 93AE

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Chapter 17 Solutions

Chemistry: The Central Science Plus Mastering Chemistry with Pearson eText -- Access Card Package (14th Edition)

Ch. 17.1 - For the generic equilibrium HA(aq)H+(aq)+A(aq) ,...Ch. 17.1 - Practice Exercise 2 Calculate the pH of a solution...Ch. 17.1 - Calculate the concentration of the lactate ion in...Ch. 17.1 - Practice Exercise 2 Calculate the format ion...Ch. 17.2 - Practice Exercise 1 If the pH of a buffer solution...Ch. 17.2 - Prob. 17.3.2PE Ch. 17.2 - Prob. 17.4.1PE Ch. 17.2 - Prob. 17.4.2PE Ch. 17.2 - Calculate the number of grams of ammonium chloride...Ch. 17.2 - Prob. 17.5.2PE

Ch. 17.2 - Prob. 17.6.1PE Ch. 17.2 - Determine The pH of the original buffer described...Ch. 17.3 - An acid-base titration is performed: 250.0 mL of...Ch. 17.3 - Prob. 17.7.2PE Ch. 17.3 - Prob. 17.8.1PE Ch. 17.3 - Calculate the pH in the solution formed by adding...Ch. 17.3 - Prob. 17.9.1PE Ch. 17.3 - Prob. 17.9.2PE Ch. 17.4 - Which of these expressions correctly expresses the...Ch. 17.4 - Prob. 17.10.2PE Ch. 17.4 - You add 10.0 grams of solid copper(II) phosphate,...Ch. 17.4 - Prob. 17.11.2PE Ch. 17.4 - Prob. 17.12.1PE Ch. 17.4 - Prob. 17.12.2PE Ch. 17.5 - Consider a saturated solution of the salt MA3, in...Ch. 17.5 - Prob. 17.13.2PE Ch. 17.5 - Prob. 17.14.1PE Ch. 17.5 - Prob. 17.14.2PE Ch. 17.5 - Prob. 17.15.1PE Ch. 17.5 - Prob. 17.15.2PE Ch. 17.6 - An insoluble salt MA has a Kap of 1.0 × 10-10. Two...Ch. 17.6 - Does a precipitate form when 0.050 L of 2.0 × 10-2...Ch. 17.6 - Under what conditions does an ionic compound...Ch. 17.6 - Prob. 17.17.2PE Ch. 17 - Prob. 1DE Ch. 17 - The following boxes represent aqueos solutions...Ch. 17 - Prob. 2E Ch. 17 - Prob. 3E Ch. 17 - Prob. 4E Ch. 17 - Prob. 5E Ch. 17 - Prob. 6E Ch. 17 - Prob. 7E Ch. 17 - Prob. 8E Ch. 17 - 17.9 The following graphs represent the behavior...Ch. 17 - Prob. 10E Ch. 17 - 17.11 The graph below shows the solubility of a...Ch. 17 - 17.12 Three cations, Ni+2, Cu+2, and Ag+, are...Ch. 17 - Prob. 13E Ch. 17 - Prob. 14E Ch. 17 - Prob. 15E Ch. 17 - Use information from Appendix D to calculate the...Ch. 17 - Prob. 17E Ch. 17 - a. calculate the percent ionization of 0.125 M...Ch. 17 - Prob. 19E Ch. 17 - 17.20 Which of the following solutions is a...Ch. 17 - Prob. 21E Ch. 17 - Calculate the pH of a buffer that is 0.105n M in...Ch. 17 - Prob. 23E Ch. 17 - A buffer is prepared by adding 10.0 g of ammonium...Ch. 17 - You are asked to prepare a pH = 3.00 buffer...Ch. 17 - You are asked to prepare an pH = 4.00 buffer...Ch. 17 - Prob. 27E Ch. 17 - Prob. 28E Ch. 17 - Prob. 29E Ch. 17 - Prob. 30E Ch. 17 - Prob. 31E Ch. 17 - Prob. 32E Ch. 17 - The accompanying graph shows the titration curves...Ch. 17 - Prob. 34E Ch. 17 - 17.35 The samples of nitric and acetic acids shows...Ch. 17 - 17.36 Determine whether each of the following...Ch. 17 - Prob. 37E Ch. 17 - Prob. 38E Ch. 17 - Prob. 39E Ch. 17 - Assume that 30.0 mL of a M solution of a week base...Ch. 17 - Prob. 41E Ch. 17 - Prob. 42E Ch. 17 - Prob. 43E Ch. 17 - Prob. 44E Ch. 17 - Prob. 45E Ch. 17 - Consider the titration of 30.0 mL of 0.050 M NH3...Ch. 17 - Prob. 47E Ch. 17 - Prob. 48E Ch. 17 - 17.49 for each statement, incate whether it is...Ch. 17 - The solubility of two slighty soluble salts of...Ch. 17 - Prob. 51E Ch. 17 - 17.52 a. true or false: solubility and...Ch. 17 - If the molar solubility CaF2 at 35 C is 1.24 *10-3...Ch. 17 - Prob. 54E Ch. 17 - Prob. 55E Ch. 17 - Prob. 56E Ch. 17 - using calculate the molar solubility of AgBr in a....Ch. 17 - calculate the solubility of LaF3 in grams per...Ch. 17 - Prob. 59E Ch. 17 - Consider a beaker containing a saturated solution...Ch. 17 - Calculate the solubility of Mn (OH) 2 in grams per...Ch. 17 - Calculate the molar solubility of Ni (OH) 2 when...Ch. 17 - 17.63 Which of the following salts will be...Ch. 17 - For each of the following slightly soluble salts,...Ch. 17 - Prob. 65E Ch. 17 - Prob. 66E Ch. 17 - Use values of Kap for Agl and Kf for Ag (CN) 2- to...Ch. 17 - Prob. 68E Ch. 17 - Prob. 69E Ch. 17 - Prob. 70E Ch. 17 - Calculate the minimum pH needed to precipitate Mn...Ch. 17 - Prob. 72E Ch. 17 - Prob. 73E Ch. 17 - Prob. 74E Ch. 17 - Prob. 75E Ch. 17 - Prob. 76E Ch. 17 - A solution containing several metal ions is...Ch. 17 - An unknown solid is entirely soluble in water. On...Ch. 17 - Prob. 79E Ch. 17 - Prob. 80E Ch. 17 - 17.81 Precipitation of the group 4 cautions of...Ch. 17 - Prob. 82E Ch. 17 - Prob. 83AE Ch. 17 - Prob. 84AE Ch. 17 - Furoic acid (HC5H3O3) has a K value of 6.76 x 10-4...Ch. 17 - Prob. 86AE Ch. 17 - Equal quantities of 0.010 M solution of an acid HA...Ch. 17 - Prob. 88AE Ch. 17 - 17.89 A biochemist needs 750 ml of an acetic...Ch. 17 - A sample of 0.2140 g of an unknown monophonic acid...Ch. 17 - A sample of 0.1687 g of an unknown monoprotic acid...Ch. 17 - Prob. 92AE Ch. 17 - Prob. 93AE Ch. 17 - What is the pH of a solution made by mixing 0.30...Ch. 17 - Suppose you want to do a physiological experiment...Ch. 17 - Prob. 96AE Ch. 17 - Prob. 97AE Ch. 17 - For each pair of compounds, use Kap values to...Ch. 17 - Prob. 99AE Ch. 17 - Tooth enamel is composed of hydroxyapatite, whose...Ch. 17 - Salts containing the phosphate ion are added to...Ch. 17 - Prob. 102AE Ch. 17 - 17.103 The solubility –product constant for barium...Ch. 17 - Prob. 104AE Ch. 17 - Prob. 105AE Ch. 17 - A buffer of what pH is needed to give a Mg2+...Ch. 17 - The value of Kap for Mg3(AsO4)2 is 2.1 10-20 ....Ch. 17 - Prob. 108AE Ch. 17 - Prob. 109AE Ch. 17 - Prob. 110IE Ch. 17 - Prob. 111IE Ch. 17 - Prob. 112IE Ch. 17 - Prob. 113IE Ch. 17 - Prob. 114IE Ch. 17 - Prob. 115IE Ch. 17 - Prob. 116IE Ch. 17 - A concentration of 10-100 parts per billion (by...Ch. 17 - Prob. 118IE Ch. 17 - Prob. 119IE Ch. 17 - In nonaqueous solvents, it is possible to react HF...

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A mathematical proof for the fact that the pH at the halfway point of a titration of a weak acid with a strong base is equal to p K a of the acid.

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To determine: A mathematical proof for the fact that the pH at the halfway point of a titration of a weak acid with a strong base is equal to pKa of the acid.

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Chapter 17 Solutions