Textbook Question
What is the pH and the principal source of H3O+ ions in 1.0 * 10-10 M HCl? (Hint: The pH of an acid solution can’t exceed 7.) What is the pH of 1.0 * 10-7 M HCl?
Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Chapter 16, Problem 15
For a solution of two weak acids with comparable values of Ka, there is no single principal reaction. The two acid dissociation equilibrium equations must therefore be solved simultaneously. Calculate the pH in a solution that is 0.10 M in acetic acid (CH3CO2H, Ka = 1.8 * 10^-5) and 0.10 M in benzoic acid (C6H5CO2H, Ka = 6.5 * 10^-5). (Hint: Let x = [CH3CO2H] that dissociates and y = [C6H5CO2H] that dissociates; then [H3O+] = x + y.)
Verified step by step guidance1
Step 1: Write the dissociation equations for both acetic acid and benzoic acid. For acetic acid: \( \text{CH}_3\text{CO}_2\text{H} \rightleftharpoons \text{CH}_3\text{CO}_2^- + \text{H}_3\text{O}^+ \) and for benzoic acid: \( \text{C}_6\text{H}_5\text{CO}_2\text{H} \rightleftharpoons \text{C}_6\text{H}_5\text{CO}_2^- + \text{H}_3\text{O}^+ \).
Step 2: Set up the equilibrium expressions for each acid using their respective \( K_a \) values. For acetic acid: \( K_{a1} = \frac{[\text{CH}_3\text{CO}_2^-][\text{H}_3\text{O}^+]}{[\text{CH}_3\text{CO}_2\text{H}]} = 1.8 \times 10^{-5} \) and for benzoic acid: \( K_{a2} = \frac{[\text{C}_6\text{H}_5\text{CO}_2^-][\text{H}_3\text{O}^+]}{[\text{C}_6\text{H}_5\text{CO}_2\text{H}]} = 6.5 \times 10^{-5} \).
Step 3: Assume \( x \) moles per liter of acetic acid dissociate and \( y \) moles per liter of benzoic acid dissociate. Therefore, \([\text{H}_3\text{O}^+] = x + y\).
Step 4: Substitute \([\text{H}_3\text{O}^+] = x + y\) into the equilibrium expressions: \( K_{a1} = \frac{x(x + y)}{0.10 - x} \) and \( K_{a2} = \frac{y(x + y)}{0.10 - y} \).
Step 5: Solve the system of equations simultaneously to find the values of \( x \) and \( y \), which will allow you to calculate \([\text{H}_3\text{O}^+] = x + y\) and subsequently the pH using \( \text{pH} = -\log([\text{H}_3\text{O}^+]) \).
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Weak Acids and Acid Dissociation Constant (Ka)
Weak acids are substances that partially dissociate in solution to produce hydrogen ions (H3O+). The strength of a weak acid is quantified by its acid dissociation constant (Ka), which measures the extent of dissociation. A higher Ka value indicates a stronger weak acid, while a lower Ka suggests a weaker acid. In this problem, both acetic acid and benzoic acid are weak acids with given Ka values, which are essential for calculating their contributions to the pH.
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00:44
ICE Charts of Weak Acids
Simultaneous Equilibrium Calculations
When multiple weak acids are present in a solution, their dissociation reactions can affect each other, leading to a situation where no single principal reaction dominates. To find the pH, one must set up and solve the equilibrium expressions for each acid simultaneously. This involves defining variables for the concentrations of dissociated species and applying the equilibrium constants (Ka) to create a system of equations that can be solved together.
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02:38Equilibrium Constant Calculation
pH Calculation from Hydronium Ion Concentration
The pH of a solution is a measure of its acidity, defined as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+]. In this scenario, the total concentration of hydronium ions is the sum of the contributions from both weak acids, represented as [H3O+] = x + y, where x and y are the amounts of acetic and benzoic acids that dissociate, respectively. Calculating the pH requires determining this total concentration from the equilibrium expressions.
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06:25Hydronium Ion Concentration Example
Related Practice
Textbook Question
Consider the reaction: SO2 + OH- S HSO3-. Which reaction scheme shows the correct use of the curved arrow notation representing thedonation of an electron pair and the correct labeling of the Lewis acid and Lewis base? (LO 16.14)(a) (b) (c) (d)
Textbook Question
Calculate the pH of solutions prepared by:
(d) Mixing equal volumes of 0.20 M HCl and 0.50 M HNO3.
(Assume that volumes are additive.)
Textbook Question
The acidity of lemon juice is derived primarily from citric acid (H3Cit), a triprotic acid. What are the concentrations of H3Cit, H2Cit-, HCit2-, and Cit3- in a sample of lemon juice that has a pH of 2.37 and a total concentration of the four citrate-containing species of 0.350 M?