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Chapter 14: Problem 31

Consider the following statements. Write out an example reaction and \(K\) expression that is associated with each statement. a. The autoionization of water. b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion. c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion.

Short Answer

Expert verified
a. Example reaction: \( 2H_2O \longleftrightarrow H_3O^+ + OH^-\) Equilibrium constant expression: \[K_w = [H_3O^+][OH^-]\] b. Example reaction: \( CH_3COOH + H_2O \longleftrightarrow CH_3COO^- + H_3O^+\) Equilibrium constant expression: \[K_a = \frac{[CH_3COO^-][H_3O^+]}{[CH_3COOH]}\] c. Example reaction: \( NH_3 + H_2O \longleftrightarrow NH_4^+ + OH^-\) Equilibrium constant expression: \[K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}\]

Step by step solution

01

Example reaction

The autoionization of water can be written as: \( 2H_2O \longleftrightarrow H_3O^+ + OH^-\)
02

Equilibrium constant expression

The equilibrium constant expression, K, for this reaction is called the ion product of water (Kw) and is expressed as: \[K_w = [H_3O^+][OH^-]\] #b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion#
03

Example reaction

We'll use acetic acid (CH3COOH) as our example. The reaction between acetic acid and water can be written as: \( CH_3COOH + H_2O \longleftrightarrow CH_3COO^- + H_3O^+\)
04

Equilibrium constant expression

The equilibrium constant expression, K, for this reaction is called the acid dissociation constant (Ka) and is expressed as: \[K_a = \frac{[CH_3COO^-][H_3O^+]}{[CH_3COOH]}\] #c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion#
05

Example reaction

We'll use ammonia (NH3) as our example base. The reaction between ammonia and water can be written as: \( NH_3 + H_2O \longleftrightarrow NH_4^+ + OH^-\)
06

Equilibrium constant expression

The equilibrium constant expression, K, for this reaction is called the base dissociation constant (Kb) and is expressed as: \[K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}\]

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Most popular questions from this chapter

What are the major species present in a \(0.150-M \mathrm{NH}_{3}\) solution? Calculate the \(\left[\mathrm{OH}^{-}\right]\) and the pH of this solution.

A solution is prepared by dissolving 0.56 g benzoic acid $\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}, K_{\mathrm{a}}=6.4 \times 10^{-5}\right)\( in enough water to make 1.0 \)\mathrm{L}$ of solution. Calculate $\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2} \mathrm{H}\right],\left[\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{CO}_{2}\right],\left[\mathrm{H}^{+}\right]$ \(\left[\mathrm{OH}^{-}\right],\) and the pH of this solution.

A solution is made by adding 50.0 \(\mathrm{mL}\) of 0.200\(M\) acetic acid \(\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)\) to 50.0 \(\mathrm{mL}\) of \(1.00 \times 10^{-3} \mathrm{M} \mathrm{HCl}\) a. Calculate the pH of the solution. b. Calculate the acetate ion concentration.

Monochloroacetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{2} \mathrm{ClO}_{2},\) is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of \(K_{\mathrm{a}}\) for monochloroacetic acid is \(1.35 \times 10^{-3}\) Calculate the pH of a \(0.10-M\) solution of monochloroacetic acid.

An unknown salt is either $\mathrm{NaCN}, \mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2},$ NaF, NaCl, or NaOCl. When 0.100 mole of the salt is dissolved in 1.00 \(\mathrm{L}\) of solution, the pH of the solution is \(8.07 .\) What is the identity of the salt?
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