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Chapter 14: Problem 27

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. The autoionization of water: \[ 2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq) \] \[ K_w = [H_3O^+][OH^-] \] b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion: \[ HA(aq) + H_2O(l) \rightleftharpoons H_3O^+(aq) + A^-(aq) \] \[ K_a = \frac{[H_3O^+][A^-]}{[HA]} \] c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion: \[ B(aq) + H_2O(l) \rightleftharpoons BH^+(aq) + OH^-(aq) \] \[ K_b = \frac{[BH^+][OH^-]}{[B]} \]

Step by step solution

01

a. The autoionization of water

The autoionization of water refers to the process of water dissociating into hydroxide ions (OH-) and hydronium ions (H3O+). This process is represented by the following reaction: \[ 2H_2O(l) \rightleftharpoons H_3O^+(aq) + OH^-(aq) \] The equilibrium constant expression for this reaction, referred to as the ion product constant of water (Kw), is given by: \[ K_w = [H_3O^+][OH^-] \]
02

b. An acid reacts with water to produce the conjugate base of the acid and the hydronium ion

Let's consider the reaction of a generic acid (HA) with water: \[ HA(aq) + H_2O(l) \rightleftharpoons H_3O^+(aq) + A^-(aq) \] Here, HA is the acid, H3O+ is the hydronium ion, and A- is the conjugate base of the acid. The equilibrium constant expression for this reaction, referred to as the acid dissociation constant (Ka), is given by: \[ K_a = \frac{[H_3O^+][A^-]}{[HA]} \]
03

c. A base reacts with water to produce the conjugate acid of the base and the hydroxide ion

Now let's consider the reaction of a generic base (B) with water: \[ B(aq) + H_2O(l) \rightleftharpoons BH^+(aq) + OH^-(aq) \] Here, B is the base, BH+ is the conjugate acid of the base, and OH- is the hydroxide ion. The equilibrium constant expression for this reaction, referred to as the base dissociation constant (Kb), is given by: \[ K_b = \frac{[BH^+][OH^-]}{[B]} \]

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of each of the following solutions containing a strong acid in water. a. \(2.0 \times 10^{-2} \mathrm{M} \mathrm{HNO}_{3}\) c. \(6.2 \times 10^{-12} \mathrm{M} \mathrm{HNO}_{3}\) b. \(4.0 \mathrm{M} \mathrm{HNO}_{3}\)

A \(0.15 M\) solution of a weak acid is \(3.0 \%\) dissociated. Calculate \(K_{\mathrm{a}} .\)

For the reaction of hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right)\) in water. $$ \mathrm{H}_{2} \mathrm{NNH}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{NNH}_{3}^{+}(a q)+\mathrm{OH}^{-}(a q) $$ \(K_{\mathrm{b}}\) is \(3.0 \times 10^{-6}\). Calculate the concentrations of all species and the \(\mathrm{pH}\) of a \(2.0 \mathrm{M}\) solution of hydrazine in water.

Will \(0.10 M\) solutions of the following salts be acidic, basic, or neutral? See Appendix 5 for \(K_{\mathrm{a}}\) values. a. ammonium bicarbonate b. sodium dihydrogen phosphate c. sodium hydrogen phosphate d. ammonium dihydrogen phosphate e. ammonium formate

Rank the following \(0.10 \mathrm{M}\) solutions in order of increasing \(\mathrm{pH}\). a. HI, HF, NaF, NaI b. \(\mathrm{NH}_{4} \mathrm{Br}, \mathrm{HBr}, \mathrm{KBr}, \mathrm{NH}_{3}\) c. \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3} \mathrm{NO}_{3}, \mathrm{NaNO}_{3}, \mathrm{NaOH}, \mathrm{HOC}_{6} \mathrm{H}_{5}, \mathrm{KOC}_{6} \mathrm{H}_{5}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), \(\mathrm{HNO}_{3}\)
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