14.3 Exercise 29

From the equilibrium concentrations given, calculate K_a for each of the weak acids and K_b for each of the weak bases.

(a) NH₃: [OH⁻] = 3.1 $\times$ 10⁻³ M;
$\left[\text{NH}_{4} ^{+}\right]$ = 3.1 $\times$ 10⁻³ M;

[NH₃] = 0.533 M;

(b) HNO₂: $\left[\text{H}_{3} \text{O}^{+}\right]$ = 0.011 M;
$\left[\text{NO}_{2} ^{−}\right]$ = 0.0438 M;

[HNO₂] = 1.07 M;

(c) (CH₃)₃N: [(CH₃)₃N] = 0.25 M;
[(CH₃)₃NH⁺] = 4.3 $\times$ 10⁻³ M;

[OH⁻] = 3.7 $\times$ 10⁻³ M;

(d) $\text{NH}_{4} ^{+} :$ $\left[\text{NH}_{4} ^{+}\right]$ = 0.100 M;

[NH₃] = 7.5 $\times$ 10⁻⁶ M;
[H₃O⁺] = 7.5 $\times$ 10⁻⁶ M