When H 2 S(g) is dissolved in water, the following equilibrium is established: H 2 S(aq) + H 2 O(l) ⇌ H 3 O + (aq) + HS - (aq) for which the equilibrium constant is 9.1 × 10 -8 . If the pH of solution

Question

When H 2 S(g) is dissolved in water, the following equilibrium is established: H 2 S(aq) + H 2 O(l) ⇌ H 3 O + (aq) + HS - (aq) for which the equilibrium constant is 9.1 × 10 -8 . If the pH of solution is 5.0, what would be the ratio of concentration of HS - (aq) to H 2 S(aq)?

TestHub · Accepted Answer

K = [H 3 O + ][HS - ]/[H 2 S] = 9.1 × 10 -8 pH = 5.0 gives [H 3 O + ] = 10 -5 M [HS - ]/[H 2 S] = K/[H 3 O + ] = 9.1 × 10 -8 /10 -5 = 9.1 × 10 -3 This is option (d).

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