Chemistry

Problem

K_{a_2}

for

\text{H}_2\text{S} = 1.0 \times 10^{-15}

and

K_{sp}

\text{Ba}_3(\text{AsO}_4)_2

\text{Ag}_2\text{S}

and

\text{Ag}_3\text{AsO}_4

are

7.70 \times 10^{-51}

2.0 \times 10^{-49}

and

1.0 \times 10^{-22}

respectively. The equilibrium constant for the reaction :

3\text{Ag}_2\text{S}_{(s)} + \text{Ba}_3(\text{AsO}_4)_2(s) + 3\text{H}^+ \rightleftharpoons 2\text{Ag}_3\text{AsO}_{4(s)} + 3\text{HS}^- + 3\text{Ba}^{2+}

is : a.

5.6 \times 10^{-124}

3.0 \times 10^{-109}

5.6 \times 10^{-108}

4.63 \times 10^{-108}