The concentration of S2− in a 0.1MH2SKa1Ka2=1.1×10−21M2 which is also 0.1 in H+ is

The concentration of $S^{2 -}$ in a $0.1 {MH}_{2} S (K_{a 1} K_{a 2} = 1.1 \times 10^{- 21} M^{2})$ which is also $0.1$ in $H^{+}$ is

A
$1.1 \times 10^{- 19} M$
B
$1.1 \times 10^{- 20} M$
C
$1.1 \times 10^{- 21} M$
D
$1.1 \times 10^{- 22} M$

Solution:

$[S^{2 -}] = \frac{K_{al} K_{a 2}}{{[H^{+}]}^{2}} [H_{2} S] = \frac{(1.1 \times 10^{- 21} M^{3}) (0.1 M)}{[0.1 M]^{2}} = 1.1 \times 10^{- 20} M$

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