100 ml of 0.1 M HCl and 100 ml of 0.1 M HOCN are mixed. What is the concentration of ${"OCN}^{- "};$ and pH of the solution? $(K_{a} = 1.2 \times 10^{- 6})$

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$2.4 \times 10^{- 6}, 2.6$

$1.2 \times 10^{- 6}, 1$

$2.6 \times 10^{- 8}, 1.6$

$1.2 \times 10^{- 6}, 1.3$

answer is A.

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Detailed Solution

$HCl \to H^{+} {+ Cl}^{-1} \Rightarrow 0.1 M × 100 = M × 200 \Rightarrow M = 0.05M after dilution$

$HOCN ⇌ H^{+} {+ OCN}^{-1} \Rightarrow 0.1M × 100 = 1M × 200 \Rightarrow M= 0.05 after dilurion$

$K_{a} = \frac{[H^{+}] [{OCN}^{-}]}{[HOCN]} {1.2 × 10}^{-6} = \frac{0.05 × 0.05 α}{0.05}$

$[{OCN}^{-1}] {= 0.05 α = 1.2 × 10}^{-6}$

$[H^{+}] = {[H^{+}]}_{HCl} = 0.05$

$pH = 1.3$

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