A) \[{{K}_{h}}=\frac{{{K}_{w}}}{\sqrt{{{K}_{a}}(HCN)}}\]
B) \[h=\sqrt{\frac{{{K}_{h}}}{C}}\]
C) \[pH=\frac{1}{2}p{{K}_{a}}(HCN)\]
D) \[{{H}^{+}}=\sqrt{\frac{{{K}_{w}}\times {{K}_{a}}}{C}}\]
Correct Answer: D
Solution :
\[C{{N}^{-}}+{{H}_{2}}OHCN+O{{H}^{-}}\] This is the salt of weak acid and strong base. Hence, \[{{K}_{h}}=\frac{{{K}_{w}}}{{{K}_{a}}(HCN)}\] \[h=\sqrt{\frac{{{K}_{h}}}{C}}\] and \[{{K}_{w}}={{K}_{h}}\times {{K}_{a}}\] then \[[{{H}^{+}}]=\sqrt{\frac{{{K}_{w}}\times {{K}_{a}}}{C}}\]
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