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Question

The solubility of AgCN in a buffer solution of pH=3 is:
[Given Ksp of AgCN=1.2×106 and Ka for HCN=4.8×1010. Assume that no cyano complex is formed.]

A
a=1.67×105 M
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B
a=1.58×105 M
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C
a=1.51×105 M
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D
None of these
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Solution

The correct option is C a=1.58×105 M
Assume solubility of AgCN be a M in presence of a buffer of pH=3
AgCNAg+a+CNa
[Ag+]=a;[HCN]=a
For weak HCN, Ka=[H+][CN][HCN]
or 4.8×1010=103[CN]a
[CN]=4.8×107×a
For AgCN: Ksp=[Ag+][CN]
1.2×1016=a×4.8×107×a
a2=1.2×10164.8×107
a=1.58×105 M

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