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Question

Ka for HCN is 5×1010 at 250C. For maintaining a constant pH = 9, the volume of 5 M KCN solution required to be added to 10 mL of 2 M HCN solution is:

A
4 mL
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B
2.5 mL
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C
2 mL
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D
6.4 mL
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Solution

The correct option is C 2 mL
pH=pKa+log[Salt][Acid]

pH=pKa+log[KCN][HCN] .............. (i)

pKa=logKa=log(5×1010)=9.30

Let the volume of 5 M KCN solution required to be V mL.

KCN is added to 10 mL of 2 M HCN solution.

[KCN]=5M×VmLVmL+10mL and
[HCN]=10mL×2MVmL+10mL

Now from eqn.(i) ,

9=9.30+log⎢ ⎢ ⎢5×VV+1010×2V+10⎥ ⎥ ⎥

9=9.30+logV4

logV4=0.30

V4=0.5

V=2mL

Hence, the correct option is C

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