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Question
The Ka value for HCN is 10−9. What is the pH of 0.4 M HCN solution?
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Solution
Given Ka = 10−9
c = 0.4 M
pH = – log [H+]
[H+] = `sqrt("K"_"a" xx "c")`
= `sqrt(10^-9 xx 0.4)`
= 2 × 10−5
∴ pH = – log (2 × 10−5)
= 5 – log 2
= 5 – 0.3010
pH = 4.699
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