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Question
A weak monobasic acid is 10% dissociated in 0.05 M solution. What is the percent dissociation in 0.15 M solution?
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Solution
Given: ∝1 = 10% = `10/100` = 0.1, c1 = 0.05 M, c2 = 0.15 M, ∝2 = ?
If ∝1 and ∝2 are the values of the degree of dissociation at two different concentrations c1 and c2 respectively, then
Ka = `∝_1^2 "c"_1` = `∝_2^2 "c"_2`
∴ `∝_1^2 "c"_1` = `∝_2^2 "c"_2`
∴ 0.12 × 0.05 = `∝_2^2` × 0.15
∴ `∝_2^2` = `(0.1^2 xx 0.05)/0.15` = 0.0033
∝2 = 0.057 = 5.7%
∴ Percent dissociation = 5.7%
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