What is the pH of a 1.0M solution of acetic acid? To what volume of one litre of this solution be diluted so that the pH of the resulting solution will be twice the original value? Given, Ka=1.8×10−5
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Solution
We know that degree of dissociation
α=√KaC=√1.8×10−51=4.2426×10−3
[H+]=Cα=1×4.2426×10−3=4.2426×10−3molL−1
pH=log[H+]=−log4.2426×10−3=2.3724
so, pH of the acetic acid solution after dilution=2×2.3724