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Question
Two weak monobasic organic acids HA and HB have dissociation constants as 1.5×10−5 and 1.8×10−5 respectively at 25∘C. If 500 ml of 1M solution of each of these two two acids are mixed to produce 1 litre of mixed solution, what is the pH of the resulting solution?
Two weak monobasic organic acids HA and HB have dissociation constants as 1.5×10−5 and 1.8×10−5 respectively at 25∘C. If 500 ml of 1M solution of each of these two two acids are mixed to produce 1 litre of mixed solution, what is the pH of the resulting solution?
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Solution
The correct option is B 2.4
H3O+=√C1K1+C2K2=√0.5×1.5×10−5+0.52×10−5
=√16.5×10−6=4.1×10−3
pH=−log[4.1×10−3]=2.4
H3O+=√C1K1+C2K2=√0.5×1.5×10−5+0.52×10−5
=√16.5×10−6=4.1×10−3
pH=−log[4.1×10−3]=2.4
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