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Question
On the basis of the equation \[\ce{pH}\] = – log \[\ce{[H+]}\], the \[\ce{pH}\] of 10–8 mol dm–3 solution of \[\ce{HCl}\] should be 8. However, it is observed to be less than 7.0. Explain the reason.
Solution
Here concentration of water cannot be neglected since the solution is very dilute. \[\ce{pH}\] will be less than 7.0. Hence, the total concentration is given as -
\[\ce{[H3O+] = 10^{-8} + 10^{-7}M}\].
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