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Question
Calculate the pH (write only integer part) of a solution obtained by mixing 0.1 litre of pH=4 and 0.2 litre of pH=10. Both contain strong acid and base respectively.
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Solution
pH 10 corresponds to pOH 4.
Thus, 0.1 L of acid (pH4) willbe completely neutralized with 0.1 L of base (pH 10). Thus only 0.1 L of base (pH 10) is left with volume increased to 0.3 L. Thus, the concntration will be reduced to one third.
Hence, [H+]=1×10−103=3.333×10−10
Hence, the pH of the solution will be pH=−log[H+]=−log3.33×10−10=9.5338.
Hence, the pH of the solution is 9.5338.
Thus, 0.1 L of acid (pH4) willbe completely neutralized with 0.1 L of base (pH 10). Thus only 0.1 L of base (pH 10) is left with volume increased to 0.3 L. Thus, the concntration will be reduced to one third.
Hence, [H+]=1×10−103=3.333×10−10
Hence, the pH of the solution will be pH=−log[H+]=−log3.33×10−10=9.5338.
Hence, the pH of the solution is 9.5338.
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