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Question
At 90oC, pure water has [H+]=10−6M, if 100 mL of 0.2 M HCl is added to 200 mL of 0.1 M KOH at 90oC then pH of the resulting solution will be:
At 90oC, pure water has [H+]=10−6M, if 100 mL of 0.2 M HCl is added to 200 mL of 0.1 M KOH at 90oC then pH of the resulting solution will be:
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Solution
The correct option is D 6
100 mL of 0.2 M HCl will completely neutralise 200 mL of 0.1 M KOH. The resulting solution will be neutral with [H+]=10−6M and
pH=−log[H+]=−log10−6=6
100 mL of 0.2 M HCl will completely neutralise 200 mL of 0.1 M KOH. The resulting solution will be neutral with [H+]=10−6M and
pH=−log[H+]=−log10−6=6
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