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Question
When 10 mL of 0.1 M acetic acid (pKa=5.0) is titrated against 10 mL of 0.1 M ammonia solution (pKb=5.0), the equivalence point occurs at pH:
When 10 mL of 0.1 M acetic acid (pKa=5.0) is titrated against 10 mL of 0.1 M ammonia solution (pKb=5.0), the equivalence point occurs at pH:
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Solution
The correct option is C 7.0
CH3COOH+NH4OH→CH3COONH4+H2O
For salt of weak base and weak acid,
pH=−12[logKa+logKw−logKb]
=−12[−pKa+logKw+pKb]
=−12[−5+log10−14+5]
=−12[−5−14+5]
=7Hence, option C is correct.
CH3COOH+NH4OH→CH3COONH4+H2O
For salt of weak base and weak acid,
pH=−12[logKa+logKw−logKb]
pH=−12[logKa+logKw−logKb]
=−12[−pKa+logKw+pKb]
=−12[−5+log10−14+5]
=−12[−5−14+5]
=7
Hence, option C is correct.
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