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Question
The pH of a 0.1M solution of NH4OH (having Kb=1.0×10−5) is equal to:
The pH of a 0.1M solution of NH4OH (having Kb=1.0×10−5) is equal to:
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Solution
The correct option is B 11
[OH−]=√Kb×C=√1×10−5×10−1=√10−6=10−3Kw=[H+][OH−]10−14=[H+][10−3][H+]=10−11Hence, pH=−logH+−log(1×10−11)=11
[OH−]=√Kb×C
=√1×10−5×10−1
=√10−6=10−3
Kw=[H+][OH−]
10−14=[H+][10−3]
[H+]=10−11
Hence, pH=−logH+
−log(1×10−11)=11
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