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Question
What is the pH of 0.01 M glycine solution?
[For glycine, Ka1=4.5×10−3 and Ka2=1.7×10−10 at 298 K]
What is the pH of 0.01 M glycine solution?
[For glycine, Ka1=4.5×10−3 and Ka2=1.7×10−10 at 298 K]
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Solution
The correct option is C 7.1
For glycine solution:
Net Ka, acid dissociation constant = Ka1×Ka2 =4.5×10−3×1.7×10−10 =7.65×10−13
[H+]=√K.C
=√7.65×10−13×0.01=8.7×10−8
Hence, pH=−log[H+]
=−log[8.7×10−8]
=−(log10−8+log 8.7)
=8−0.93=7.07≈7.1
For glycine solution:
Net Ka, acid dissociation constant = Ka1×Ka2 =4.5×10−3×1.7×10−10 =7.65×10−13
[H+]=√K.C
=√7.65×10−13×0.01=8.7×10−8
Hence, pH=−log[H+]
=−log[8.7×10−8]
=−(log10−8+log 8.7)
=8−0.93=7.07≈7.1
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