The base dissociation constant for hydrazine N2H4 is 9.6×10−7. What would be the percent hydrolysis of 0.1MN2H5Cl, a salt containing the acid ion conjugate to hydrazine base at 25∘C?
A
2.667×10−3
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B
1.525×10−4
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C
4.557×10−6
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D
3.225×10−2
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Solution
The correct option is D3.225×10−2 N2H+5(aq)+H2O(l)⇌N2H4(aq)+H3O+(aq) Kh=KwKb=10−149.6×10−7=1.04×10−8 now, CKh=0.11.04×10−8≈107 Since CKh>100∴1−h≈1