A) 4.65
B) 5.35
C) 4.35
D) 2.65
Correct Answer: B
Solution :
For the salt of strong acid and weak base \[{{H}^{+}}=\sqrt{\frac{{{K}_{\text{w}}}\times C}{{{K}_{b}}}}\] \[\left[ {{H}^{+}} \right]=\sqrt{\frac{{{10}^{-14}}\times 2\times {{10}^{-2}}}{{{10}^{-5}}}}\] \[-\log \left[ {{H}^{+}} \right]=6-\frac{1}{2}\log 20\] \[\therefore \]\[pH=5.35\]You need to login to perform this action.
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