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A certain weak acid has Ka = 1.0 \times 10-4. Calculate the equilibrium constant for its reaction with a strong base.

Option: 1

10-10


Option: 2

1010


Option: 3

104


Option: 4

108


Answers (1)

best_answer

Given, 

\mathrm{HA \rightleftharpoons H^+ + A^-, K_a = 10^{-4}}

and we know that

\mathrm{H^+ + OH^- \rightleftharpoons H_2O, K =\frac{1}{K_w}= 10^{14}}

Adding the above two reactions we get

\mathrm{HA + OH^- \rightleftharpoons A^- +H_2O, K_{net} =\frac{K_a}{K_w}}

\therefore \mathrm{ K_{net} =\frac{K_a}{K_w}= \frac{10^{-4}}{10^{-14}}= 10^{10}}

Therefore, option(2) is correct

Posted by

Kuldeep Maurya

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