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In each question a blank or blanks are left. Fill in the blank(s) with relevant answer(s).
The concentration of $$\text{H}^+$$ ions in 0.10 M solution of a weak acid is $$1 \times 10^{-5}\text{ mol L}^{-1}$$. Calculate the dissociation constant of the acid __________ [Note - [HA] can be taken as 0.1 M as $$1 \times 10^{-5}$$ is very small]
Correct Answer: 0.000000001
For $$\text{HA} \rightleftharpoons \text{H}^+ + \text{A}^-$$, $$[\text{H}^+] = [\text{A}^-] = 10^{-5}$$ and $$[\text{HA}] \approx 0.1$$. So $$K_a = \frac{(10^{-5})^2}{0.1} = 10^{-9}$$, i.e. 0.000000001.
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