Two weak monobasic organic acids `HA` and `HB` have dissociation constants as `3.0 xx 10^(-5)` and `1.5 xx 10^(-5)`, respectively, at `25^(@)C`. If `500mL` of `1M` solutions of each of these two acids are mixed to produce`1L` of mixed acid solution, what is the `pH` of the resulting solutions?

Explanation

To solve the problem, we need to find the pH of a mixed solution of two weak monobasic organic acids, HA and HB, with given dissociation constants. Here’s a step-by-step solution:

### Step 1: Understand the Dissociation of the Acids
Both acids dissociate in water as follows:
- For acid HA:
\[ HA \rightleftharpoons H^+ + A^- \]
- For acid HB:
\[ HB \rightleftharpoons H^+ + B^- \]
...