Upon titrating a solution of weak monoprotic acid with a weak monoacidic base solution at equivalent point:

Options

A. `pH` in general weak would increase if both solution are first diluted to `10` times the original volume & then titration is carries out
B. `pH` in general would decrease if both solution are first diluted to `10` times the original volume & then titration is carried out.
C. `pH` in general would remain same `(=7)` if both solutions are first diluted to `10` times the original volumes & then titration is carried out
D. `pH` in general coule be less than , greater then or equal to `7`if both solutions are first diluted to`10` times the original volume & then titration is carried out.

Explanation

To solve the problem of determining which of the two salts, AB or XY2, is more soluble given that they have the same solubility product (Ksp), we can follow these steps:

### Step 1: Define the Dissolution Reactions
- For salt AB, which dissociates into A⁺ and B⁻ ions:
\[ AB (s) \rightleftharpoons A^+ (aq) + B^- (aq) \]

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