1 M solution of `CH_(3)COOH` is diluted to x times so that pH of solution is doubled. Calculate x
Given `K_(a)=1.8xx10^(-5)`

Explanation

To solve the problem, we need to find the dilution factor \( x \) such that the pH of a 1 M solution of acetic acid (\( CH_3COOH \)) is doubled upon dilution. Given the dissociation constant \( K_a = 1.8 \times 10^{-5} \), we can follow these steps:

### Step 1: Calculate the initial pH of the 1 M acetic acid solution.

The dissociation of acetic acid can be represented as:
\[ CH_3COOH \rightleftharpoons H^+ + CH_3COO^- \]
...