Calculate `pH` of the solution which is `10^(-1)M` in `HCl` & `10^(-3)M` in `CH_(3)COOH[K_(a)=2xx10^(-5)]`.Also calculate `[H^(+)]` form `CH_(3)COOH`.

Explanation

To solve the problem, we need to calculate the pH of a solution that is 0.1 M (10^(-1) M) in HCl and 0.001 M (10^(-3) M) in acetic acid (CH₃COOH), given that the dissociation constant (Kₐ) for acetic acid is 2 x 10^(-5). We also need to find the concentration of hydrogen ions ([H⁺]) contributed by acetic acid.

### Step 1: Calculate the contribution of H⁺ from HCl
HCl is a strong acid and completely dissociates in solution. Therefore, the concentration of H⁺ ions from HCl is equal to the concentration of HCl.

\[ [H^+]_{HCl} = 0.1 \, M \]
...