One litre of a strong acid solution contains `10^(-5)` moles of `H^(+)` ions.Then:

Options

A. `pOH=9`
B. Percentage ionisation of water in solution in `1.8xx10^(-9)%`
C. Number of `OH^(-)` ions per `mL` of solution `6.022xx10^(15)`
D. `[H^(+)]_("from"H_(2)O)=10^(-9)M`

Explanation

To solve the problem, we need to analyze the given information about the strong acid solution and the concentration of \( H^+ \) ions.

### Step-by-Step Solution:

1. **Identify the concentration of \( H^+ \) ions**:
The problem states that there is \( 10^{-5} \) moles of \( H^+ \) ions in 1 liter of solution. Therefore, the concentration of \( H^+ \) ions is:
\[
[H^+] = 10^{-5} \, \text{M}
...