Accepting Kw = 1  10-14 at 250C, calculate concentrations of H3O+ and OH- in mole/litre in 0.1M, 0.001M and 0.0002M HCl solutions; also calculate pH and pOH of the solutions.

Sure, let's calculate the concentrations of H3O+ and OH- in mole/litre, as well as the pH and pOH of the solutions for each of the given HCl solutions.

1. For 0.1M HCl solution:

HCl is a strong acid and it ionizes completely in water. So, the concentration of H3O+ ions will be equal to the concentration of HCl, which is 0.1M.

The ion product of water, Kw = [H3O+][OH-] = 1 x 10^-14. We can use this to find the concentration of OH- ions.

[OH-] = Kw / [H3O+] = 1 x 10^-14 / 0.1 = 1 x 10^-13 M

The pH is the negative logarithm of the H3O+ concentration, so pH = -log(0.1) = 1.

The pOH is the negative logarithm of the OH- concentration, so pOH = -log(1 x 10^-13) = 13.

2. For 0.001M HCl solution:

The concentration of H3O+ ions will be 0.001M.

[OH-] = Kw / [H3O+] = 1 x 10^-14 / 0.001 = 1 x 10^-11 M

pH = -log(0.001) = 3.

pOH = -log(1 x 10^-11) = 11.

3. For 0.0002M HCl solution:

The concentration of H3O+ ions will be 0.0002M.

[OH-] = Kw / [H3O+] = 1 x 10^-14 / 0.0002 = 5 x 10^-11 M

pH = -log(0.0002) = 3.7 (approx).

pOH = -log(5 x 10^-11) = 10.3 (approx).

So, these are the concentrations of H3O+ and OH- ions, and the pH and pOH values for the given HCl solutions.