. Calculate the pH of a 0.1M solution of HClO (Ka = 3.0 x 10-8).8.524.2612.02

To calculate the pH of a 0.1M solution of HClO, we first need to set up the ionization equation and the Ka expression for HClO.

The ionization of HClO in water can be represented as follows:

HClO ⇌ H+ + ClO-

The Ka expression for this reaction is:

Ka = [H+][ClO-] / [HClO]

Given that the initial concentration of HClO is 0.1M and assuming that x is the amount of HClO that ionizes, we can express the concentrations of H+, ClO-, and HClO at equilibrium as follows:

[H+] = x, [ClO-] = x, [HClO] = 0.1 - x

Substituting these values into the Ka expression gives:

3.0 x 10^-8 = x^2 / (0.1 - x)

Since Ka is very small, we can assume that x is much smaller than 0.1, so the equation simplifies to:

3.0 x 10^-8 = x^2 / 0.1

Solving for x gives:

x = sqrt(3.0 x 10^-8 * 0.1) = 5.48 x 10^-5 M

This is the concentration of H+ ions, so the pH of the solution is:

pH = -log[H+] = -log(5.48 x 10^-5) = 4.26

So, the pH of a 0.1M solution of HClO is approximately 4.26.