Calculate the concentration of H+in 0.1(M) acetic acid solution containing 0.1(M)HCl as medium (Ka = 1.75 × 10-5)

To calculate the concentration of H+ in a 0.1M acetic acid solution containing 0.1M HCl as medium, we need to consider the ionization of both the acetic acid and the HCl.

Step 1: Calculate the ionization of HCl HCl is a strong acid, which means it completely ionizes in solution. Therefore, the concentration of H+ ions from HCl is 0.1M.

Step 2: Calculate the ionization of acetic acid Acetic acid is a weak acid, so it does not completely ionize in solution. We can use the Ka expression to calculate the concentration of H+ ions from acetic acid.

The Ka expression for acetic acid is Ka = [H+][A-]/[HA], where [H+] is the concentration of hydrogen ions, [A-] is the concentration of acetate ions, and [HA] is the concentration of acetic acid.

Given that Ka = 1.75 × 10^-5 and [HA] = 0.1M, we can set up the equation as follows:

1.75 × 10^-5 = [H+][A-]/0.1

Assuming that the ionization of acetic acid is small compared to the initial concentration, we can simplify this to:

1.75 × 10^-5 = [H+]^2/0.1

Solving for [H+], we get:

[H+] = sqrt(1.75 × 10^-5 * 0.1) = 1.32 × 10^-3 M

Step 3: Add the concentrations of H+ ions from HCl and acetic acid The total concentration of H+ ions in the solution is the sum of the concentrations from HCl and acetic acid, which is 0.1M + 1.32 × 10^-3 M = 0.10132 M.