Question

Calculate the percent ionization of 0.110 m lactic acid (ka=1.4×10−4).

Answer 1

To calculate the percent ionization of a 0.10-M solution of acetic acid with a pH of 2.89, first calculate the concentration of hydronium ions using the pH value. Then, use the formula for percent ionization to calculate the percent ionization of the acid.

Step-by-step explanation:

To calculate the percent ionization of a solution, we need to first calculate the concentration of the hydronium ions in the solution. From the given pH of 2.89, we can determine the concentration of hydronium ions using the equation pH = -log[H3O+].

So, 2.89 = -log[H3O+]. Taking the antilog of both sides, we get [H3O+] = 10^(-2.89) = 1.22 x 10^(-3) M.

Next, we can calculate the percent ionization using the equation Percent Ionization = (concentration of ionized acid / initial concentration of acid) x 100.

For acetic acid, the initial concentration is given as 0.10 M. Since it is a weak acid, it does not completely ionize, so the concentration of ionized acid can be assumed to be equal to the concentration of hydronium ions. Plugging in the values, we get Percent Ionization = (1.22 x 10^(-3) M / 0.10 M) x 100 = 1.22%.

Answer 2

3.57

Step-by-step explanation:

Ka = ca2

==> a = √ ( Ka / c )

Given Ka = 1.4x10^-4

c = concentration = 0.110 M

Plug the values we get a = 0.0357

% dissociation = 0.0357 x 100 = 3.57