Question

question at position 15 a 0.00100 m solution of a weak acid, hx, is 3.0% ionized. calculate the ionization constant for the acid. a 0.00100 m solution of a weak acid, hx, is 3.0% ionized. calculate the ionization constant for the acid. 4.8 x 10-4 8.2 x 10-6 3.0 x 10-2 9.3 x 10-7 5.5 x 10-10

Answer 1

To calculate the ionization constant for the weak acid, we can use the concentration of the acid and the percentage of ionization. In this case, we have a 0.00100 M solution of the weak acid, hx, that is 3.0% ionized. To find the ionization constant, we can use the equation: Ka = ([HX-][H+])/[HX]. Given that [HX] = 0.00100 M, and the acid is 3.0% ionized, we can determine that [H+] = 0.00100 M * 0.030 = 0.00003 M and [HX-] = 0.00100 M * 0.030 = 0.00003 M. Plugging these values into the equation, we get: Ka = (0.00003 M * 0.00003 M) / 0.00003 M = 0.0000009 M. Therefore, the ionization constant for the acid is 9.0 x 10-7.

Step-by-step explanation:

To calculate the ionization constant for the weak acid, we can use the concentration of the acid and the percentage of ionization. In this case, we have a 0.00100 M solution of the weak acid, hx, that is 3.0% ionized.

To find the ionization constant, we can use the equation:

Ka = ([HX-][H+])/[HX]

Given that [HX] = 0.00100 M, and the acid is 3.0% ionized, we can determine that [H+] = 0.00100 M * 0.030 = 0.00003 M and [HX-] = 0.00100 M * 0.030 = 0.00003 M.

Plugging these values into the equation, we get:

Ka = (0.00003 M * 0.00003 M) / 0.00003 M = 0.0000009 M

Therefore, the ionization constant for the acid is 9.0 x 10-7.