If a solution originally 0.532 M in acid HA is found to have a hydronium concentration of 0.112 M at equilibrium,...
A 0.10 M solution of a weak monoprotic acid (HA) has a hydronium-ion concentration of 4.2× 10⁻⁴ M at equilibrium. What is the acid-ionization constant, Ka, for this acid?
The initial concentration of acid HA in solution is 1.7 M. If the pH of the solution at equilibrium is 2.20, what is the percent ionization of the acid? Round the answer to two significant figures.
The initial concentration of acid HA in solution is 2.0 M. If the pH of the solution at equilibrium is 2.2, what is the percent ionization of the acid? Remember to report your answer with the correct number of significant figures Sorry, that's incorrect. Try again? [0.032]%
What is the hydronium ion concentration of a 0.280 M weak acid solution of an acid whose ionization constant is 3.10 x 10-9?
6. A0.68 M solution of a weak acid HA is 0.35 % ionized. What are the H, A, and HA concentrations at equilibrium? What is K? 7. The K, for glyoxylic acid, HC HO, is 6.6 x 104. What is the pH of a 0.45 M solution of the acid? What is the % ionization of the acid at this concentration?
44. A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 4.6 x 10 *M. What is the acid- ionization constant, Ka, for this acid? 2.2.1 x 10-2 b. 3.2 * 10-3 C.4.6 x 104 d. 2.1 x 10-6 e.5.5 x 10-5
You make a 0.1 M solution with acid HA, a monoprotic acid. The Ka for this acid is 1.0E-8. If HA is mixed with a 50 M NaCl solution (no common ions with HA), determine the percent ionization of HA. So I calculated that the ionic strength of the solution is equal to 0.2 and found the activity coefficent to be 0.7469. When I plugged in the values into the Ka=(activity of A- * activity of H3O+)/activity of HA equation,...
Calculate the equilibrium concentration of a weak acid HA solution when 20.0 mL of 1.0 M HA is mixed with 20.0 mL of 1.0 M NaA. (Ka = 1.8x10-5)
A 10.0 mL solution containing an unknown monoprotic acid, HA, ([HA]0 = 0.450 mol/L) was found to have a percent ionization of 1.18 % at 25.0 ̊C. Determine the value of Ka for this unknown acid.
What is the hydronium ion concentration, pH, and percent ionization of a .025M solution of carbonic acid? Ka = 4.5 x 10^-7