A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is...
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H2O ⇌ H3O+ + A- What is the percent ionization of the acid?
A weak base has an initial concentration of 0.287 M. After undergoing dissociation the pH is 12.23. A- + H2O ⇌ OH- + HA What is the percent ionization of the base? Options: A 5.92% B 12.3% C 1.68% D 0.0123% E 0.995%
Question 6 (1 point) A weak base has an initial concentration of 0.588 M. After undergoing dissociation the pH is 12.14. A+ H2O = HA + OH- What is the percent ionization pf the base? 0.569% O 1.41% 4.84% 0.0992% 2.35%
A weak acid, (HA), has an acid dissociation constant of 4.60∙10–6. A 25.00 ml sample with a concentration of 0.1200 M is titrated with 0.1500 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.1200 M sample of HA? c. What is the percent ionization of the 0.1200 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 8.00 ml NaOH have been added?
A weak acid, HF, is prepared with an initial concentration of 1.20 M. After reaching equilibrium, it has a pH of 1.551. What is the percent ionization of this acid? Select one: 4.2% 0.84% 2.4% None of these 0.082%
14. A weak acid, (HA), has an acid dissociation constant of 2.50 . 10-6. A 25.00 ml sample with a concentration of 0.250 M is titrated with 0.150 M NaOH. a. Write the equation for the acid dissociation equilibrium. b. What is the pH of the original 0.250 M sample of HA? c. What is the percent ionization of the 0.250 M acid? d. Write the equation for the neutralization reaction. e. What is the pH after 12.00 ml 0.150M...
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+ (aq) + A (aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, K ? Answer in scientific...
A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the hydrogen ion concentration of this solution? Answer in scientific notation and be sure to include your units. (Scientific notation: Ex. 2.4 x 103 = 2.4E3) HA(aq) + H+(aq) + A'(aq) Answer: A 0.048 M solution of an unknown weak acid, HA, has a pH = 2.75. What is the value of the acid dissociation constant, Ka? Answer in scientific notation. Answer: A...
The percent dissociation for a weak acid is given by the following relationship: % Dissociation = for HA + H2O ? H3O+ + A- Show mathematically that doubling the initial concentration of weak acid lowers the % dissociation. Hint: Start with [HA]o and solve ICE problem for this initial condition, then do the same for [HA]o/2. *It seems obvious to me that doubling the initial concentration would lower the % dissociation based on the% dissociation equation. I'm...
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.