When a weak acid solution is diluted by half, the fraction of ionized weak acid increases. Using the reaction quotient, demonstrate this effect and explain why the increase in ionization occurs.
Also why is increse in ionization occurs on dilution is because of the fact ,On dilution of weak acids it dissociates into ions because of high dielectric constant of water. on dilution ions are readily available and consequently the degree of ionisation increases
When a weak acid solution is diluted by half, the fraction of ionized weak acid increases....
When a weak acid solution is diluted by half, the fraction of ionized weak acid increases. Using the reaction quotient, demonstrate this effect and explain why the increase in ionization occurs.
Use the reaction quotient, Q, to explain why the fraction of dissociation of weak acid, HA, increases when the solution is diluted by a factor of 4. When the system is at equilibrium, Q = [A^-][H^+]/[HA] = K_a. Let's call the concentrations at equilibrium [A^-]e, [H^+]e, and [HA]_e. if the solution is diluted by a factor of 4, the concentrations become [A^-]_e, [H^+]_e, [H^+]_e, and [HA]_e. The reaction quotient becomes Q = K_a. Since Q K_a, the concentrations of products...
4. Acetic acid is a weak electrolyte. Determine the fraction ionized for a 10,3 molal aqueous solution at 25°C, At 25°C, the equilibrium constant is K 1.758x10-5
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?
2. DILUTION EFFECT ON THE PERCENT IONIZATION OF A WEAK ACID a. A weak acid, HX, is 1.3 % ionized in 0.20 M solution. What percent of HX is ionized in a 0.030 M solution? Show the complete setup. percent ionization b. From your result in (a) above answer the following questions: i) How did the percent of ionization change upon dilution? (increased, or decreased) ii) How did the [H,O') concentration of the above weak acid change upon dilution? (increased,...
At a concentration of 1 M, the weak acid HNO, is 2% ionized, and the pH of the solution is 1.7. What happens when KNO, (s) is dissolved into the solution? The extent of HNO, ionization The concentration of H+ The pH You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pK. = 4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer?...
. Calculate the ionization constant for a weak acid, acetic acid (CH3COOH), that is 1.60% ionized in 0.0950 M solution. (Use the ICE table for the dissociation equation) (K. = 1.8 x 10-5 for the acetic acid)
A weak acid, HA, has a pK, of 4.618. If a solution of this acid has a pH of 4.253, what percentage of the acid is not ionized? Assume all H+ in the solution came from the ionization of HA percentage not ionized The Kb for an amine is 1.449 × 10-5 what percentage of the amine is protonated if the pH of a solution of the amine is 9.569? Assume that all OH came from the reaction of B...
A weak acid, HA, has a pK, of 4.971. If a solution of this acid has a pH of 4.437, what percentage of the acid is not ionized? Assume all H+ in the solution came from the ionization of HA. percentage not ionized:
calculate the pH of a 1.3M weak acid solution that is 2.8% ionized