Question

For the generic equilibrium HA(aq) ⇌ H+(aq) + A−(aq), which of these statements is true? For the generic equilibrium , which of these statements is true? The equilibrium constant for this reaction changes as the pH changes. If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of A− would decrease. If you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase. If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of HA would decrease.

Answer 1

The equilibrium constant for the reaction HA(aq) ⇌ H+(aq) + A-(aq) does not change as the pH changes. Adding the soluble salt KA to a solution of HA at equilibrium does not change the pH, the concentration of A-, or the concentration of HA.

Step-by-step explanation:

The equilibrium constant for the reaction HA(aq) ⟶ H+(aq) + A-(aq) does not change as the pH changes. The equilibrium constant, represented by K, is a constant value that depends on the temperature and the nature of the reaction, but not on the pH. Therefore, statement one is false.

If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of A- would increase, not decrease. This is because KA is a salt that dissociates into K+ and A- ions, and the equilibrium will shift to the right to increase the concentration of A-. Therefore, statement two is false.

If you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would remain unchanged. The addition of KA does not directly affect the pH since it does not introduce any H+ or OH- ions. Therefore, statement three is false.

If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of HA would remain unchanged. The addition of KA does not directly affect the concentration of HA since it does not introduce any HA or A- ions. Therefore, statement four is false.

Answer 2

The correct answer is The equilibrium constant for this reaction changes as the pH changes.

Step-by-step explanation:

The equilibrium constant of a reaction depends of pH and viceverca.There is a equation that link pH with equilibrium constant Ka(for assumption).The equation is given below,

pH=pKa+log[A-/HA]

where[A-] is the concentration of conjugate base and [HA] is the concentration of conjugate acid.