Calculating the pH When a Common Ion Is Involved For the generic equilibrium HA(

Question

Calculating the pH When a Common Ion Is Involved

For the generic equilibrium HA(aq) H+(aq) + A(aq) , which of these statements is true?

For the generic equilibrium m HA (aq) ~ ightleftharpoons~ m H^+ (aq)~+~A^-(aq), which of these statements is true?

1 If you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase. 2 If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of HA would decrease. 3 If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of A would decrease. 4 The equilibrium constant for this reaction changes as the pH changes.

Explanation / Answer

HA(aq) H+(aq) + A(aq)

If you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase. TRUE, equilibrium will shift to left, therefore H+ is decreased, therefore pH increases

If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of HA would decrease. FALSE, it will increase due to the shift of equilibrium

If you add the soluble salt KA to a solution of HA that is at equilibrium, the concentration of A would decrease. FALSE, since you are adding KA--> K+ and A-

The equilibrium constant for this reaction changes as the pH changes. Ka wont change with ´pH

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