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? if you add the soluble salt ka to a solution of ha that is at equilibrium, the concentration of ha would decrease. if you add the soluble salt ka to a solution of ha that is at equilibrium, the ph would increase. 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.

THIS USER ASKED 👇

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? if you add the soluble salt ka to a solution of ha that is at equilibrium, the concentration of ha would decrease. if you add the soluble salt ka to a solution of ha that is at equilibrium, the ph would increase. 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.

THIS IS THE BEST ANSWER 👇

The correct statement is that if you add the KA soluble salt to a solution of HA that is in equilibrium, the pH would increase.

Explanation:

A common ion effect is defined as the effect that occurs on equilibrium when a common ion (ion already in the solution) is added to a solution. This effect usually reduces solubility.

The equilibrium reaction of HA and KA follows the equation:

According to the Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium shifts in the direction in order to minimize the effect.

In the equilibrium reactions, ion is increasing on the product side, so the equilibrium will shift in the direction to minimize this effect, which is towards HA.

Thus, the addition of KA will shift the equilibrium in the left direction.

An equilibrium constant depends on the temperature of the system. It has no effect on any change in pH.

PH is defined as the negative logarithm of the hydrogen ions contained in the solution

If there is a high concentration of hydrogen ions in the solution, then the pH will be low. If the hydrogen ion concentration in the solution is low, then the pH will be high.

Because the equilibrium is shifting in the left direction, that means concentration of it ion is declining. This will increase the pH of the solution.

Hence, the correct statement is that if you add the KA soluble salt to an equilibrium solution of HA, the pH would increase.