Question

Indicate how the concentration of each aqueous species in the chemical equation changes to reestablish equilibrium after changing the concentration of a reactant or product. also indicate how the ph changes. an up arrow indicates an increase in concentration, a down arrow indicates a decrease in concentration, and leaving it blank means there is no change in the concentration.

HCN(aq)+H₂O(l) ⇋ CN⁻(aq) + H₃O⁺(aq) pH
after the concentration of HCN is increased
after the concentration of CN⁻ is decreased

Answer 1

When the concentration of HCN is increased, the concentration of HCN will decrease and the concentration of CN⁻ will increase to reestablish equilibrium. The pH of the solution may also change depending on the specific reaction. When the concentration of CN⁻ is decreased, the concentration of CN⁻ will decrease and the concentration of HCN will increase to reestablish equilibrium. The pH of the solution may also change depending on the specific reaction.

Step-by-step explanation:

When the concentration of HCN is increased, the reaction will shift in order to reestablish equilibrium. This means that the concentration of HCN will decrease, represented by a down arrow, while the concentration of CN⁻ will increase, represented by an up arrow. The pH of the solution may also change depending on the specific reaction. For example, if the reaction involves HCN acting as an acid, an increase in its concentration would lead to a decrease in pH, making the solution more acidic.

On the other hand, when the concentration of CN⁻ is decreased, the reaction will again shift to reach equilibrium. In this case, the concentration of CN⁻ will decrease, indicated by a down arrow, while the concentration of HCN will increase, represented by an up arrow. The pH of the solution may also change, depending on the specific reaction. If the reaction involves CN⁻ acting as a base, a decrease in its concentration would lead to an increase in pH, making the solution more basic.