When acetic acid (HC_2 H_3 O_2) is added to water, it reacts to form hydronium i

Question

When acetic acid (HC_2 H_3 O_2) is added to water, it reacts to form hydronium ions (H_3 O^+) and acetate ions (C_2 H_3 O_2) as well as producing heat. HC_2 H_3 O_2 + H_2 O H_3 O^+ + C_2 H_3 O_2^- + heat How will the equilibrium change, if at all, if you remove acetate ions (C_2 H_3 O_2^-)? The rate of the forward reaction would increase, shifting the reaction to the right and increasing the amount of product. The equilibrium changes, but how it changes can not be determined. The reaction equation has changed and is no longer balanced. The reaction stops and no reaction can now occur. No changes occur. The rate of the reverse reaction would increase, shifting the reaction to the left and increasing the amount of reactant.

Explanation / Answer

According to the Le-Charterlier's principle,

If the concentration of reactants is increased or product is removed , the reaction will take place in the forward direction. If the concentration of reactants decreases or increasing the concentration of products the reaction will take place in the backward direction.

Here we are removing acetate ions (products) , the equilibrium shifts in forward direction, so the rate of forward reaction would increases and increasing the formation of more product.

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