Reaction Rates and Equilibrium — Test

Question 17 • Chemistry

Consider the chemical equilibrium of a soap that is present in its aqueous solution. Expand Image What will happen if a large quantity of NaCl is added to the aqueous solution?

Answer

The equilibrium will be permanently destroyed by the addition of NaCl .

The equilibrium will shift to the right, favoring the dissociation of soap in aqueous solution.

The equilibrium will shift to the left to such an extent that it leads to the precipitation of solid soap.

The equilibrium will not be affected by the addition of NaCl to the solution.

Explanation

Soap dissociates in water to form soap ions and sodium ions. Adding a large amount of NaCl increases the concentration of sodium ions, a common ion in this equilibrium. By Le Châtelier’s principle, the equilibrium shifts left, reducing the dissolved soap ions; enough soap can then form an insoluble solid and precipitate. Therefore, the equilibrium shifts left and may produce solid soap.

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