Question

Consider the chemical equilibrium of a soap that is present in its aqueous solution. C17H35COONa(aq) mc017-1.jpg C17H35COO–(aq) + Na+(aq) sodium stearate (soap) stearate ion What will happen if a large quantity of NaCl is added to the aqueous solution?
A)The equilibrium will shift to the right, favoring the dissociation of soap in aqueous solution.
B)The equilibrium will shift to the left to such an extent that it leads to the precipitation of solid soap.
C)The equilibrium will not be affected by the addition of NaCl to the solution.
D)The equilibrium will be permanently destroyed by the addition of NaCl.

Answer 1

B.

The shift to the left will be due to the fact that sodium ions will be released when NaCl is dissolved in the solution.

Answer 2

Answer : Option B) The equilibrium will shift to the left to such an extent that it leads to the precipitation of solid soap.

Explanation : The equilibrium will tend to shift to left because addition of sodium chloride salt will lead to precipitate the soap as a product. The volume increase in the sodium ions because of sodium chloride addition will generate the more amount of solid soap.