1.) Which of the factors affecting solubility explains the observation that silv

Question

1.) Which of the factors affecting solubility explains the observation that silver phosphate (Ag3PO4) is more soluble in pure water than in an aqueous solution of sodium phosphate (Na3PO4).

A. Some insoluble compounds are amphoteric. B. The formation of complex ions displaces the solubility equilibrium toward the aqueous ions. C. The solubility of many salts is affected by the pH of the solution. D. The solubility of most salts increases as temperature increases. E. A common ion displaces the solubility equilibrium toward the undissolved solute.

Explanation / Answer

E. A common ion displaces the solubility equilibrium toward the undissolved solute. this option is true.

Ag3PO4 <---> 3Ag+ + PO43-

Increase in solubility of this salt means the equilibrium has to be shifted on the right hand side in order to form the dissociated ions.

But when it's the aqueous solution of sodium phosphate (Na3PO4), Na3PO4 remains in its dissociated form mostly

Na3PO4 <---> 3Na+ + PO43-

So, in presence of more PO43- in the solution, the common ion effect comes into consideration, i.e. with increase in corresponding concentration of PO43- shifts the equilibrium of Ag3PO4 towards undissociated Ag3PO4, which means it decreases the solubility. In normal water, no such common ion effect is observed. Hence, Ag3PO4 is found to be more soluble in pure water than in an aqueous solution of sodium phosphate.

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