Chapter 16, Problem 66E

Interpretation Introduction

Interpretation:

It is given that, when sodium chloride is added to a solution of silver nitrate, a white precipitate is formed. This precipitate will be dissolved when ammonia is added to this mixture. Now a pale yellow precipitate will appear when a solution of potassium bromide is added to it. Now this precipitate will be dissolved when sodium thiosulfate is added and finally a yellow precipitate is formed when potassium iodide is added to this solution. The balanced equations are to be stated to explain these observations. The conclusion drawn corresponding to the size of the $K_{\text{sp}}$ values for $\text{AgCl},\text{AgBr}$ and $\text{AgI}$ is to be stated.

Concept introduction:

The formation of solid in a solution is known as precipitation. Solubility product, $K_{\text{sp}}$, is defined as the concentration of ions in a saturated solution where each ion is raised to the power of their coefficients.