Chapter 7, Problem 97CP

Interpretation Introduction

Interpretation:

The precipitate (if formed) for the following reaction should be determined.

Concept Introduction:

The reaction in which precipitate would be formed is known as precipitation reaction. The solubility guidelines help to determine whether the formed compound is soluble or not in the given solution.

There are following solubility rules:

1. The salts formed from sodium, potassium and ammonium ions are soluble in nature.
2. All sulfate salts are soluble except ${\text{CaSO}}_4$, ${\text{PbSO}}_4$ and ${\text{BaSO}}_4$.
3. All nitrate salts are soluble. The formula of nitrate polyatomic ion is ${\text{NO}}_3^{-}$.
4. All the salts formed from chloride, bromide and iodide are soluble except those with ${\text{Pb}}^{2+}$ and ${\text{Ag}}^{+}$.
5. All sulfate salts are insoluble except ${\text{Na}}_{\text{2}}{\text{SO}}_{\text{3}}$, ${\text{K}}_{\text{2}}{\text{SO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{SO}}_{\text{3}}$.
6. All sulfides are insoluble except ${\text{Na}}_{\text{2}}\text{S}$, ${\text{K}}_{\text{2}}\text{S}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}\text{S}$.
7. All oxides and hydroxides are insoluble except ${\text{Na}}_{\text{2}}\text{O}$ /NaOH, ${\text{K}}_{\text{2}}\text{O}$ /KOH and $\text{BaO}/\text{Ba}{\left(\text{OH}\right)}_{\text{2}}$.
8. All carbonates are insoluble except ${\text{Na}}_{\text{2}}{\text{CO}}_3$, ${\text{K}}_{\text{2}}{\text{CO}}_{\text{3}}$ and ${\left({\text{NH}}_4\right)}_{\text{2}}{\text{CO}}_{\text{3}}$.