Textbook Problem

On the basis of the general solubility rules given in Table 7.1, write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Underline the formula of the precipitate (solid) that forms. If no precipitation reaction is likely for the reactants given, explain why.

monium chloride, ${\text{NH}}_4\text{Cl}$, and sulfuric acid, ${\text{H}}_2{\text{SO}}_4$

tassium carbonate, ${\text{K}}_2{\text{CO}}_3$, and tin(IV) chloride, ${\text{SnCl}}_4$

monium chloride, ${\text{NH}}_4\text{Cl}$

1. , and lead(lI) nitrate,

   $\text{Pb}{\left({\text{NO}}_3\right)}_2$

pper(II) sulfate, ${\text{CuSO}}_4$, and potassium hydroxide, $\text{KOH}$

dium phosphate, ${\text{Na}}_3{\text{PO}}_4$, and chromium(III) chloride, ${\text{CrCl}}_3$

monium sulfide, ${\left({\text{NH}}_4\right)}_2\text{S}$, and iron(III) chloride, ${\text{FeCl}}_3$