Question

Predict whether each of the following ionic compounds is soluble in water:

a.$AgCl$

b.$KI$

c.$N{a}_{2}S$

d.$A{g}_{2}O$

e.$CaS{O}_4$

Short answer

(part a) The ionic compound $AgCl$is insoluble in water.

(part b) The ionic compound $KI$is soluble in water.

(part c) The ionic compound $N{a}_{2}S$is soluble in water.

(part d) The ionic compound $A{g}_{2}O$is insoluble in water.

(part e) The ionic compound $CaS{O}_4$is insoluble in water.

Step-by-step solution

Introduction (part a).

Ionic compounds are those that are constituted by ionic species connecting together via electrostatic forces.

Find the ionic compound is soluble in water or not (part a).

Given:

$AgCl$

$A{g}^{+}$and $C{l}^{-}$ions are present in the ionic compound $AgCl$. Silver compounds do not dissolve in the water. Therefore,$AgCl$ is insoluble in water.

Find the ionic compound is soluble in water or not (part b). 

Given:

$Kl$

$K^{+}$ and $I^{-}$ ions are present in the ionic compound $KI.$ In water, $K^{+}$ ions have always been soluble. As a result, $Kl$ is soluble in water.

Find the ionic compound is soluble in water or not (part c).

Given:

$N{a}_{2}S$

The ionic compound $N{a}_{2}S$contains $N{a}^{+}$and $S^{-2}$ions. Usually sulfides are insoluble in water but $N{a}^{+}$ions are always soluble in water. For this reason,$N{a}_{2}S$ is soluble in water.

Find the ionic compound is soluble in water or not (part d). 

Given:

$A{g}_{2}O$

Like most metal oxides and silver compounds, the ionic compound$A{g}_{2}O$ is insoluble in water.

Find the ionic compound is soluble in water or not (part e).

Given:

$CaS{O}_4$

$C{a}^{+2}$and $S{O_4}^{-2}$ions are present in the ionic compound $CaS{O}_4$Therefore,$CaS{O}_4$is insoluble in water.