Solubility Equilibrium

$1.77 \times 10^{-10}$

$2.5 \times 10^{-9}$

$5.0 \times 10^{-7}$

$3.2 \times 10^{-8}$

Increases

Decreases

Remains the same

Becomes insoluble

$K_{sp} = [Pb^{2+}][CrO_{4}^{2-}]$

$K_{sp} = [PbCrO_{4}]$

$K_{sp} = [Pb^{2+}] + [CrO_{4}^{2-}]$

$K_{sp} = [Pb^{2+}] \times [CrO_{4}^{2-}]$

$BaSO_{4}$

$NaCl$

$KNO_{3}$

$Mg(OH)_{2}$

$Ag^{+}$ and $Br^{-}$

$Ag_{2}^{+}$ and $Br^{-}$

$Ag^{+}$ only

$Br^{-}$ only

Increases with temperature

Decreases with temperature

No effect

Varies by salt

Increase in solubility due to a common ion

Decrease in solubility due to a common ion

No effect on solubility

Increase in solubility with temperature

$1.0 \times 10^{-5}$ M

$2.0 \times 10^{-5}$ M

$3.0 \times 10^{-5}$ M

$4.0 \times 10^{-5}$ M

The rate of dissolution equals the rate of precipitation.

Only solid is present at equilibrium.

Solubility does not depend on temperature.

Saturation means no solute is present.

Increases solubility

Decreases solubility

No significant effect

Varies by substance