Questions: According to solubility rules, which compound should dissolve in water? Select one: CaSO4 K3PO4 AgBr MgCO3

Transcript text: According to solubility rules, which compound should dissolve in water? Select one: $\mathrm{CaSO}_{4}$ $\mathrm{K}_{3} \mathrm{PO}_{4}$ AgBr $\mathrm{MgCO}_{3}$

Solution

Solution Steps

Step 1: Identify Solubility Rules for Each Compound

To determine which compound dissolves in water, we need to apply general solubility rules:

Calcium sulfate ($\mathrm{CaSO}_{4}$): Sulfates are generally soluble, but there are exceptions such as $\mathrm{CaSO}_{4}$, which is only slightly soluble.
Potassium phosphate ($\mathrm{K}_{3} \mathrm{PO}_{4}$): Compounds containing alkali metal ions (like potassium) are generally soluble.
Silver bromide (AgBr): Most silver salts are insoluble, with exceptions like $\mathrm{AgNO}_{3}$ and $\mathrm{AgC}_{2}\mathrm{H}_{3}\mathrm{O}_{2}$.
Magnesium carbonate ($\mathrm{MgCO}_{3}$): Carbonates are generally insoluble, except for those of alkali metals and ammonium.

Step 2: Apply Solubility Rules to Determine Solubility

Based on the solubility rules:

$\mathrm{CaSO}_{4}$ is slightly soluble.
$\mathrm{K}_{3} \mathrm{PO}_{4}$ is soluble because it contains potassium, an alkali metal.
AgBr is insoluble.
$\mathrm{MgCO}_{3}$ is insoluble.