Questions: Classify each ionic compound as insoluble or soluble in water. Select the single best answer for each part. Note: Reference the General solubility rules for ionic compounds in water table for additional information. Part 1 of 4 K2SO4 soluble insoluble Part 2 of 4 PbBr2 soluble insoluble Part 3 of 4 Zn(OH)2 soluble insoluble Part 4 of 4 Bi(NO3)3 soluble insoluble

Classify each ionic compound as insoluble or soluble in water. Select the single best answer for each part. Note: Reference the General solubility rules for ionic compounds in water table for additional information. Part 1 of 4 K2SO4 soluble insoluble Part 2 of 4 PbBr2 soluble insoluble Part 3 of 4 Zn(OH)2 soluble insoluble Part 4 of 4 Bi(NO3)3 soluble insoluble
Transcript text: Classify each ionic compound as insoluble or soluble in water. Select the single best answer for each part. Note: Reference the General solubility rules for ionic compounds in water table for additional information. Part 1 of 4 \[ \mathrm{K}_{2} \mathrm{SO}_{4} \] soluble insoluble Part 2 of 4 $\mathrm{PbBr}_{2}$ soluble insoluble Part 3 of 4 \[ \mathrm{Zn}(\mathrm{OH})_{2} \] soluble insoluble Part 4 of 4 $\mathrm{Bi}\left(\mathrm{NO}_{3}\right)_{3}$ soluble insoluble
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Solution

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Solution Steps

Step 1: Determine the Solubility of \(\mathrm{K}_{2} \mathrm{SO}_{4}\)

Potassium sulfate (\(\mathrm{K}_{2} \mathrm{SO}_{4}\)) contains the potassium ion (\(\mathrm{K}^+\)). According to the general solubility rules, all compounds containing alkali metal ions (such as \(\mathrm{K}^+\)) are soluble in water.

Step 2: Determine the Solubility of \(\mathrm{PbBr}_{2}\)

Lead(II) bromide (\(\mathrm{PbBr}_{2}\)) contains the lead ion (\(\mathrm{Pb}^{2+}\)) and bromide ions (\(\mathrm{Br}^-\)). According to the solubility rules, most bromides are soluble, except those of lead, silver, and mercury. Therefore, \(\mathrm{PbBr}_{2}\) is insoluble in water.

Step 3: Determine the Solubility of \(\mathrm{Zn}(\mathrm{OH})_{2}\)

Zinc hydroxide (\(\mathrm{Zn}(\mathrm{OH})_{2}\)) contains the hydroxide ion (\(\mathrm{OH}^-\)). According to the solubility rules, most hydroxides are insoluble, except those of alkali metals and \(\mathrm{Ba(OH)_2}\). Therefore, \(\mathrm{Zn}(\mathrm{OH})_{2}\) is insoluble in water.

Final Answer

\[ \begin{align_} \text{Part 1:} & \quad \boxed{\text{soluble}} \\ \text{Part 2:} & \quad \boxed{\text{insoluble}} \\ \text{Part 3:} & \quad \boxed{\text{insoluble}} \\ \end{align_} \]

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