Questions: Now examine salts containing the halide anions, Cl^- and Br-. Most of these are soluble. What two cations listed lead to insoluble halide salts?

Now examine salts containing the halide anions, Cl^- and Br-. Most of these are soluble. What two cations listed lead to insoluble halide salts?

Transcript text: Now examine salts containing the halide anions, $\mathrm{Cl}^{-}$and Br$^{-}$. Most of these are soluble. What two cations listed lead to insoluble halide salts?

Solution

Solution Steps

Step 1: Identify the Halide Anions

The halide anions mentioned in the question are chloride ($\mathrm{Cl}^{-}$) and bromide ($\mathrm{Br}^{-}$).

Step 2: Review the Solubility Rules for Halides

In general, most halide salts are soluble in water. However, there are exceptions, particularly with certain cations. Common exceptions include salts containing silver ($\mathrm{Ag}^{+}$), lead ($\mathrm{Pb}^{2+}$), and mercury ($\mathrm{Hg}_2^{2+}$).

Step 3: Identify Cations Leading to Insoluble Halide Salts

From the table provided, we need to identify which cations form insoluble salts with the halide anions ($\mathrm{Cl}^{-}$ and $\mathrm{Br}^{-}$).

Silver ($\mathrm{Ag}^{+}$): Known to form insoluble salts with halides such as $\mathrm{AgCl}$ and $\mathrm{AgBr}$.
Lead ($\mathrm{Pb}^{2+}$): Known to form insoluble salts with halides such as $\mathrm{PbCl}_2$ and $\mathrm{PbBr}_2$.

Final Answer

\[ \boxed{\mathrm{Ag}^{+} \text{ and } \mathrm{Pb}^{2+}} \]

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