Give the expression for the solubility product constant for PbCl2. [Pb²+][Cl]² [PbCl₂] [PbC1₂] [Pb²+][Cl]² [Pb²+][Cl-]² [Pb²+]²[Cl] [PbCl₂] [Pb²+]²[CI-]
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![**Question:**
Give the expression for the solubility product constant for PbCl₂.
**Options:**
1. \(\frac{[\text{Pb}^{2+}][\text{Cl}^-]^2}{[\text{PbCl}_2]}\)
2. \(\frac{[\text{PbCl}_2]}{[\text{Pb}^{2+}][\text{Cl}^-]^2}\)
3. \([\text{Pb}^{2+}][\text{Cl}^-]^2\)
4. \(\frac{[\text{Pb}^{2+}][2\text{Cl}^-]}{[\text{PbCl}_2]}\)
5. \([\text{Pb}^{2+}]^2[\text{Cl}^-]\)
**Explanation:**
Each option represents a possible expression for the solubility product (K_sp) of lead(II) chloride (PbCl₂). The correct expression for K_sp is based on the equilibrium:
\[ \text{PbCl}_2 (s) \rightleftharpoons \text{Pb}^{2+} (aq) + 2\text{Cl}^- (aq) \]
The solubility product expression is:
\[ K_{sp} = [\text{Pb}^{2+}][\text{Cl}^-]^2 \]
This corresponds to option 3.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5cb748f-b247-416f-8df5-751d92c52687%2F06358024-d2d7-4f30-8d43-7d415b44242e%2Fo7kttop_processed.png&w=3840&q=75)
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