A) \[6.8\times {{10}^{-6}}\]
B) \[6.8\times {{10}^{6}}\]
C) \[2.2\times {{10}^{-9}}\]
D) none of these
Correct Answer: D
Solution :
Key Idea: Write the dissociation reaction for Pbl2, then find relationship between solubility product \[({{K}_{sp}})\] and solubility. Substitute the values and find the value of \[{{K}_{sp}}\] \[Pb{{I}_{2}}P{{b}^{2+}}+2{{I}^{-}}\] Let solubility of \[Pb{{I}_{2}}\] \[=x\,\,mol/L\] (concentration) \[x\] \[x\] \[2x\] \[{{K}_{sp}}=[P{{b}^{2+}}]{{[{{I}^{-}}]}^{2}}\] \[=(x)\,{{(2x)}^{2}}\] \[=4{{x}^{3}}\] Given \[x=0.005\,mol/L\] \[\therefore \] \[{{K}_{sp}}=4{{x}^{3}}\] \[=4\times {{(0.005)}^{3}}\] \[=5\times {{10}^{-7}}\]
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