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ozzi
2 years ago
14

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?a. 8.5 ? 10^-6b. 4.2 ? 10^-6c. 1.7 ?

10^-5d. 4.9 ? 10^-2e. < 1.0 ? 10^-6
Chemistry
1 answer:
frosja888 [35]2 years ago
8 0

The value of  K_{sp} of PbCl_{2}  is 1.7×10^{-5} .

So, option C is correct one.

Calculation,

Number of moles of PbCl_{2}  = mass/molar mass = 0.45/278.1 = 1.618×10^{-3} moles

Concentration of Pb^{+2} and Cl^{-} ion

Molarity  of Pb^{+2} = Number of moles of solute /volume in lit

Molarity  of Pb^{+2} = 1.618×10^{-3} moles /0.1 lit = 0.0162 M

PbCl_{2} →  Pb^{+2} +  2Cl^{-}

For certain amount of  Pb^{+2} , twice this amount of  Cl^{-} ion formed.

The concentration of   Cl^{-} ion formed = 2× 0.0162 M = 0.0324 M

Now,

K_{sp} of PbCl_{2} = [ Pb^{+2} ][Cl^{-}]^{2} = 0.0162 ×[0.0324 ]^{2} =  1.7×10^{-5} .

learn about Molarity  

brainly.com/question/8732513

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