Problem: The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?A) 4.9 x 10-2B) 1.7 x 10-5C) 8.5 x 10-6D) 4.2 x 10-6E) <1.0 x 10-6    

FREE Expert Solution

We're asked to calculate the value of Ksp for Lead (II) chloride, PbCl2 if its solubility in water is 0.45 g/100 mL


PbClis an ionic compound and will dissociate in water by the reaction:


The charge of lead, Pb = +2 (from Roman numeral = II)


PbCl2 (s)  Pb2+ (aq) + 2 Cl(aq)

The molar concentration of PbCl2 is:


Molarity of PbCl2=0.45 g PbCl2100 mL(1 mol PbCl2278.1 g PbCl2)(1 mL10-3 L)=0.016 mol/L 0.016 M


We can construct an ICE table for this dissociation

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Problem Details

The solubility of lead(II) chloride is 0.45 g/100 mL of solution. What is the Ksp of PbCl2?

A) 4.9 x 10-2

B) 1.7 x 10-5

C) 8.5 x 10-6

D) 4.2 x 10-6

E) <1.0 x 10-6    

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