(1)A student measures the molar solubility of lead iodide in a water solution to

Question

(1)A student measures the molar solubility of lead iodide in a water solution to be 1.32×10-3 M. Based on her data, the solubility product constant for this compound is

(2)A student measures the OH- concentration in a saturated aqueous solution ofnickel(II) hydroxide to be 8.03×10-6 M.
Based on her data, the solubility product constant for nickel(II) hydroxide is

(3)A student measures the molar solubility of calcium sulfate in a water solution to be 4.76×10-3 M.
Based on her data, the solubility product constant for this compound is

(4)The solubility of Fe(OH)3 is measured and found to be 2.31×10-8 g/L. Use this information to calculate a Ksp value for iron(III) hydroxide.

Ksp =

(5)The solubility of Ag2S is measured and found to be 7.09×10-15 g/L. Use this information to calculate a Ksp value for silver sulfide.

Ksp =

(6)The solubility of CaS is measured and found to be 0.211 g/L. Use this information to calculate a Ksp value for calcium sulfide.

Ksp =

Explanation / Answer

PbI2 =====> Pb2+ + 2I-

                    x             2x

So, given x = 1.32e-3M

Ksp = [Pb2+][I-]^2 = [x][2x]^2 = 9.2 x 10^-9

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