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A student measures the molar solubility of silver sulfide in a water solution to be 2.99x10-17 M. Based on her data, the soluA student measures the so-concentration in a saturated aqueous solution of calcium sulfate to be 5.03x10-3 M. Based on her da

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Answer #1

Silver sulfide ionized as

Ag2S(s) ---------> Ag+(aq) + 2S--(aq)

Suppose the molarity/solubility of Ag2S is S

Then Ksp = Sx(2S)^2 = 4S3

It is given that

S = 2 99x10^-17 M

Therefore Ksp = 4*(2.99x10^-17)^3

Ksp = 1.069 x 10^-49 M3

Ionization of calcium sulphate is

CaSO4(aq) -------> Ca2+(aq) + SO42-(aq)

Ksp = SxS = S2

Where S is the molar concentration of SO4--which is also equal to the concentration of Ca2+

It is given that S = 5.03 x 10^-3 M

Hence Ksp = (5.03x10^-3)^3 = 1.27 x 10^-7 M3

Hence the answers are

Ksp = 1.069 x 10^-49 M3

Ksp = 1.27 x 10^-7 M2

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