# Use the molar solubility in pure water to calculate Ksp for these three compounds.?

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A) Use the molar solubility 1.08 x 10^-5 M in pure water water to calculate Ksp for BaCrO4.

B) Use the molar solubility 1.55 x 10^-5 M in pure water water to calculate Ksp for Ag2SO3

C) Use the molar solubility 2.22 x 10^-8 M in pure water water to calculate Ksp for Pd(SCN)2.

• A) Ksp = [Ba++][CrO4–]

For every x moles of BaCrO4 that dissolves in a liter of water, the concentration of Ba++ is x Molar, and the concentration of CrO4– is x Molar. Therefore,

Ksp = (x)(x) = x² = (1.08 x 10^-5 M)² = 1.17 x 10^-10 M².

B) Ksp = [Ag]²[SO3–]

For every x moles of Ag2SO3 that dissolves in a liter of water, the concentration of Ag+ is 2x Molar, and the concentration of SO3– is x Molar. Therefore,

Ksp = (2x)²(x) = 4x³ = (4)(1.55 x 10^-5 M)³ = 1.49 x 10^-14 M³.

C) Ksp = [Pd++][SCN-]²

In the same manner as question B),

Ksp = (x)(2x)² = 4x³ = (4)(2.22 x 10^-8 M)³ = 4.38 x 10^-23 M³.

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