The molar solubility of chromium(III) hydroxide in a 0.148 M chromium(III) nitra

Question

The molar solubility of chromium(III) hydroxide in a 0.148 M chromium(III) nitrate solution is  M.

The molar solubility of calcium phosphate in a 0.108 M sodium phosphate solution is  M.

Write a balanced net ionic equation to show why the solubility of Co(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.

Find K :

Write a balanced net ionic equation to show why the solubility of Ni(CN)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.

K=

Explanation / Answer

Ksp of Cr(OH)3 = 3×10–29

Cr(OH)3   --------------->   Cr+3   + 3 OH-

                                        0.148      3 S

Ksp = [Cr+3][OH-]^3

3×10–29 = 0.148 x (3S)^3

S = 1.96 x 10^-10

molar solubility = 1.96 x 10^-10 M

2)

Ksp of Ca3(PO4)2 = 2.07×10–33

Ca3(PO4)2 -----------------> 3 Ca+2 + 2 PO43-

                                              3 S             0.108

Ksp = [Ca+2]^3[PO43-]^2

2.07×10–33 = (3S)^3 x (0.108)^2

S = 1.87 x 10^-11 M

molar solubility = 1.87 x 10^-11 M

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