Write the ionic equation for dissolution and the solubility product ( K sp ) exp
ID: 537223 • Letter: W
Question
Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the following slightly soluble ionic compounds. (For the ionic equations, include states-of-matter under the given conditions in your answer.
Solubility equilibrium expressions take the general form: Ksp = [An+]a . [Bm]b. Subscripts and superscripts that include letters must be enclosed in braces {}. For example: Ksp=[A+]2.[B2-] must be typed using K_{sp}=[A^+]^2.[B^2-]
(a) Cu3(PO4)2
Net ionic equation
Solubility product expression
(b) Ag2S
Net ionic equation
Solubility product expression
(c) BaSO3
Net ionic equation
Solubility product expression
(d) BaF2
Net ionic equation
Solubility product expression
AND
Use solubility products and predict which of the following salts is the most soluble, in terms of moles per liter, in pure water. (Hint: The size of Ksp tells us about solubility in general, but technically you must calculate the molar solubility in order to compare.)
Special note: mercury(I) ions forms a dimer and behaves like a polyatomic ion. So, Hg2X2 breaks into Hg22+ + 2X-
Hg2I2, Ksp= 5.2e-29
Sn(OH)2, Ksp= 5.5e-27
Ag2SO4, Ksp= 1.2e-05
BaF2, Ksp= 1.8e-07
Explanation / Answer
To write the net ionic equation we need to consider the following:
To write the solubility product (ksp) expression, we use the coefficients of the net ionic equation as superscripts in the concentration of the ion. For example:
A2B3 <=> 2A3+ + 3B2-
ksp = [A3+]2[B2-]3
With that in mind we can answer the problem:
(a) Cu3(PO4)2
Net ionic equation: Cu3(PO4)2 (s) <=> 3Cu2+ + 2PO43-
Solubility product expression: ksp = [Cu2+]3[PO43-]2
(b) Ag2S
Net ionic equation: Ag2S (s) <=> 2Ag+ + S2-
Solubility product expression: ksp = [Ag+]2[S2-]
(c) BaSO3
Net ionic equation: BaSO3 <=> Ba2+ + SO32-
Solubility product expression: ksp = [Ba2+][SO32-]
(d) BaF2
Net ionic equation: BaF2 <=> Ba2+ + 2F-
Solubility product expression: [Ba2+][F-]2
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