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Multiple Choice
Using the Ksp for calcium iodate hexahydrate, calculate the molarity of calcium ions in a saturated solution if the Ksp is 6.47 x 10^-6.
A
3.23 x 10^-3 M
B
2.54 x 10^-3 M
C
6.47 x 10^-6 M
D
1.27 x 10^-2 M
Verified step by step guidance
1
First, understand the dissolution process of calcium iodate hexahydrate, which can be represented by the chemical equation: Ca(IO3)2·6H2O(s) ⇌ Ca²⁺(aq) + 2 IO3⁻(aq).
The solubility product constant (Ksp) expression for this equilibrium is given by: . This expression relates the concentrations of the ions in a saturated solution.
Let the molarity of calcium ions, [Ca²⁺], be represented by x. Since the stoichiometry of the dissolution shows that for every mole of Ca²⁺ produced, 2 moles of IO3⁻ are produced, the concentration of iodate ions, [IO3⁻], will be 2x.
Substitute these expressions into the Ksp expression: . Set this equal to the given Ksp value, 6.47 x 10⁻⁶.
Solve the equation for x to find the molarity of calcium ions in the saturated solution.