Multiple Choice
Determine the molar solubility of BaF2 in pure water given that the Ksp for BaF2 is 2.45 × 10⁻⁵.
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following is the correct Ksp expression for the compound C2D3 in terms of its molar solubility x?
A
Ksp = 4x^5
B
Ksp = x^3
C
Ksp = x^5
D
Ksp = 2x^3
Verified step by step guidance1
Understand the dissociation of the compound C2D3 in water. When C2D3 dissolves, it breaks into its constituent ions. Assume it dissociates into 2 C ions and 3 D ions.
Write the balanced chemical equation for the dissociation: C2D3(s) ⇌ 2C(aq) + 3D(aq).
Define the molar solubility of C2D3 as x. This means that for every mole of C2D3 that dissolves, x moles of C2D3 dissociate.
Express the concentrations of the ions in terms of x. From the balanced equation, the concentration of C ions will be 2x and the concentration of D ions will be 3x.
Write the Ksp expression using the concentrations of the ions: Ksp = [C]^2[D]^3 = (2x)^2(3x)^3. Simplify this expression to find the correct Ksp formula in terms of x.
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