Multiple Choice
What is the minimum concentration of sulfate ions (SO₄²⁻) required to cause precipitation of calcium ions (Ca²⁺) from a 9.0×10⁻² M CaI₂ solution, given that the Ksp of CaSO₄ is 2.4×10⁻⁵?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Determine the molar solubility of Fe(OH)₂ in pure water given that the Ksp for Fe(OH)₂ is 4.87 × 10⁻¹⁷.
A
2.34 × 10⁻⁸ M
B
4.87 × 10⁻¹⁷ M
C
9.74 × 10⁻⁹ M
D
1.23 × 10⁻⁶ M
Verified step by step guidance1
Start by writing the balanced chemical equation for the dissolution of Fe(OH)₂ in water:
Define the expression for the solubility product constant (Ksp) for Fe(OH)₂. The Ksp expression is based on the concentrations of the ions in solution:
Let the molar solubility of Fe(OH)₂ be 's'. Then, the concentration of Fe²⁺ ions in solution will be 's', and the concentration of OH⁻ ions will be '2s' because two OH⁻ ions are produced for each formula unit of Fe(OH)₂ that dissolves.
Substitute the concentrations into the Ksp expression:
Solve the equation for 's' by substituting the given Ksp value (4.87 × 10⁻¹⁷) and simplifying the expression:
1:47mWatch next
Master Solubility Product Constant with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Solubility Product Constant: Ksp practice set
Problem sets built by lead tutorsExpert video explanations