Multiple Choice
Given a solution containing Ca^{2+} at 2.00 imes 10^{-2} ext{ M} and CrO_4^{2-} at 3.00 imes 10^{-2} ext{ M}, what is the value of the reaction quotient Q for the precipitation of CaCrO_4?
17
views
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
What is the molar solubility of PbBr2 in pure water? Ksp for PbBr2 is 4.67 × 10−6.
A
1.05 × 10−2
B
1.67 × 10−2
C
1.08 × 10−3
D
2.18 × 10−3
E
4.67 × 10−6
Verified step by step guidance1
Write the dissolution equation for PbBr2: PbBr2(s) ⇌ Pb²⁺(aq) + 2Br⁻(aq).
Define the molar solubility of PbBr2 as 's'. This means that at equilibrium, the concentration of Pb²⁺ will be 's' and the concentration of Br⁻ will be '2s'.
Write the expression for the solubility product constant (Ksp) for PbBr2: Ksp = [Pb²⁺][Br⁻]².
Substitute the equilibrium concentrations into the Ksp expression: Ksp = (s)(2s)² = 4s³.
Set the Ksp expression equal to the given Ksp value and solve for 's': 4s³ = 4.67 × 10⁻⁶. Solve for 's' to find the molar solubility.
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