Open Question
Calculate the solubility of in water at. You'll find data in the Aleks data tab.
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
A solution is 0.040 M in Pb²⁺. What minimum concentration of Cl⁻ is required to begin to precipitate PbCl₂? For PbCl₂, Ksp = 1.17×10⁻⁵.
A
8.55×10⁻³ M
B
6.84×10⁻⁴ M
C
1.17×10⁻⁵ M
D
1.71×10⁻² M
Verified step by step guidance1
Understand the concept of solubility product constant (Ksp). Ksp is the equilibrium constant for the dissolution of a sparingly soluble compound. For PbCl₂, the dissolution can be represented as: PbCl₂(s) ⇌ Pb²⁺(aq) + 2Cl⁻(aq).
Write the expression for the solubility product (Ksp) of PbCl₂. The Ksp expression is: .
Substitute the given concentration of Pb²⁺ into the Ksp expression. Since the solution is 0.040 M in Pb²⁺, substitute this value into the expression: .
Rearrange the equation to solve for the concentration of Cl⁻. Isolate [Cl⁻]² by dividing both sides of the equation by 0.040: .
Calculate the minimum concentration of Cl⁻ required to begin precipitation by taking the square root of both sides: . This will give you the minimum concentration of Cl⁻ needed.
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