Multiple Choice
Which of the following ionic salts is generally soluble in water according to solubility rules?
6. Chemical Quantities & Aqueous Reactions
Solubility Rules
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What is the solubility of M(OH)₂ in a 0.202 M solution of M(NO₃)₂, given that M(OH)₂ is sparingly soluble in water?
A
M(OH)₂ is completely soluble in the solution.
B
M(OH)₂ is sparingly soluble in the solution.
C
M(OH)₂ is highly soluble in the solution.
D
M(OH)₂ is insoluble in the solution.
Verified step by step guidance1
Identify the chemical equilibrium involved: M(OH)₂ dissociates in water to form M²⁺ and OH⁻ ions. The equilibrium expression for the solubility product (Ksp) is Ksp = [M²⁺][OH⁻]².
Recognize that the presence of M(NO₃)₂ in the solution provides a common ion effect due to the M²⁺ ions already present in the solution, which affects the solubility of M(OH)₂.
Set up the expression for the solubility of M(OH)₂ in terms of its molar solubility, s. In the presence of the common ion, the concentration of M²⁺ is (0.202 + s) M, but since s is small, it can be approximated as 0.202 M.
Write the Ksp expression using the approximation: Ksp = (0.202)[OH⁻]². Solve for [OH⁻] in terms of s, where [OH⁻] = 2s.
Substitute the expression for [OH⁻] back into the Ksp equation and solve for s, the solubility of M(OH)₂ in the 0.202 M M(NO₃)₂ solution.
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