객관식
What concentration of hydroxide ions (OH-) is needed to begin the formation of Pb(OH)2 in a solution with a [Pb2+] of 4.5 x 10^-5 M, given that the solubility product constant (Ksp) of Pb(OH)2 is 8.0 x 10^-15?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Which of the following is the correct solubility product expression (Ksp) for magnesium phosphate, Mg3(PO4)2, when it dissociates in water?
A
Ksp = [Mg^2+]^3[PO4^3-]^2
B
Ksp = [Mg^3+][PO4^2-]
C
Ksp = [Mg^2+]^2[PO4^3-]^3
D
Ksp = [Mg^2+][PO4^3-]
검증된 단계별 안내1
Identify the chemical formula of magnesium phosphate, which is Mg3(PO4)2.
Understand that the solubility product expression (Ksp) is based on the equilibrium concentrations of the ions produced when the compound dissociates in water.
Write the dissociation equation for magnesium phosphate: Mg3(PO4)2 (s) ⇌ 3 Mg^2+ (aq) + 2 PO4^3- (aq).
Based on the dissociation equation, determine the stoichiometry of the ions: 3 moles of Mg^2+ ions and 2 moles of PO4^3- ions are produced per mole of Mg3(PO4)2 that dissolves.
Construct the Ksp expression using the stoichiometry: Ksp = [Mg^2+]^3[PO4^3-]^2, where the exponents correspond to the coefficients of the ions in the balanced dissociation equation.
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