Multiple Choice
The equilibrium constant for the reaction 2NO(g) + Br2 ⇌ 2NOBr(g) is Kc = 2.0 × 10⁻² at a certain temperature. Calculate Kc for the reverse reaction NOBr(g) ⇌ NO(g) + 1/2Br2(g).
16. Chemical Equilibrium
Equilibrium Constant Calculations
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In a solution at equilibrium with both PbSO4 and SrSO4, what is the relationship between the concentrations of [SO4^2-], [Pb^2+], and [Sr^2+]?
A
[SO4^2-] = [Pb^2+] = [Sr^2+]
B
[SO4^2-] is determined by the solubility product constants of PbSO4 and SrSO4
C
[SO4^2-] = [Pb^2+] + [Sr^2+]
D
[SO4^2-] is independent of [Pb^2+] and [Sr^2+]
Verified step by step guidance1
Understand that the problem involves a solution at equilibrium with both PbSO4 and SrSO4, which are sparingly soluble salts.
Recall the concept of solubility product constant (Ksp), which is used to describe the equilibrium between a solid and its ions in a saturated solution.
Write the equilibrium expressions for the dissolution of PbSO4 and SrSO4: PbSO4(s) ⇌ Pb^2+(aq) + SO4^2-(aq) and SrSO4(s) ⇌ Sr^2+(aq) + SO4^2-(aq).
Express the solubility product constants for each salt: Ksp(PbSO4) = [Pb^2+][SO4^2-] and Ksp(SrSO4) = [Sr^2+][SO4^2-].
Recognize that the concentration of [SO4^2-] is influenced by both Ksp values, and thus, [SO4^2-] is related to the sum of [Pb^2+] and [Sr^2+], leading to the relationship: [SO4^2-] = [Pb^2+] + [Sr^2+].
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