Enthalpy of solution, hydration and solubility Quiz
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5 questions, one answer each
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1. Which equation represents the enthalpy change of hydration of the bromide ion?
- A. Br⁻(aq) → Br⁻(g) + aq
- B. Br⁻(g) + aq → Br⁻(aq)
- C. ½Br₂(l) + e⁻ + aq → Br⁻(aq)
- D. KBr(s) + aq → K⁺(aq) + Br⁻(aq)
2. The lattice energy of a salt AB is −650 kJ mol⁻¹. ΔhydH(A⁺) = −400 and ΔhydH(B⁻) = −300 kJ mol⁻¹. What is ΔsolH?
- A. +50 kJ mol⁻¹
- B. −1350 kJ mol⁻¹
- C. +1350 kJ mol⁻¹
- D. −50 kJ mol⁻¹
3. Which ion has the most exothermic enthalpy change of hydration?
- A. Mg²⁺
- B. K⁺
- C. Na⁺
- D. Ba²⁺
4. Why does the solubility of Group 2 sulfates decrease down the group?
- A. The lattice energy becomes much more exothermic
- B. The sulfate ion becomes smaller
- C. The cation hydration enthalpy becomes less exothermic by more than the lattice energy changes
- D. The activation energy increases
5. A salt has a positive ΔsolH but dissolves in water. What must be true?
- A. ΔSsurroundings is positive
- B. ΔSsystem is positive and large enough to make ΔStotal positive
- C. The lattice energy is positive
- D. The hydration enthalpies are zero