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What is the BEST explanation for the observation that 1.0 M HCl(aq) has a greater boiling point than 1.0 M HF(aq)?
A. HCl has a greater molecular mass than HF, so the molality of the HCl solution is greater than the molality of the HF solution.
B. HCl has a greater molecular mass than HF, so the molality of the HCl solution is less than the molality of the HF solution.
C. HCl does not dissociate completely in water, while HF does.
D. HF does not dissociate completely in water, while HCl does.
D is the best answer. Choices A and B can be eliminated immediately, because even though HCl has a greater molecular mass than HF, the solutions have the same molarity (which is based on moles of solute, not grams of solute). That means the two solutions have approximately the same molality.
If two solutions have the same molarity, then they have the same molality? Is that true in all cases?
A. HCl has a greater molecular mass than HF, so the molality of the HCl solution is greater than the molality of the HF solution.
B. HCl has a greater molecular mass than HF, so the molality of the HCl solution is less than the molality of the HF solution.
C. HCl does not dissociate completely in water, while HF does.
D. HF does not dissociate completely in water, while HCl does.
D is the best answer. Choices A and B can be eliminated immediately, because even though HCl has a greater molecular mass than HF, the solutions have the same molarity (which is based on moles of solute, not grams of solute). That means the two solutions have approximately the same molality.
If two solutions have the same molarity, then they have the same molality? Is that true in all cases?