Which one of the following aqueous solutions has a freezing point of –2.60°C? (Kf for water is 1.86°C/m)?
Which one of the following aqueous solutions has a freezing point of –2.60°C? (Kf for water is 1.86°C/m)
A. 1.30 m Na2CO3(aq)
B. 0.47 m NaBr(aq)
C. 0.20 m K2SO4(aq)
D. 0.35 m AlCl3(aq)
E. 0.24 m CH3OH (aq)
How do I solve this problem using change in temperature= H freezing times molality?
Can you please show me the work?
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Verified answer
(2.60 °C change) / (1.86 °C/m) = 1.3978 m
So you're looking for the solution that is 1.4 m in ions.
A. 1.30 m x 3 = 3.9 m , so that's wrong
B. 0.47 m x 2 = 0.94 m, so that's wrong
C. 0.20 m x 3 = 0.60 m, so that's wrong
D. 0.35 m x 4 = 1.40 m, so that's correct
E. 0.24 m x 1 = 0.24 m, so that's wrong