Two solutions: 2 mols acetic acid in 2000 g water, 2 mols acetic acid in 2000 g ammonia. Passage states that weak acids MAY (not "do") ionize completely in ammonia, unlike in water, but whatever, let's say acetic acid does. Kf for water is roughly, but under, twice the Kf for ammonia. Is the freezing point depression less in the first solution or in the second?
They claim it's less in the water solution, since it dissociates to a hugely less degree than 100%, which they somehow assume happens in NH3. Even if it didn't dissociate at all in water, and it dissociates completely in NH3, shouldn't you just multiply the molality for the NH3 solution by 2, making it roughly equal, and basically impossible to answer this question, since the Kf for water is roughly double? Or am I wrong here?
They claim it's less in the water solution, since it dissociates to a hugely less degree than 100%, which they somehow assume happens in NH3. Even if it didn't dissociate at all in water, and it dissociates completely in NH3, shouldn't you just multiply the molality for the NH3 solution by 2, making it roughly equal, and basically impossible to answer this question, since the Kf for water is roughly double? Or am I wrong here?
