four flasks each contain 100 milliliters of aqueous solutions equal concentrations at 25 degress C and 1 atm. the four flasks are KCL,CH3OH, Ba(OH)2, and CH3COOH.
the question is Which solution had the lowest freezing point and explain answer

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  1. delta T = i*Kb*molality.
    You CAN calculate delta T for all four, then you will know quantitatively which is the lowest (actually you can't because concn is not given). BUT, you can do it the easy way. You won't know exactly what the freezing point is but you will know which is the lowest. To do it the easy, note that Kb is the same for all and the volume is the same for all, the pressure is the same for all, concentrations are the same for all. So the only thing different is the i, which is the number of particles formed when the compounds ionize. KCl forms two (K^+ and Cl^-), CH3OH doesn't ionize so it has 1, etc. The one with the most particles has the lowest freezing point because delta T will be the greatest.

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