3. Which aqueous solution would you expect to have the lowest freezing point?
0.10 molal glucose, C6H12O6 or 0.10 molal NaCl solution
delta T = i*Kf*m
i = van't Hoff factor = 1 for glucose
i = 2 for NaCl.
m is the same, Kf is the same;the only difference is i so ......is the lowest.
To determine which aqueous solution would have the lowest freezing point, we can use the concept of freezing point depression. When a solute is added to a solvent, it lowers the freezing point of the resulting solution compared to the pure solvent.
The extent of freezing point depression depends on the concentration of the solute particles in the solution. In general, ionic compounds, like NaCl, dissociate into multiple ions when dissolved in water. This leads to a greater number of solute particles and hence a larger freezing point depression.
On the other hand, glucose, C6H12O6, is a non-ionic solute and does not dissociate into ions when dissolved in water. This means that it will not produce as many solute particles as NaCl for the same concentration. Consequently, the freezing point depression caused by glucose will be relatively smaller compared to the same concentration of a ionic compound like NaCl.
Therefore, the 0.10 molal NaCl solution would be expected to have the lowest freezing point among the two aqueous solutions.