Assuming equal concentrations and complete dissociation, rank these aqueous solutions by their freezing points.

CoCl3 K2CO3 KNO3

The equation is delta T = i*Kf*m

i = van't Hoff factor which is the number of particles. CoCl3 is 4, K3CO3 is 3, KNO3 is 2.
Kf is a constant
The problem tells you m is constant, so.....

DrBob222,

you put K3CO3 not K2CO3

Highest freezing point:

KNO3
K2SO4
CoCl3
Lowest freezing point

To rank these aqueous solutions by their freezing points, we need to consider their effect on the colligative properties, specifically the freezing point depression caused by the presence of solute particles.

Freezing point depression occurs when solute particles are added to a solvent, disrupting the formation of regular crystalline structures and causing the freezing point of the solution to be lower than that of the pure solvent.

In this case, assuming equal concentrations and complete dissociation, we need to compare the number of particles that each compound produces when dissolved in water.

1. CoCl3: Cobalt(III) chloride (CoCl3) dissociates into one cobalt ion (Co3+) and three chloride ions (Cl-) in solution. So, it produces a total of four solute particles in water.

2. K2CO3: Potassium carbonate (K2CO3) dissociates into two potassium ions (2 K+) and one carbonate ion (CO3^2-) in solution. Hence, it produces a total of three solute particles in water.

3. KNO3: Potassium nitrate (KNO3) dissociates into one potassium ion (K+) and one nitrate ion (NO3-) in solution. It produces a total of two solute particles in water.

Based on the number of solute particles produced, we can conclude that CoCl3 has the highest number of particles, followed by K2CO3, and then KNO3.

Therefore, the ranking of these aqueous solutions by their freezing points, from highest to lowest, would be:
1. CoCl3
2. K2CO3
3. KNO3