Which one of the following liquids will have the highest

freezing point?
A. pure H2O
B. aqueous glucose (0.050 m)
C. aqueous CoI2 (0.030 m)
D. aqueous FeCl3 (0.030 m)
E. aqueous NaI (0.030 m)

Could you please give a step by step process?

To determine which liquid will have the highest freezing point, we need to use the concept of freezing point depression. The freezing point depression is a colligative property that depends on the concentration of solute particles in a solution.

Step 1: Calculate the number of particles in each solution:
A. Pure H2O does not contain any solute particles, so the number of particles is 1.
B. Aqueous glucose (0.050 m) consists of glucose dissolved in water. Glucose is a nonionic compound, so it does not dissociate into ions. Therefore, the number of particles is also 1.
C. Aqueous CoI2 (0.030 m) contains CoI2, which will dissociate into three ions: one Co2+ ion and two I- ions. So, the number of particles is 3.
D. Aqueous FeCl3 (0.030 m) contains FeCl3, which will dissociate into four ions: one Fe3+ ion and three Cl- ions. So, the number of particles is 4.
E. Aqueous NaI (0.030 m) contains NaI, which will dissociate into two ions: one Na+ ion and one I- ion. So, the number of particles is 2.

Step 2: Compare the number of particles. The higher the number of particles, the greater the freezing point depression.

A. Pure H2O has the fewest number of particles (1).
B. Aqueous glucose (0.050 m) also has 1 particle.
C. Aqueous CoI2 (0.030 m) has 3 particles.
D. Aqueous FeCl3 (0.030 m) has 4 particles.
E. Aqueous NaI (0.030 m) has 2 particles.

Step 3: The greater the concentration of solute particles, the higher the freezing point depression. Therefore, the liquid with the highest freezing point will be the one with the highest number of particles.

So, the liquid with the highest freezing point will be D. aqueous FeCl3 (0.030 m), as it has the highest number of particles (4) among the given options.

To determine which of the liquids will have the highest freezing point, we need to consider the concept of freezing point depression, which states that the presence of solutes in a liquid lowers its freezing point.

Here is a step-by-step process to determine the liquid with the highest freezing point:

Step 1: Understand the concept.
Freezing point depression occurs when a solute is added to a solvent, reducing the solvent's vapor pressure and therefore lowering the temperature at which it freezes.

Step 2: Compare the solutions.
We are given five options:

A. pure H2O
B. aqueous glucose (0.050 m)
C. aqueous CoI2 (0.030 m)
D. aqueous FeCl3 (0.030 m)
E. aqueous NaI (0.030 m)

Step 3: Analyze the solutions.
The solutions in options B, C, D, and E all have solutes dissolved in the water, which will lead to freezing point depression and a lower freezing point compared to pure water.

Step 4: Compare the concentrations.
Now, we need to compare the concentrations of the solutes in each solution: 0.050 m for glucose, 0.030 m for CoI2, 0.030 m for FeCl3, and 0.030 m for NaI.

Step 5: Apply the concept of colligative properties.
Colligative properties, like freezing point depression, depend only on the number of solute particles in a solution, not their identity. Therefore, we can compare the solutions based on their molar concentrations.

Step 6: Determine the highest freezing point.
Since all four solutions (glucose, CoI2, FeCl3, and NaI) have the same concentration (0.030 m), their freezing point depressions will be the same. However, NaI is an ionic compound and will split into two particles (Na+ and I-) when dissolved, while the other solutes (glucose, CoI2, and FeCl3) remain undissociated. Hence, NaI will have the highest freezing point because it produces more solute particles, resulting in a greater depression of the freezing point.

Therefore, the answer is E. aqueous NaI (0.030 m).

delta T = i*Kf*m

i = 1 for glucose
i = 3 for CoCl2
i = 4 for FeCl3
i = 2 for NaI
(i = van't Hoff factor which is the number of particles in soln). But you really don't need any of that stuff above to answer the question.
Note that pure water freezes at 0 C. ALL solutes will lower the freezing point so B, C, D, and E will lower the freezing point from zero C. The highest freezing point will be .....?
Or you can forget reasoning and solve each of the above equations to determine how much each will be changed.