Hey guys I did a lab and I have to answer the questions relating to the lab. I did question 1 & 2, can someone check if they are correct, and question 3 I don't know how to do it.

1. Calculation to Determine the molecular weight of unknown substance

Mass of unknown used: 2.0 g
Mass of water used: 50.0 g (0.05kg)
Kf = 1.86°C kg/mole
Experimentally determined freezing point of unknown: -1°C

Solution = delta Tf/-Kf
= -1°C/-1.86°C kg/mole
= 0.538 m (molality)

Molar mass = 2g / 0.05 kg * 0.538 m
= 74.4 g/mol

2. Calculations to determine i for KCl solution:

Kf = 1.86°C kg/mole
Experimentally determined freezing point of KCl: -1°C
m KCl (given): 0.1 m (molality)

Solution: i = measured delta Tf/ expected delta Tf
= -1°C /-1.86°C kg/mole * 0.1m KCl
i = 5.376

3. Explain why i has this value = ??

The first is correct IF the substance was non ionizing.

The second
calcdeltaT= 1.86*.1=.186C
Measured=1C
= 1/.186=5.376

The thing that strikes me is precision. You measured the freezing point to ONE significant digit, and then did math with it. OUCH.

What if your measured deltaT in the second had been 1.4999, which is in tolerance for your 1 +-.5C measurement.
If it had been 1.49999, then i would have been 5.8, but if delta T had been .5, then i would have been 2.6 This is quite a range, .8 to 2.6. Frankly, I would have expected i to be 2.0 for KCl, which breaks into two ions.

So I attribute your results to lack of precision in measurements.

Do impurities take into account? for #3?

yeah it should be around or less den 2.

i mean the i should be = 2 because it breaks into to ions for KCL and i am getting 1.6. pretty close eh.

To explain why i has a value of 5.376, we need to understand what i represents in this context. In colligative properties, i stands for the van't Hoff factor, which represents the number of particles that a solute molecule dissociates into when it dissolves in a solvent.

In the given question, we are determining the value of i for a KCl solution. KCl is an ionic compound that dissociates into K+ and Cl- ions when it dissolves in water. Thus, each KCl molecule dissociates into two ions.

The experimentally determined freezing point of the KCl solution is -1°C, and the expected freezing point depression (delta Tf) can be determined using the formula:

delta Tf = Kf * m * i

Where Kf is the cryoscopic constant (1.86°C kg/mole), m is the molality of the solution (0.1m), and i is the van't Hoff factor.

Rearranging the formula, we can solve for i:

i = measured delta Tf / (Kf * m)

Substituting the given values:

measured delta Tf = -1°C
Kf = 1.86°C kg/mole
m = 0.1m

i = -1°C / (1.86°C kg/mole * 0.1m)
i = 5.376

Therefore, the value of i for the KCl solution is 5.376. This indicates that each KCl molecule in the solution dissociates into approximately 5.376 ions when it dissolves in water.