two solutions are prepared using the same solute
solution a: 0.27g of the solute disolves in 27.4g of t-butanol
solution b: 0.23g of the solute disolves in 24.8g of cyclohexane
which solution has the greatest freesing point change? show calculations and explain.
Robin, I answered this below. Complete with explanation. I poured my heart out and you didn'teven read it? "-)
To determine which solution has the greatest freezing point change, we need to calculate the molality of each solution and compare them.
1. First, we need to calculate the molality (m) for each solution. The formula to calculate molality is:
molality (m) = moles of solute / mass of solvent (kg)
For Solution A:
moles of solute = 0.27g / molar mass of solute
mass of solvent = 27.4g / 1000 (to convert from g to kg)
For Solution B:
moles of solute = 0.23g / molar mass of solute
mass of solvent = 24.8g / 1000
2. Once we have the molality, we can use the freezing point depression formula:
ΔTf = -Kf * m
ΔTf represents the change in freezing point, Kf is the cryoscopic constant for the solvent, and m is the molality.
The solution with the greater ΔTf will have the greater freezing point change.
3. Look up the cryoscopic constant (Kf) for t-butanol and cyclohexane. These values are specific to each solvent.
4. Calculate the ΔTf for each solution using the molality from step 1 and the Kf value for each solvent from step 3.
5. Compare the ΔTf values calculated in step 4. The solution with the greater value has the greatest freezing point change.
By following these steps, you can calculate the molality and compare the ΔTf values for both solutions to determine which solution has the greatest freezing point change.