A 0.5 molal urea solution causes freezing point depression of two degrees .what is the molal delression constant ????
delta T = i*Kf*m
2 = 1*Kf*0.5
Solve for Kf.
I wanna solve...
To calculate the molal depression constant (Kf), we can use the formula:
ΔTf = Kf * molality
Given that the solution causes a freezing point depression (ΔTf) of 2 degrees and the molality is 0.5 molal, we can rearrange the formula to solve for Kf:
Kf = ΔTf / molality
Substituting the values into the formula:
Kf = 2 degrees / 0.5 molal
Kf = 4 molal degrees (or mol·kg⁻¹·°C⁻¹)
Therefore, the molal depression constant (Kf) is 4 molal degrees (or mol·kg⁻¹·°C⁻¹).
To find the molal depression constant, we can use the formula for freezing point depression:
ΔT = Kf * m
Where:
ΔT is the freezing point depression in degrees Celsius,
Kf is the molal depression constant, and
m is the molality of the solute.
In this case, we are given that a 0.5 molal urea solution causes a freezing point depression of 2 degrees Celsius. We need to find Kf, the molal depression constant.
Rearranging the formula, we get:
Kf = ΔT / m
Plugging in the given values, we have:
Kf = 2 degrees Celsius / 0.5 molal
Simplifying the expression, we find:
Kf = 4 degrees Celsius/molal
Therefore, the molal depression constant for the given urea solution is 4 degrees Celsius/molal.