Question

A. If an aqueous solution is prepared with molality= 4.58 moles of glycerine/100 kg water, calculate the freezing point of the solution. Kf for water = 1.86C/m. (Glycerine is a molecular solute)

b. if an aqueous solution is prepared with molality = 8.21 moles of magnesium chloride/100kg water, calculate the freezing point of the solution. Note : the ionic formula of this salt is MgCl2.

C. Calculate the boiling pointof the solution described in question 2b. Given Kb for water=0.520C/m.

Answer #1

A solution is prepared by mixing 12.0g of unknown electrolyte
with 80.0g of water. The solutions freezes at -1.94C. The freezing
point of pure water is 0.0C. the value of Kf for water is
1.86C/m.
a) what is the molality of the solution?
b)what are the moles of unknown electrolyte in the solution?
c)what is the molecular weight of the unknown?

What is the normal boiling point of an aqueous solution that has
a freezing point of 1.04 oC. Kf for water 1.86 oC/m (oC-kg/mol).
Hint: Calculate the molality from the freezing point depression and
use it to calculate the normal boiling point.

Calculate the freezing point and boiling point of aqueous 1.9 m
CuCl3 given Kf for water = 1.86 deg.C/m; Kb for water = 0.512 deg
C/m. Assume theoretical value for i. Show work for credit.

1.The freezing point of an aqueous solution prepared by adding
0.0100 mol of acetic acid to 100. g of water is -0.190 C. The
freezing point depression of pure water is 0.000 C, and the
freezing point depression constant for water is 1.86 C/m. What is
the value for the van't Hoff factor for acetic acid in the aqueous
solution. You must show work to support your response.
2. Which of the following aqueous solutions should have the
lowest freezing...

The osmotic pressure of an aqueous solution at 300K is 250.0
kPa. (1)Calculate the molarity of solute (impurity) M
(mol/m3)=; (2) Calculate the molality of solute
(impurity) b (mol/kg)=; Calculate the freezing point of the
solution T(oC)=. Please pay attention to the sign. The
cryoscopicconstant Kf=1.86Kkgmol-1. Please enter your
answers with 2 decimals. for example, 3.02466 is written as
3.02.

what is the freezing point of an aqueous 200m (NH4)PO4 salt
solution? The Kf of water 1.86 C/m. Assume complete dissociation of
the soluble salt.

Please answer only if you 100% know and it has to be all of
them! Please show work neatly!!! :)Thanks!
1. Calculate the molarity, molality and mass % of NH3 in a
solution in which 60.0g of NH3 are dissolved in 140.0g of water.
The Density of this solution is 0.982g/mL
2. A solution is prepared by dissolving 38.0g of non-volatile
molecular solute in 125 grams of benzene. The boiling point of this
solution is 84.5C (Celsius) and the boiling...

A solution contains 221 grams of calcium chloride in 600
millimeters of water. For the solvent the Kf is 1.86 and Kb is
0.51. What the should the boiling point and the freezing point of
the solution be?

A solution is made by dissolving 2.04 g of KBr in 188 g of
water. The kf of water is 1.86 oC/m, the
kb of water is 0.51 oC/m.
Calculate the freezing point
Calculate the boiling point

must show all work. Observe sig fig rules and include units.
1) In a lab three determinations were made for
the freezing point of an unknown liquid. The values obtained were:
25.1°C, 25.9°C and 25.4°C. Calculate the average and Standard
Deviation.
2) Compound X was dissolved in
water. The freezing point of this solution was determined to be
-0.072°C.
a) Calculate the
ΔTf
? (Freezing Point of water is
0.00°C)
b) Calculate the molality of the
solution? (Kf
for water...

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