Question

Calculate the freezing point and boiling point in each solution, assuming complete dissociation of the solute. Part A Calculate the freezing point of a solution containing 12.3 g FeCl3 in 180 g water. Tf = ∘C Request Answer Part B Calculate the boiling point of a solution above. Tb = ∘C Request Answer Part C Calculate the freezing point of a solution containing 4.2 % KCl by mass (in water). Express your answer using two significant figures. Tf = ∘C Request Answer Part D Calculate the boiling point of a solution above. Tb = ∘C Request Answer Part E Calculate the freezing point of a solution containing 0.152 m MgF2. Tf = ∘C Request Answer Part F Calculate the boiling point of a solution above.

Answer #1

Calculate the freezing point and boiling point in each solution,
assuming complete dissociation of the solute
Calculate the freezing point of a solution containing 13.9 g
FeCl3 in 177 g water.
Calculate the boiling point of a solution above
Calculate the freezing point of a solution containing 4.2 % KCl
by mass (in water).
Calculate the boiling point of a solution above
Calculate the freezing point of a solution containing 0.157 m
MgF2
Calculate the boiling point of a solution...

Calculate the freezing point of the following solutions,
assuming complete dissociation. Part A 10.4 g FeCl3 in 151 g water
Part B 3.2 % KCl by mass (in water) Express your answer using two
significant figures. Part C 0.175 m MgF2 Part D Calculate the
boiling point of the solution in part A, assuming complete
dissociation. Part E Calculate the boiling point of the solution in
part B, assuming complete dissociation. Part F Calculate the
boiling point of the solution...

To use freezing-point depression or boiling-point elevation to
determine the molal concentration of a solution.
The freezing point, Tf, of a solution is lower than the
freezing point of the pure solvent. The difference in freezing
point is called the freezing-point depression, ΔTf:
ΔTf=Tf(solvent)−Tf(solution)
The boiling point, Tb, of a solution is higher than the
boiling point of the pure solvent. The difference in boiling point
is called the boiling-point elevation, ΔTb:
ΔTb=Tb(solution)−Tb(solvent)
The molal concentration of the solution, m,...

A solution is made by dissolving 0.579 mol of nonelectrolyte
solute in 891 g of benzene. Calculate the freezing point, Tf, and
boiling point, Tb, of the solution.

A solution is made by dissolving 0.633 mol0.633 mol of
nonelectrolyte solute in 857 g857 g of benzene. Calculate the
freezing point, Tf,Tf, and boiling point, Tb,Tb, of the solution.
Constants can be found in the table of colligative constants.

Assuming complete dissociation of the solute, how many grams of
KNO3 must be added to 275 mL of water to produce a solution that
freezes at −14.5 ∘C? The freezing point for pure water is 0.0 ∘C
and Kf is equal to 1.86 ∘C/m ANSWER=109 g PART B NEEDED: If the
3.90 m solution from Part A boils at 103.45 ∘C, what is the actual
value of the van't Hoff factor, i? The boiling point of pure water
is 100.00...

Part A
10.4 g FeCl3 in 151 g water. Calculate the boiling point of the
solution in part A, assuming complete dissociation.

A solution is made by dissolving 0.726 mol of nonelectrolyte
solute in 857 g of benzene. Calculate the freezing point, Tf, and
boiling point, Tb, of the solution. Constants may be found
here.

A solution is made by dissolving 0.647 mol of nonelectrolyte
solute in 771 g of benzene. Calculate the freezing point, Tf, and
boiling point, Tb, of the solution. Constants may be found
here.

A solution is made by dissolving 0.656 mol of nonelectrolyte
solute in 825 g of benzene. Calculate the freezing point, Tf, and
boiling point, Tb, of the solution. Constants may be found
here.

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