Question

A
1% w/v solution of drug X had a freezing point depression of 0.92
Celsius. At what percent strength of drug X isotonic? Use 2 sig
figs

Answer #1

The freezing point depression of a solution of nitrobenzene and
a nonionic unknown was used to determine the molar mass of the
unknown. Time-temperature data for the cooling of nitrobenzene and
for the cooling of a solution containing 50.0 g of nitrobenzene and
5.00 mL of a nonionic liquid unknown. Density of the unknown is
0.714 g mL^-1. And the Kf of nitrobenzene is 6.87 degrees C Kg
mol^-1.
What is the freezing point of the unknown solution? I
know...

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,...

Benzene has a normal freezing point of 5.50°C and a molal
freezing point depression constant of 5.12°C/m. A solution prepared
by dissolving 0.335g of compound X in 5.00g of benzene has a
freezing point of 1.34°C. Assuming that compound X is a
nonelectrolyte, what is the molar mass of compound X?

Molar Mass Determination by Freezing Point Depression
Calculate and enter the freezing point
depression of a solution of 74.2 g ethylene glycol
(C2H6O2) in 422 g
H2O.
Kf for H2O is 1.86 °C kg/mol.
°C
1homework pts
Incorrect.
Tries 2/5
Previous Tries
A solution which contains 57.1 g of an unknown molecular
compound in 383 g of water freezes at -5.32°C.
What is the molar mass of the unknown?
g/mol

Freezing Point Depression Lab
Objective: To use freezing point to determine the molecular
weight of an unknown substance.
In this lab, we used benzophene as the solvent, which has a
freezing point of 48.1 degrees celsius and Kf value of 9.80 degrees
C/m. The procedure consisted of measuring out 10 g benzophenone in
a test tube and melting the substance in a warm water bath. When
melted, we removed the test tube from the bath and allowed it to
cool....

A sample of acetic acid solution has a freezing point depression
of 2.0 C. What is the e estimated percent by mass of acetic acid in
the acetic acid solution? Molar mass of acetic acid
C2H3O2=60g/mol.

How many mol of NaOH are in 0.55 mL of 25%w/v NaOH solution?
(Report your answer to 2 sig figs.)

5. Determine the molal freezing point depression constant (Kf)
(in °C⋅kg/mol) of water by using the data of three NaCl solutions .
Use Equation 3 in the “Background and Procedure” file, the molality
values of all solutes from Question s 1 – 3 and the freezing point
depression ( ∆T) from Question 4. In your calculation, rewrite the
symbol“m ” (the molality) as “mol/kg” so that the molal freezing
point depression constant will have the correct unit. Make
sure to...

A certain substance X has a normal freezing point of -6.4 C and
a molal freezing point depression constant Kf= 3.96
degrees C.kg.mol-1. A solution is
prepared by dissolving some urea ((NH2)2CO)
in 950. g of X. This solution freezes at -13.6 C. calculate the
mass of urea that was dissolved. Round your answer to 2 significant
digits.

The freezing point depression constant tells how the temperature
changes for a 1 molal concentration of solute. If camphor is
dissolved in cyclohexane so that the concentration is 1.5 molal,
what is the freezing point of the solution? (See Table in lab
procedure for Kf values.)
What are the five major steps in this experiment? a.
b. c. d. e.
An important hazard of cyclohexane is
__________________________________. How will you know if the solute
is completely dissolved?
Howdoyoucleanupthetesttubeattheendoftheexperiment?
4. 5....

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