Question
In: Chemistry
9.537 g of a non-volatile solute is dissolved in 220.0 g of water. The solute does...
9.537 g of a non-volatile solute is dissolved in 220.0 g of
water.
The solute does not react with water nor dissociate in
solution.
Assume that the resulting solution displays ideal Raoult's law
behaviour.
At 25°C the vapour pressure of the solution is 23.498
torr.
The vapour pressure of pure water at 25°C is 23.756
torr.
Calculate the molar mass of the solute (g/mol).
71.1 g/mol
Now suppose, instead, that 9.537 g of a volatile
solute is dissolved in 220.0 g of water.
This solute also does not react with water nor dissociate in
solution.
The pure solute displays, at 25°C, a vapour pressure of 2.376
torr.
Again, assume an ideal solution.
If, at 25°C the vapour pressure of this solution is also 23.498
torr.
Calculate the molar mass of this volatile solute.
Solutions
queen_honey_blossom answered 7 months agoRelated Solutions
16.636 g of a non-volatile solute is dissolved in 410.0 g of water. The solute does...
16.636 g of a non-volatile solute is dissolved in 410.0 g of
water.
The solute does not react with water nor dissociate in
solution.
Assume that the resulting solution displays ideal Raoult's law
behaviour.
At 90°C the vapour pressure of the solution is 517.01 torr.
The vapour pressure of pure water at 90°C is 525.80
torr. The molar mass of the solute is 43.0
g/mol.
Now suppose, instead, that 16.636 g of a volatile
solute is dissolved in 410.0 g of...
Vapour Pressure of Solutions of Non-Volatile or Volatile Solutes 22.555 g of a non-volatile solute is...
Vapour Pressure of Solutions of Non-Volatile or Volatile Solutes
22.555 g of a non-volatile solute is dissolved in 215.0 g of water.
The solute does not react with water nor dissociate in solution.
Assume that the resulting solution displays ideal Raoult's law
behaviour. At 10°C the vapour pressure of the solution is 9.073
torr. The vapour pressure of pure water at 10°C is 9.209 torr.
Calculate the molar mass of the solute (g/mol). See example 17.1 on
pp865-6 of Zumdahl...
When 2.13 g of a nonelectrolyte solute is dissolved in water to make 395 mL of...
When 2.13 g of a nonelectrolyte solute is dissolved in water to
make 395 mL of solution at 21 °C, the solution exerts an osmotic
pressure of 959 torr. What is the molar concentration of the
solution? How many moles of solute are in the solution? What is the
molar mass of the solution?
When 2.14 g of a nonelectrolyte solute is dissolved in water to make 165 mL of...
When 2.14 g of a nonelectrolyte solute is dissolved in water to
make 165 mL of solution at 22 °C, the solution exerts an osmotic
pressure of 821 torr.
a solution is made by mixing 1.08 g of an unknown non-volatile non-electrolyte with 10.0 g...
a solution is made by mixing 1.08 g of an unknown non-volatile
non-electrolyte with 10.0 g of benzene. The freezing point of pure
benzene is is 5.5 degrees Celsius. The molal freezing point
depression constant, Kf, for benzene is 5.12 degrees Celsius per
molale.
What is the value of the freezing point depression? What is the
molality of the solution? What is the molar mass of the
unknown?
1) When 2.69g of a nonelectrolyte solute is dissolved in water to make 655 mL of...
1) When 2.69g of a nonelectrolyte solute is dissolved in water
to make 655 mL of solution at 23 C, the solution exerts an osmotic
pressure of 877 torr.
What is the molar concentration of the solution?
How many moles of solute are in the solution?
What is the molar mass of the solute?
2) Biphenyl, C12H10, is a nonvolatile, nonionizing solute that
is soluble in benzene, C6H6
At 25 ∘C, the vapor pressure of pure benzene is 100.84 Torr....
What is the mechanism by which solute is dissolved in non polar solvents? Explain briefly. (5...
What is the mechanism by which solute is dissolved in non polar
solvents? Explain briefly. (5 mark)
A solution contains 12.00 g of unknown compound (non-electrolyte) dissolved in 50.0 mL of water. (Assume...
A solution contains 12.00 g of unknown compound
(non-electrolyte) dissolved in 50.0 mL of water. (Assume a density
of 1.00 g/mL for water.) The freezing point of the solution is
-4.95 ∘C. The mass percent composition of the compound is 53.31% C,
11.19% H, and the rest is O. Part A What is the molecular formula
of the compound? Express your answer as a molecular formula.
If 17.5 g of NaCl is dissolved in 100. g of water, what is the mass...
If 17.5 g of NaCl is dissolved in 100. g of water, what is the
mass % concentration of NaCl in this solution?
Note:
1. Use 3 sig figs for your final answer.
2. Do not answer as fractions. For example, if you think 30% is
the correct answer, either "30" or "30%" will be accepted, but
"0.30" will not. "30%" will actually be converted to 30
automatically
When 1.31 g of an unknown non-electrolyte is dissolved in 50.0 g of acetone, the freezing...
When 1.31 g of an unknown non-electrolyte is dissolved in 50.0 g
of acetone, the freezing point decreased to -94.1 degrees C from
-93.4 degrees C. If the Kfp of the solvent is 2.4 K/m, calculate
the molar mass of the unknown solute
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