Question

At 288 K, the vapor pressure of pure water is 12.79 mmHg and
that of seawater is 12.51 mmHg. Assuming that seawater contains
only NaCl, estimate its concentration (in mol/L). (*Hint*:
Sodium chloride is a strong electrolyte. The density of water at
this temperature is 0.99910 g·cm^{−3}.)

Answer #1

An aqueous CaCl2 solution has a vapor pressure of 84.0 mmHg at
50 ∘C. The vapor pressure of pure water at this temperature is 92.6
mmHg. Part A What is the concentration of CaCl2 in mass
percent?

What is the vapor pressure in mmHg of a solution made by
dissolving 12.5 g of NaCl in 500.0 g of water at 70°C, assuming a
van't Hoff factor of 1.9? The vapor pressure of pure water at 70°C
is 233.7 mmHg. watch for sig figs

At 27 degrees Celcius, the vapor pressure of pure water is 23.76
mmHg and that of an aqueous solution of urea 22.95 mmHg. Calculate
the molality of urea in the solution.

15 OC, where the pure vapor pressures are 12.5 mmHg
for water and 32.1 mmHg for ethanol. According to Raoult’s Law, the
pressure of a component in a solution is equal to its pure vapor
pressure times its mole fraction, that is PA = ()
(XA). Use Raoult’s law to determine the vapor pressure
of each component in the solution. Then, add them to find the total
vapor pressure. Show all equations and conversion factors

An aqueous CaCl2 solution has a vapor pressure of 80.8 mmHg at
50 ∘C. The vapor pressure of pure water at this temperature is 92.6
mmHg. What is the concentration of CaCl2 in mass percent?
I have done this multiple times and always get 47% but my prof
insists it is 23%. Could someone post a step by step so I can
compare my calculations? Thank you!

The vapor pressure of pure water is 0.0317 bar and the vapor
pressure of acetone is 0.309 bar at 25C. What is the vapor pressure
of a solution having a concentration of acetone = 0.400?

An isotonic solution will produce an osmotic pressure of 7.84
atm measured against pure water at human body temperature (37.0°C).
How many grams of sodium chloride must be dissolved in a liter of
water to produce an isotonic solution? (molar mass NaCl = 58.44
g/mol; molar mass H2O = 18.01 g/mol)

The
vapor pressure of water at 45.0 degrees C is 71.93 mmHg. What is
the vapor pressure of water over a solution prepared from 75.0 g of
citric acid (C6H8O7) (a nonelectrolyte) in 0.420 kg of water at
this temperature?

1. A solution of sodium chloride in water has a vapor pressure
of 19.6 torr at 25ºC. What is the mole fraction of solute particles
in this solution? What would be the vapor pressure of this solution
at 45ºC? The vapor pressure of pure water is 23.8 torr at 25ºC and
71.9 torr at 45ºC, and assume sodium chloride exists as Na+ and Cl-
ions in solution.

a) the pressure of pure water vapor at 25 ° C equals 23.758,
if the total pressure on the liquid is only due to water vapor,
calculate the vapor pressure of water at 25 ° C if enough gaseous
oxygen is added Steam to give a total pressure of 1,000atm.
Consider that oxygen does not dissolve in water.
b) Calculate the molar fraction of oxygen dissolved in the
water under the conditions of part a. The constant for Henry's law...

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