The following table provides some information on carbon dioxide
solubility in water.
C
(mol/L)
P
(atm)
k
(mol/L⋅atm)
T
(∘C)
3.80×10−2
1.00
20.0
4.90×10−2
20.0
1.00
3.40×10−2
25.0
What is the Henry's law constant for CO2 at 20∘C?
What pressure is required to achieve a CO2 concentration of
4.90×10−2 M at 20∘C?
At 1 atm, how many moles of CO2 are released by raising the
temperature of 1 liter of water from 20∘C to 25∘C?
The following table provides some information on carbon dioxide
solubility in water.
C
(mol/L)
P
(atm)
k
(mol/L⋅atm)
T
(∘C)
3.80×10−2
1.00
20.0
4.90×10−2
20.0
1.00
3.40×10−2
25.0
What is the Henry's law constant for CO2 at 20∘C?
What pressure is required to achieve a CO2 concentration of
4.90×10−2 M at 20∘C?
At 1 atm, how many moles of CO2 are released by raising the
temperature of 1 liter of water from 20∘C to 25∘C?
If the concentration (solubility) of carbon monoxide in water is
0.27 M and the Henry's Law constant for carbon monoxide is 9.5 x
10-4 M/atm, what is the partial
pressure of the gas above the solution?
A solution is prepared by adding 3.65 x 10-3 g of
sodium carbonate to 575 g of water. Find ppb and molality
At
25 C, the vapor pressure of pure water is 23.8 torr. What is the
vapor pressure of an aqueous solution that is 8.00% NaCl by mass?
Assume the NaCl is 100% dissociated.
The water in a shallow lake is at equilibrium with carbon
dioxide in the air. The pH was measured to be 7.0. What is the
alkalinity of the water in mg/L as CaCO3? The partial
pressure of CO2 is 1 X 10-1.5 atm. The
Henry's constant for CO2 is 3.162 X 10-4
moles/(L-atm) at 25oC.
1-propanol (P1° = 20.9 Torr at 25 °C) and 2-propanol (P2° = 45.2
Torr at 25 °C) form ideal solutions in all proportions. Let x1 and
x2 represent the mole fractions of 1-propanol and 2-propanol in a
liquid mixture, respectively, and y1 and y2 represent the mole
fractions of each in the vapor phase. For a solution of these
liquids with x1 = 0.210, calculate the composition of the vapor
phase at 25 °C.
1-propanol (P1° = 20.9 Torr at 25 °C) and 2-propanol (P2° = 45.2
Torr at 25 °C) form ideal solutions in all proportions. Let x1 and
x2 represent the mole fractions of 1-propanol and 2-propanol in a
liquid mixture, respectively, and y1 and y2 represent the mole
fractions of each in the vapor phase. For a solution of these
liquids with x1 = 0.790, calculate the composition of the vapor
phase at 25 °C.
The solubility of CO2 in a salt water lake at 298 K and 750 torr
pressure was found to be 1.0 x 10-5 moles CO2/liter of aqueous
solution. The Henry’s Law constant in this case is 3.0 x 10-2
mol/L.atm.
A) Please find the partial pressure of CO2 (g) (PCO2, in atm) in
the air above the lake.
B) Please use your answer to determine the percentage of CO2 in the
atmosphere.
C) Given the percentage of CO2 in the...
Calculate the molar solubility in pure water for the following
compound at 25°C, Ag2SO3 Ksp =
1.5x10-14
What is the molar solubility in 0.0010 M sodium
sulfite?
What is the equilibrium concentration of carbon dioxide in water
that is in contact with air at 25 °C and 4.53 atm. The mole
fraction of CO2 in air is 3.01×10-4. The Henry's law constant for
carbon dioxide is 4.48×10-5 M/mmHg.