Question

The solubility of the salt MxAy is 1.0 ´ 10-2 mol/L at 25°C. The osmotic pressure exhibited by a solution saturated with MxAy at 25°C is 1.22 atm. Determine the values of x and y by assuming ideal behavior.

Answer #1

At 25 ?C, the osmotic pressure of a solution of the salt XY is
60.8torr . What is the solubility product of XY 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. Please find the partial pressure of CO2 (g) (PCO2, in
atm) in the air above the lake (2) Please use your answer to
determine the percentage of CO2 in the atmosphere (2) Given the
percentage of CO2 in the atmosphere...

The solubility of oxygen, O2, in water is 7.20 ✕ 10−4 mol/L at
0°C when the nitrogen pressure above water is 0.554 atm. Calculate
the solubility of oxygen in water when the partial pressure of
oxygen above water is 1.083 atm at 0°C? The Henry's Law constant
for oxygen is 1.30 ✕ 10−3 mol/ L atm.

The molar solubility of Cd3(PO4)2 is 1.19×10-7 mol/L at
25°C.
Calculate the solubility of Cd3(PO4)2 at 25°C._____g/L.
Calculate Ksp at 25°C._______

1) At 25 °C, only 0.0670 mol of the generic salt AB is soluble
in 1.00 L of water. What is the ?sp of the salt at 25 °C?
AB(s)↽−−⇀A+(aq)+B−(aq)
2) A generic salt, AB3AB3, has a molar mass of 173173 g/mol and
a solubility of 1.601.60 g/L at 25 °C.
What is the ?spKsp of this salt at 25 °C?
AB3(s)↽−−⇀A3+(aq)+3B−(aq)
3)The ?spKsp of manganese(II) hydroxide, Mn(OH)2, is
2.00×10−132.00×10−13. Calculate the solubility of this compound in
grams per liter....

A) The solubility of neon gas in water at 25°C is 1.05x10-3 M when
the pressure of the Ne above the solution is 1.0 atm. the
solubility of Ne (g) is?
B) the vapor pressure of pure ethanol at 60°C is 0.459 atm.
Raoult's law predicts that a solution prepared by dissolving 10.0
mmol naphthalene in 90.0 mmol ethanol will have a vapor pressure
of?

The osmotic pressure of 100.0 mL of a 25 C solution containing
0.50 g of a protein is 5.8 Torr. Based on this information,
determine the molar mass of the protein in g/mol.
Hint: The protein does not dissociate in water;
thus the Van't Hoff factor equals 1.
a) 1.6 x 101
b) 1.6 x 103
c) 1.6 x 104

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
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?

Knowing that at 0 oC and an oxygen pressure
of 1.00 atm, the aqueous solubility of O2 (g) is 48.9 mL
O2 per liter. The approximate values for the molarity of
O2 (g) in solution and the partial pressure of
O2 above a 8.23 x 10-4 M O2 (g) saturated
aqueous solution at 0 oC are respectively:
A. 2.18 M and 3.78 x 10-4 atm
B. 2.18 x 10-3 M and 0.378 atm
C. 0.0446 M and 0.0179 atm
D....

Knowing that at 0 oC and an oxygen pressure
of 1.00 atm, the aqueous solubility of O2 (g) is 48.9 mL
O2 per liter. The approximate values for the molarity of
O2 (g) in solution and the partial pressure of
O2 above a 8.23 x 10-4 M O2 (g) saturated
aqueous solution at 0 oC are respectively:
A. 2.18 M and 3.78 x 10-4 atm
B. 2.18 x 10-3 M and 0.378 atm
C. 0.0446 M and 0.0179 atm
D....

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