Question

The vapor pressure of pure liquid water is p*(H2O) = 0.02308 atm. Above an aqueous solution...

The vapor pressure of pure liquid water is p*(H2O) = 0.02308 atm. Above an aqueous solution with 122 g of a non-volatile solute (molar mass 241 g/mol) in 920 g H2O has a vapor pressure of 0.02239 atm. Calculate the activity and the activity coefficient of water in the solution.

Homework Answers

Answer #1

Ans:

The vapor pressure of pure liquid water is p*(H2O) = 0.02308 atm. Above an aqueous solution with 122 g of a non-volatile solute (molar mass 241 g/mol) in 920 g H2O has a vapor pressure of 0.02239 atm.

Moles solute = nB= 122 g (1. mol/241. g) = 0.5062 mol

Moles water = nA = 920 g (1. mol/18.01 g) = 51.083 mol

XB= nB/(nA+ nB) = (0.5062)/(51.083 + 0.5062) = 0.00981 and XA= 0.99019

Activity of water in the solution aA = pH2O/pH2O* = 0.02239/0.02308 = 0.9701

Since aA= gAXA, then gA= aA/XA

Therefore Activity coefficient of water of water in the solution = gA = 0.9701/0.99019 = 0.980

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
An isotonic solution will produce an osmotic pressure of 7.84 atm measured against pure water at...
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)
A solution is obtained by dissolving 99.5 g of sucrose (i = 1) with 360.4 g...
A solution is obtained by dissolving 99.5 g of sucrose (i = 1) with 360.4 g of H2O at 55 ºC. Sucrose is a non-volatile solute. The water vapor pressure at 55ºC is 118.1 torr. The molar mass of sucrose is 342.3 g / mol and H2O is 18.02 g / mol. Calculate the vapor pressure on the solution: How much is the change in vapor pressure, ΔP:
a 39.8 degree celcius aqueous solution has a vapor pressure of 47 torr .the solution contains...
a 39.8 degree celcius aqueous solution has a vapor pressure of 47 torr .the solution contains 63.4 g of the non volatile ,non dissociating liquid glycerin and 73.7 g of water.find the VP of water at 39.8 degree celcius?
The vapor pressure of pure water at 25.0 oC is 23.8 torr. What is the vapor...
The vapor pressure of pure water at 25.0 oC is 23.8 torr. What is the vapor pressure (at 25.0 oC), in atm, of an aqueous solution of 54.0 g glucose (C6H12O6), MM = 180. g mol-1) in 285.0 g of water? 760 torr = 1 atm P1 = X1Po1 Circle your choice. a) 0.0451 b) 0.194 c) 0.0307 d) 0.105 e) 0.146 f) 0.0287
16.177 g of a non-volatile solute is dissolved in 290.0 g of water. The solute does...
16.177 g of a non-volatile solute is dissolved in 290.0 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 40°C the vapour pressure of the solution is 54.506 torr. The vapour pressure of pure water at 40°C is 55.324 torr. Calculate the molar mass of the solute (g/mol). Now suppose, instead, that 16.177 g of a volatile solute is dissolved in 290.0 g of...
Please answer only if you 100% know and it has to be all of them! Please...
Please answer only if you 100% know and it has to be all of them! Please show work neatly!!! :)Thanks! 1. Calculate the molarity, molality and mass % of NH3 in a solution in which 60.0g of NH3 are dissolved in 140.0g of water. The Density of this solution is 0.982g/mL 2. A solution is prepared by dissolving 38.0g of non-volatile molecular solute in 125 grams of benzene. The boiling point of this solution is 84.5C (Celsius) and the boiling...
A 500.0 mL solution of NaNO3 in water has a vapor pressure of 21.445 mm Hg...
A 500.0 mL solution of NaNO3 in water has a vapor pressure of 21.445 mm Hg at 25°C. How many grams of NaNO3 (molar mass = 84.994 g/mol) were added to the water if the vapor pressure of pure water at 25°C is 23.76 mm Hg. Assume the volume of the water (d = 1.000 g/mL) is the same as the volume of the solution.
The vapor pressure of water is 3.1672 kPa at 25oC. If the vapor pressure over a...
The vapor pressure of water is 3.1672 kPa at 25oC. If the vapor pressure over a non-electrolyte solution of the nonvolatile solute urea is 3.1232 kPa when the mass fraction of urea is 0.0450, what is the experimental value of the molar mass of urea?
At 25o C the vapor pressure of pure benzene is 0.1252 atm. If we dissolve 9...
At 25o C the vapor pressure of pure benzene is 0.1252 atm. If we dissolve 9 g of an unknown hydrocarbon in 88.9 g of pure benzene (MW = 78.0 g/mol), we observe that the vapor pressure of the benzene in the resulting solution is 0.1191 atm. What is the molecular weight of the unknown solid (in g/mol)?
At 25o C the vapor pressure of pure benzene is 0.1252 atm. If we dissolve 9...
At 25o C the vapor pressure of pure benzene is 0.1252 atm. If we dissolve 9 g of an unknown hydrocarbon in 88.9 g of pure benzene (MW = 78.0 g/mol), we observe that the vapor pressure of the benzene in the resulting solution is 0.1191 atm. What is the molecular weight of the unknown solid (in g/mol)?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT