5.(20pts) Complete the following table. All work must be shown. Compound KCI C2H

Question

5.(20pts) Complete the following table. All work must be shown. Compound KCI C2H OH If the Molality wt% Xgolute 0.50 4.3 % 6.(12pts) osmotic pressure of a solution which contains 15.0 g of hemoglobin is in 1.00 x 10 mL of solution is 0.0560 atm at 25.0°C, what is the molar mass of hemoglobin .(12pts) hen 1.00 g of reserpine, a natural product used as a tranquilizer, is dissolved in 25.0 g of camphor, the freezing point depression is 2.63 degrees C. Ke for camphor is 40.0 °C/m. What is the molecular mass of reserpine? A solution is prepared by mixing 35.0 g of glucose CaHi,O% with 400.0 g of water. What is the vapor pressure in mmHg of the solution at 25°C ? The vapor pressure of pure water at 25 degrees C is 23.8 mm Hg. 8. (12pts) The solubility of N(g) in water is 8.21 x 10 mol/L at 0.0°C when the N2 pressure above the water is 0.790 atm. Calculate Henry's Law Constant kg. What will be the solubility of N2(g) in the water when the partial pressure of N2(g) above the water is 0.650 atm at 0.0°C?

Explanation / Answer

5.

1.

Molality of KCl = 0.50 m

It means that, 0.5 mol of KCl is in 1000 g. of solvent.

Mass of KCl = moles * molar mass = 0.5 * 74.5 = 37.25 g.

Therefore, % by mass solute = mass of solute * 100 / mass of solution = 37.25 * 100 / (1000 + 37.25) = 3.59 %

Moles of solvent = mass / molar mass = 1000 / 18 = 55.55 mol

Moles fraction of solute = moles of solute / total moles of solution

Xsolute = 0.5 / (0.5 + 55.55)

Xsolute = 0.00892

2.

4.3 % by weight of C2H5OH solution means,

4.3 g. of C2H5OH is in 100 g. of solution

Mass of C2H5OH = 4.3 g.

Mass of solvent = 100 - 4.3 = 95.7 g.

Molar mass of C2H5OH = 46 g/mol

Moles of solute = mass / molar mass = 4.3 / 46 = 0.0935 mol

Molality = moles of solute / mass of solvent in kg

m = 0.0935 / 0.0957

m = 0.977 m

Moles of solvent = mass / molar mass = 95.7 / 18 = 5.32 mol

Mole fraction of solute = moles of solute / total moles of solution

Xsolute = 0.0935 / (0.0935 + 5.32)

Xsolute = 0.0173

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