1.Calculate the concentration of argon in the Pacific Ocean given that the parti

Question

1.Calculate the concentration of argon in the Pacific Ocean given that the partial pressure of argon is 0.00934 atm. The Henry’s law constant for argon in water at 25oC is 1.4 x 10-3 mol/L·atm

2.The solubility of potassium chloride (KCl) is 34.2 g per 100.0 g of water at 20oC. (a) Calculate the molality of a saturated solution of potassium chloride.

(b) Is a 4.00 m solution of potassium chloride in water at 20oC saturated, supersaturated, or unsaturated? Answer: saturated, supersaturated, or unsaturated

(c) Is a 6.00 m solution of potassium chloride in water at 20oC saturated, supersaturated, or unsaturated? Answer: saturated, supersaturated, or unsaturated

3.A supermarket brand bleach contains 4.88 g of sodium hypochlorite (NaOCl) in 100.0 g of water. Calculate the molality, mass percent, ppm, and mole fraction of sodium hypochlorite in this solution.
Molality of sodium hypochlorite in water

a.Mass percent of sodium hypochlorite in water

b.ppm of sodium hypochlorite in water

c.Mole fraction of sodium hypochlorite in water

4.The vapor pressure of water at 20°C is 17.54 torr. Calculate the vapor pressure (in torr) of an aqueous solution containing 8.444 g of urea (CO(NH2)2) in 84.48 g of water at 20°C.

5.The addition of nonvolatile solute would elevate the boiling point of a substance. Calculate the boiling point of 0.243 kg of water containing 21.1 g of urea (CO(NH2)2). The boiling point of water is exactly 100 oC, and Kb of water is 0.51 oC·kg/mol.  

6.The freezing point of water is exactly 0oC but the freezing point can be lowered by the addition of solutes. Calculate the freezing point of 0.199 kg of water containing 22.4 g of urea (CO(NH2)2). Kf of water is 1.86 oC·kg/mol.

7.A 1.424 g sample of a protein dissolved in 1.000 L of an aqueous solution at 37.15°C has an osmotic pressure of 1.988 x 10-4 atm. What is the molar mass of the protein?

8.True or false
1. Sea water is a heterogeneous solution containing salts and water. Answer: _______
2. In the solution process, the breaking of solute particles is an endothermic process because energy is absorbed when molecules are separated. Answer: _______
3. Entropy change in the solution process is always negative. Answer: _______
4. Polar solutes are generally insoluble in polar solvents. Answer: _______
5. Decreasing partial pressure increases the solubility of gases, liquids and solids. Answer: _______
6. Solubility of gases in water generally decreases at higher temperature. Answer: _______
7. Solubility of gases in water generally decreases at higher partial pressure. Answer: _______
8. Solubility of solids in water generally increases at higher temperature. Answer: _______
9. Addition of a nonvolatile solute to a solvent lowers the vapor pressure and reduces the boiling point of the solution. Answer: _______
10. The semipermeable cell membrane in red blood cells permits water and small molecules such as salts to pass through. Answer: _______

Explanation / Answer

1)
use Henry’s law equation

C = KH*P
C = 1.4*10^-3 * 0.00934
= 1.3076*10^-5 mol/L

Answer: 1.3076*10^-5 mol/L

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