14. How many grams of nitrogen and oxygen are dissolved in 125 grams of water at

Question

14. How many grams of nitrogen and oxygen are dissolved in 125 grams of water at 20.0 degrees Celsius when the water is saturated with air, in which PN2 is 593 Torr and Po2 is 159 Torr? At 1 atm, the solubility of pure oxygen in water is 0.00430 grams 02/100 g H20, and the solubility of pure Nitrogen in water is 0.00190 g N2/100 g H20. 15. If the mol fraction of oxygen in air is 0.21, what is the partial pressure of oxygen if the atmosphere pressure is 1 atm? What is the molar solubility of oxygen in an aquarium at 1 atm? KH 1.26x 10-3 M/atm at 25 C. 16. What is the molality (m) of a 1.20 M NaCI solution in a 1 L container whose density is 1.0200 g/mL? MM of NaCl 58.5 g/mol, 17. What is the ppm of Ca2 in a 2.50 L solution containing 1.20 g CaCl2? MM of CaCl2 111.1 g/mol 18. CCl4 has a vapor pressure of 155 Torr at 20 'C. This solvent can dissolve candle wax which is nonvolatile. The MM of candle wax is 311 g/mol. How much will the vapor pressure of CCl be lowered when a solution is prepared by dissolving 10.0 g of wax into 40.00 g of carbon tetrachloride? What is the resulting vapor pressure of this solution?

Explanation / Answer

15)

a)

partial pressure of O2 = mole fraction * total pressure

= 0.21 * 1 atm

= 0.21 atm

Answer: 0.21 atm

b)

Now use Henry’s law to calculate solubility:

use:

S = KH*P

= (1.26*10^-3 M/atm) * 0.21 atm

= 2.65*10^-4 M

Answer: 2.65*10^-4 M

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