CO2 in water has a Henry’s law constant KB = 1.25 × 106 torr. How many liters of CO2 are needed to make 1 liter of sparkling water at 1 atm and 300 K? The density of water is 1 kg/L and it does not change as CO2 is dissolved. N.B. Treat gas as a solute, and note that in order for water to “sparkle” the partial pressure of CO2 in the vapor phase must equal the atmospheric pressure (note that this neglects the partial pressure of the water vapor).

A solution of 4.55 % phenol (C6H6O) solution by mass in carbon tetrachloride, CCl4.  The density of the solution is 1.602g/mL.  What are the molality, mole fraction, and molarity of phenol in the solution?   a. Fill in the summary table as you determine different parts of the problem – the first few columns are labeled – it is up to you to decide what is important information:   Molar mass mole         Solute             Solvent             Solution               b. Molality:   c. Mole Fraction:     d. Molarity:

Lead levels in drinking water should be no higher than 15 ppb. What is this in mol/L? Assume the density of drinking water is 1.0 g/mL. O 2.0 x 10-⁹ M O 3.1 x 10 ⁹ M O 3.1 x 107 M O 7.2 x 10 8 M O 7.2 x 10 5 M

At a particular temperature, the solubility of CO₂ in water is 0.13 M when the partial pressure is 1.5 atm. What partial pressure (in atm) of CO₂ would give a solubility of 0.078 M?

What would be the theoretical freezing point of a solution made by dissolving 10.43 g of NiCl 2 in 365.0 g of water? The freezing point constant of water is 1.86 °C/molal. The molar mass of NiCl 2 is 129.5994 g/mol.     1.230 °C     1.506 °C     0.8128 °C     -1.230 °C     1.022 °C

The partial pressure of CO2 gas above the liquid in a bottle of champagne at 20°C is 4.3 atm. What is the solubility of CO2 in champagne? Assume the Henry's law constant is the same for champagne as it is for water: at 20°C, kH = 3.7 × 10−2 mol/(L·atm).

8. Compounds A and B form an ideal solution. The vapor pressure of pure A is P= 72.2 mmHg and a solution with a mole fraction of A of XA= 0.60 has a total vapor pressure of PTot= 59.6 mmHg. What is the vapor pressure of pure B?

Calculate the solubility of O2 in water at a partial pressure of O₂ of 150. torr at 25°C. The Henry's law constant for O₂ is 1.3 x 10-3 mol/L atm for Henry's law in the form C = KP, where C js the gas concentration (mol/L). Solubility= mol/L

Suppose that you add 21.1 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 °C/m. With the added solute, you find that there is a freezing point depression of 2.86 °C compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound?

A solution is made by mixing 100.0 g acetone (CH3COCH3) and 100.0 g methanol (CH3OH). a. What is the vapor pressure of this solution at 25C? b. What is the composition of the vapor expressed as a mole fraction? Assume ideal solution and gas behavior. (At 25 C the vapor pressures of pure acetone and pure methanol are 271 and 143 torr, respectively.) The actual vapor pressure of this solution is 161 torr. Explain any discrepancies.