18) Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10-4 M O2at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 × 10-3M/atm.A) 1.9 atmB) 0.53 atmC) 0.24 atmD) 0.77 atmE) 0.32 atmAnswer: EDiff: 2Page Ref: 12.419) Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.20) Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10-3M/atm.21) Which of the following concentration units are temperature dependent?22) Identify the colligative property.A) Vapor pressure lowering.B) Freezing point depression.C) Boiling point elevation.D) Osmotic pressure.
HW 12 with answers E) All of the above.Answer: EDiff: 1Page Ref: 12.523) Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water.24) What mass (in g) of NH3must be dissolved in 475 g of methanol to make a 0.250 m solution?25) How many moles of KF are contained in 347 g of water in a 0.175 mKF solution?26) How many moles of KF are contained in 244 mL of 0.135 mKF solution? The density of the solution is 1.22 g/mL.A) 4.31 × 10-2mol KFB) 4.02 × 10-2mol KFC) 3.29 × 10-2mol KFD) 2.32 × 10-2mol KFE) 1.67 × 10-2mol KFAnswer: B
HW 12 with answers Diff: 3Page Ref: 12.5
HW 12 with answers 27) Calculate the molality of a solution that is prepared by mixing 25.5 mL of CH3OH (d= 0.792 g/mL) and 387 mL of CH3CH2CH2OH (d= 0.811 g/mL).28) Determine the molality of a solution prepared by dissolving 0.500 moles of CaF2in 11.5 moles H2O.
- Spring '14
- Partial Pressure, Page Ref, Freezing-point depression