The solubility of gases in water is generally lower under what conditions?higher temperature and lower pressurelower temperature and lower pressurehigh temperature and high pressurelower temperature and higher pressureO None, gases have a fixed solubility in water at all temperatures and pressures

According to Henry's law,Where, P is the partial pressure of the gasX is the solubility of gas in…

The solubility of gases in water is generally lower under what conditions? O higher temperature and lower pressure lower temperature and lower pressure O high temperature and high pressure O lower temperature and higher pressure None, gases have a fixed solubility in water at all temperatures and pressures

The solubility of gases in water is generally lower under what conditions? O higher temperature and lower pressure lower temperature and lower pressure O high temperature and high pressure O lower temperature and higher pressure None, gases have a fixed solubility in water at all temperatures and pressures

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter1: Matter And Measurements

Section: Chapter Questions

Problem 57QAP: The solubility of lead nitrate at 100C is 140.0 g/100 g water. A solution at 100C consists of 57.0 g...

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Rationalize the temperature dependence of the solubility of a gas in water in terms of the kinetic molecular theory.
Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?
Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H2O. What is the mole fraction of HCl in concentrated hydrochloric acid? What is the molal concentration of HCl?
Consider the following aqueous solutions: (i) 0.20 m HOCH2CH2OH (nonvolatile, nonelectrolyte); (ii) 0.10 m CaCl2 (iii) 0.12 m KBr; and (iv) 0.12 m Na2SO4. (a) Which solution has the highest boiling point? (b) Which solution has the lowest freezing point? (c) Which solution has the highest water vapor pressure?
Which of the following will have the lowest total vapor pressure at 25C? a. pure water (vapor pressure = 23.8 torr at 25C) b. a solution of glucose in water with C6H12O6=0.01 c. a solution of sodium chloride in water with NaCl = 0.01 d. a solution of methanol in water with CH3OH=0.2 (Consider the vapor pressure of both methanol [143 torr at 25C] and water.)
Samples of each of the substances listed below are dissolved in 125 g of water. Which of the solutions has the highest boiling point? (a) 3.0 g sucrose, C12H22O11 (b) 1.0 g glycerol, C3H3(OH)3 (c) 1.0 g propylene glycol, C3H6(OH)2 (d) 2.0 g glucose, C6H12(OH)2
An aqueous solution contains 0.180 g of an unknown, nonionic solute in 50.0 g of water. The solution freezes at 0.040 C. What is the molar mass of the solute?
Acetylene can be made by reacting calcium carbide with water. CaC2(s) + 2 H2O() C2H2(g) + Ca(OH)2(aq) Assume that you place 2.65 g CaC2 in excess water and collect the acetylene over water. The volume of the acetylene and water vapor is 795 mL at 25.0 C and a barometric pressure of 735.2 mmHg. Calculate the percent yield of acetylene. The vapor pressure of water at 25 C is 23.8 mmHg.
Equal numbers of moles of two soluble, substances, substance A and substance B, are placed into separate 1.0-L samples of water. a The water samples are cooled. Sample A freezes at 0.50C, and Sample B freezes at l.00C. Explain how the solutions can have different freezing points. b You pour 500 mL of the solution containing substance B into a different beaker. How would the freezing point of this 500-mL portion of solution B compare to the freezing point of the 1.0-L sample of solution A? c Calculate the molality of the solutions of A and B. Assume that i = 1 for substance A. d If you were to add an additional 1.0 kg of water to solution B, what would be the new freezing point of the solution? Try to write an answer to this question without using a mathematical formula. e What concentration (molality) of substances A and B would result in both solutions having a freezing point of 0.25C? f Compare the boiling points, vapor pressure, and osmotic pressure of the original solutions of A and B. Dont perform the calculations; just state which is the greater in each ease.
The solubility of lead nitrate at 100C is 140.0 g/100 g water. A solution at 100C consists of 57.0 g of lead nitrate in 64.0 g of water. When the solution is cooled 10C to 25.0 g of lead nitrate crystallize out. What is the solubility of lead nitrate in g/100 g water at 10C?
In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
n oil spill spreads out on the surface of water, rather than dissolving in the water. Explain why.