For the listed solutions, compare the osmotic pressure, boiling point, freezing point, and vapor pressure at 50. °C. Part 1 of 4 Which solution has the highest osmotic pressure? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose O 0.100 m CaCl₂ Part 2 of 4 Which solution has the highest boiling point? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose 0 0.100 m CaCl₂ Part 3 of 4 Which solution has the highest freezing point? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose O 0.100 m CaCl₂ Part 4 of 4 x Which solution has the highest vapor pressure at 50. °C? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose 0.100 m CaCl₂ X

For the listed solutions, compare the osmotic pressure, boiling point, freezing point, and vapor pressure at 50. °C. Part 1 of 4 Which solution has the highest osmotic pressure? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose O 0.100 m CaCl₂ Part 2 of 4 Which solution has the highest boiling point? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose 0 0.100 m CaCl₂ Part 3 of 4 Which solution has the highest freezing point? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose O 0.100 m CaCl₂ Part 4 of 4 x Which solution has the highest vapor pressure at 50. °C? Select the single best answer. O 0.100 m NaNO3 O 0.100 m glucose 0.100 m CaCl₂ X

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 73QAP: Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol,...

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Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Oxygen gas in water with P = 1 atm and T = 10C Oxygen gas in water with P = 1 atm and T = 20C b. Nitrogen gas in water with P = 2 atm and T = 50C Nitrogen gas in water with P = 1 atm and T = 70C c. Table salt in water with P = 1 atm and T = 40C Table salt in water with P = 1 atm and T = 70C d. Table sugar in water with P = 3 atm and T = 30C Table sugar in water with P = 1 atm and T = 80C
Will red blood cells swell, remain the same size, or shrink when placed in each of the solutions in Problem 8-101? Classify each of the following solutions as hypotonic, isotonic, or hypertonic relative to red blood cells? a. 0.92%(m/v) glucose solution b. 0.92%(m/v) NaCl solution c. 2.3%(m/v) glucose solution d. 5.0%(m/v) NaCl solution
Arrange the following solutions in order by their decreasing freezing points: 0.1 m Na3PO4, 0.1 m C2H5OH, 0.01 m CO2, 0.151 m NaCI, and 0.21 m cacI2.
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
Refer to Figure 13.10 ( Sec. 13-4b) to determine whether these situations would result in an unsaturated, saturated, or supersaturated solution. 120. g RbCl is added to 100. g H2O at 50 °C. 30. g KCl is dissolved in 100. g H2O at 70 °C. 20. g NaCl is dissolved in 50. g H2O at 60 °C. Figure 13.10 Solubility of ionic compounds versus temperature.
The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?