What is the freezing point depression (in °C) and freezing point (in K) of a solution containing 2.40 g biphenyl (C₁2H10) in 75.0 g benzene (C6H₁)? Kf (benzene): -5.12 °C kg mol-¹, with a melting temperature of 5.5 °C. a. Freezing point depression: -1.06 °C; freezing point: 277.6 K O b. Freezing point depression: -1.16 °C; freezing point: 277.5 K O C. Freezing point depression: -1.26 °C; freezing point: 277.4 K O d. Freezing point depression: -1.36 °C; freezing point: 277.3 K e. Freezing point depression: -1.46 °C; freezing point: 277.2 K

What is the freezing point depression (in °C) and freezing point (in K) of a solution containing 2.40 g biphenyl (C₁2H10) in 75.0 g benzene (C6H₁)? Kf (benzene): -5.12 °C kg mol-¹, with a melting temperature of 5.5 °C. a. Freezing point depression: -1.06 °C; freezing point: 277.6 K O b. Freezing point depression: -1.16 °C; freezing point: 277.5 K O C. Freezing point depression: -1.26 °C; freezing point: 277.4 K O d. Freezing point depression: -1.36 °C; freezing point: 277.3 K e. Freezing point depression: -1.46 °C; freezing point: 277.2 K

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter13: Solutions And Their Behavior

Section: Chapter Questions

Problem 107SCQ

See similar textbooks

Similar questions

Insulin is a hormone responsible for the regulation of glucose levels in the blood. An aqueous solution of insulin has an osmotic pressure of 2.5 mm Hg at 25C. It is prepared by dissolving 0.100 g of insulin in enough water to make 125 mL of solution. What is the molar mass of insulin?
The freezing point of a 0.11 m solution of HNO2 is -0.20C. (a) What is i for the solution? (b) Is the solution made (i) of HNO2 molecules only? (ii) of H+ and NO2- only? (iii) of more HNO2 molecules than H+ ions? (iv) primarily of H+ and NO2- ions with some HNO2 molecules?
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
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)
A compound has a solubility in water of 250 mg/L at 25C. Should this compound be characterized as a soluble or insoluble compound at 25C?
The Henry's law constant for the solubility of argon gas in water is 1.0103M/atm at 30C. (a) Express the constant in M/mm Hg. (b) If the partial pressure of argon gas at 30C is 693 mm Hg, what is the concentration (in M) of the dissolved argon gas at 30C? (c) How many grams of argon gas can be dissolved in 29 L of water at 693 mm Hg and 30C? (Ignore the partial pressure of water.)
The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25 C. What is the molar mass of insulin?