A student prepared a sugar solution containing 1.463 g of sugar (C12H22On) in 25.00 mL of water, and he/she produced the following freezing point data: Freezing Point of Pure Water 20 15 10 10 20 60 100 110 120 130 time (seconds) Freezing Point of Sugar Solution 25 20 30 10 een What is the Ki of water based on the student's data? A. 20 °C/m B. 8.8 °C/m C. 4.2 °C/m D. 0.49 °C/m Temperature ()

A student prepared a sugar solution containing 1.463 g of sugar (C12H22On) in 25.00 mL of water, and he/she produced the following freezing point data: Freezing Point of Pure Water 20 15 10 10 20 60 100 110 120 130 time (seconds) Freezing Point of Sugar Solution 25 20 30 10 een What is the Ki of water based on the student's data? A. 20 °C/m B. 8.8 °C/m C. 4.2 °C/m D. 0.49 °C/m Temperature ()

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

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 104SCQ: Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride...

See similar textbooks

Similar questions

A 12-oz (355-mL) Pepsi contains 38.9 mg caffeine (molar mass = 194.2 g/mol). Assume that the Pepsi, mainly water, has a density of 1.01 g/mL. For such a Pepsi, calculate: (a) its caffeine concentration in ppm; (b) its molarity of caffeine; and (c) the molality of caffeine.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
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.)
Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through, as shown in the following diagram. Based on each of the following identities for solutions A and B, indicate whether the liquid level in compartment A, with time, will increase, decrease, or not change. a. A = 1.0 M NaCl solution and B = 2.0 M NaCl solution b. A = 5.0%(m/v) glucose solution and B = 4.0%(m/v) glucose solution c. A = 2.0 M KCl solution and B = 2.0 M KNO3 solution d. A = 1.0 M glucose solution and B = 1.0 M NaCl solution