Dre The freezing point of ethanol, CH₂CH₂OH, is -117.30 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin A student dissolves 11.59 grams of saccharin, C,H, NO₂S (163.2 g/mol), in 191.4 grams of ethanol. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH₂CH₂OH CHCI Calle Diethyl ether CH, CH,OCH,CH, The molality of the solution is The freezing point of the solution is An Ray Care Gr K. (C/m) K (C/m) 0.512 1.86 1.99 1.22 3.67 2.53 2.02 m view Topics Platorencon Use the References to access important values if needed for this question. 5.12 "C

Dre The freezing point of ethanol, CH₂CH₂OH, is -117.30 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin A student dissolves 11.59 grams of saccharin, C,H, NO₂S (163.2 g/mol), in 191.4 grams of ethanol. Use the table of boiling and freezing point constants to answer the questions below. Solvent Water Ethanol Chloroform Benzene Formula H₂O CH₂CH₂OH CHCI Calle Diethyl ether CH, CH,OCH,CH, The molality of the solution is The freezing point of the solution is An Ray Care Gr K. (C/m) K (C/m) 0.512 1.86 1.99 1.22 3.67 2.53 2.02 m view Topics Platorencon Use the References to access important values if needed for this question. 5.12 "C

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.95QE

See similar textbooks

Similar questions

Calculate the freezing point and normal boiling points of each of the following aqueous solutions. (a) 2.63 m acetic acid (b) 33.0 % by mass lactose, C12H22O11 (c) 32.15 mL of ethylene glycol, C2H6O2(d=1.113g/mL) in 624 mL of water (d=1.00g/mL)
What is the freezing point and normal boiling point of a solution made by adding 39 mL of acetone, C3H6O, to 225 mL of water? The densities of acetone and water are 0.790 g/cm3 and 1.00 g/cm3, respectively.
In a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.
Calculate the freezing point of 525 g of water that contains 25.0 g of NaCl. Assume i, the vant Hoff factor, is 1.85 for NaCl.
Ice Cream A rock salt (NaCl), ice, and water mixture isused to cool milk and cream to make homemade icecream. How many grams of rock salt must be added towater to lower the freezing point by 10.0°C?
The solubility of NaCl in water at 100 C is 39.1 g/100. g of water Calculate the boiling point of this solution. (Assume i = 1.85 for NaCl.)
Two samples of sodium chloride solutions are brought to a boil on a stove. One of the solutions boils at 100.10C and the other at 100.15C. a Which of the solutions is more concentrated? b Which of the solutions would have a lower freezing point? c If you split the solution that boils at 100.1C into two portions, how would the boiling points of the samples compare? Which of the following statements do you agree with regarding the determination of your answer for part c? I. The question cannot be answered with certainty without knowing the volumes of each portion. II. Making the necessary assumption that the two samples have equal volumes, I was able to correctly answer the question. III. The volumes that the sample was split into are irrelevant when determining the correct answer.
6-68 If we add 175 g of ethylene glycol, C2H6O2, per 1000. g of water to a car radiator, what will be the freezing point of the solution?