✓ Question Completion Status:Which aqueous solution has the lowest freezing point? (Assume complete dissociation for electrolytes)O a. 0.10 m HCIO b.0.10 (NH4)2SO c. 0.20 m C₂H5OHO d. 0.20 m K₂SO4Ⓒe.0.20 Fel3QUESTION 3What is the freezing point of a solution prepared from 45.0 g ethylene glycol (C2H602) and 85.0 g H2O? Kf of water is 1.86°C/m.O a.-15.9°COb. 15.9°COc.-159°CO d.-1.50°CO e. 1.50°CQUESTION 4A 29.90 g sample of an unknown substance (nonelectrolyte) is mixed with 250.0 g of stearic acid. The freezing point depression was6.7°C. Calculate molar mass of the unknown substance. kf of stearic acid is 5.1°C/mO 155 6 almolClick Save and Submit to save and submit. Click Save All Answers to save all answers.2.5 polSav

Question: which of the aqueous solution has lowest freezing point? Given 5 option of different…

Which aqueous solution has the lowest freezing point? (Assume complete dissociation for electrolytes) O a. 0.10 m HCI O b.0.10 (NH4)2S O c. 0.20 m C₂H5OH O d. 0.20 m K₂SO4 Ⓒe.0.20 Fel3 QUESTION 3 What is the freezing point of a solution prepared from 45.0 g ethylene glycol (C2H602) and 85.0 g H20? Kf of water is 1.86°Clm. O a.-15.9°C O b. 15.9°C O c.-159°C O d.-1.50°C O e. 1.50°C

Which aqueous solution has the lowest freezing point? (Assume complete dissociation for electrolytes) O a. 0.10 m HCI O b.0.10 (NH4)2S O c. 0.20 m C₂H5OH O d. 0.20 m K₂SO4 Ⓒe.0.20 Fel3 QUESTION 3 What is the freezing point of a solution prepared from 45.0 g ethylene glycol (C2H602) and 85.0 g H20? Kf of water is 1.86°Clm. O a.-15.9°C O b. 15.9°C O c.-159°C O d.-1.50°C O e. 1.50°C

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.
Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
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?
Assume that you have identical volumes of two liquids; the first is 0.3 M glucose solution and the second is 0.1 M glucose solution. Based on the diagrams in Problem 8-85, where red is the 0.3 M glucose and blue is the 0.1 M glucose, which one of the diagrams best represents the two liquids after they have stood uncovered for a few days and some evaporation of liquid has occurred?
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.)
Graph Table 14.10 shows solubility data that was collectedin an experiment. Plot a graph of the molarity ofKI versus temperature. What is the solubility of KI at55°C?