The boiling point of water is 100.00 °C at 1 atmosphere.A student dissolves 13.53 grams of copper(II) acetate, Cu(CH3COO)2 (181.7 g/mol), in 281.1 grams of water. Usethe table of boiling and freezing point constants to answer the questions below.SolventWaterEthanolChloroformBenzeneFormulaH₂OCH3CH₂OHCHCI 3C6H6Diethyl ether CH3CH₂CH₂CH3The molality of the solution isThe boiling point of the solution isK₁ (°C/m) K₁ (°C/m)0.5121.861.221.993.672.532.02m.°C.5.12

Answered: Image /qna-images/answer/e303106c-cd1f-4920-a81c-12d866296133.jpg

The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 13.53 grams of copper(II) acetate, Cu(CH3COO)2 (181.7 g/mol), in 281.1 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Formula H2₂O CH3CH₂OH CHCI 3 соно Diethyl ether CH3CH₂OCH₂CH3 Solvent Water Ethanol Chloroform Benzene The molality of the solution is The boiling point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12

The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 13.53 grams of copper(II) acetate, Cu(CH3COO)2 (181.7 g/mol), in 281.1 grams of water. Use the table of boiling and freezing point constants to answer the questions below. Formula H2₂O CH3CH₂OH CHCI 3 соно Diethyl ether CH3CH₂OCH₂CH3 Solvent Water Ethanol Chloroform Benzene The molality of the solution is The boiling point of the solution is Kb (°C/m) Kf (°C/m) 1.86 1.99 0.512 1.22 3.67 2.53 2.02 m. °C. 5.12

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A certain liquid X has a normal freezing point of −6.30°C and a freezing point depression constant Kf=7.40·°C·kgmol−1. Calculate the freezing point of a solution made of 31.g of benzamide (C7H7NO) dissolved in 800.g of X. Round your answer to 2 significant digits.
q 2req Visited 2req [Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. Kb (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 10.17 grams of the compound were dissolved in 204.5 grams of ethanol, the solution began to boil at 78.723 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Q Graph_08-30-2....pdf NO Retry Entire Group O J A 9 more group attempts remaining I' 6 Previous Next> Show all 11:15 PM 9/12/2022
4. Hexachlorophene is used as a disinfectant in germicidal soaps. What mass of hexachlorophene ( M = 406.9 g/mol) must be added to 125 g of chloroform to give a solution with a boiling point of 62.60°C? K = 3.63°C/m, boiling point of pure chloroform = 61.70°C %3D
[References] Use the References to access important values if needed for this question. The boiling point of ethanol, CH3 CH₂OH, is 78.500 °C at 1 atmosphere. K₁ (ethanol) = 1.22 °C/m In a laboratory experiment, students synthesized a new compound and found that when 14.95 grams of the compound were dissolved in 293.3 grams of ethanol, the solution began to boll at 78.570 °C. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? g/mol Submit Answer Retry Entire Group 9 more group attempts remaining Show Hint Congage Learning Cengage Technical Support Previous Next Save and Exit
The normal freezing point of a certain liquid X is −9.10 °C, but when 8.7 g of potassium bromide (KBr) are dissolved in 100. g of X the solution freezes at - 12.2 °C instead. Use this information to calculate the molal freezing point depression constant K of X. Round your answer to 2 significant digits. K₁ = °C.kg mol x10 X
4- 30- [14] How many liters of the antifreeze ethylene glycol (HOCH₂CH₂OH, 54.09 g/mol) would you add to a car-radiator containing 6.50 L of water to keep it from freezing if the coldest winter temperature in your area is -20°C? Calculate the boiling point of this water-ethylene glycol mixture. (The density of ethylene glycol is 1.11 g/mL, the molal freezing and boiling point constants are respectively kf = 1.86°/m and kb= 0.52 °/m). & Page 5
A solution is prepared by adding 62 g Pb(NO3)2 to 100 g water at 20 °C. Is the solution saturated, unsaturated, or supersaturated? The temperature is raised to 80 °C. There is a temperature at which the solution is no longer classified by the term you answered above. What is that temperature? Just list the number, don't include the °C unit. At 80 °C, is the solution classified as saturated, unsaturated, or super saturated?
17
A certain substance X has a normal freezing point of 4.7 °C and a molal freezing point depression constant K₁ = 3.86 °C · kg • mol by dissolving some urea ((NH,),CO) in 600. of X. This solution freezes at 1.3 °C. Calculate the mass of urea that was dissolved. Be sure your answer has the correct number of significant digits. g ☐ x10 X 1 . A solution is prepared 5
Which chemical or functional group helps a molecule dissolve in water? NH2 (amino group) fats hydrocarbon tails (side chains) CH3 (methyl group)
10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5 °C. What is the molar heat of dissolution for ZnCl2? Assume the specific heat capacity of the solution is the same as pure water, 4.184 J/g·°C.
c) To save money, some state Department of Transportation decided to replace relatively expensive calcium chloride (CaCl2) by more affordable beet juice (mostly made of sugar molecules) in the solutions used to treat the roads before a snow/freezing rain storm. However, the beet juice was not as effective at de-icing the roads as was the calcium chloride solution. When road temperatures were very low, the beet juice treatment did not prevent the water from freezing again. You are called to one of those Departments of Transportation to: 1) Explain that observation and 2) Justify why they should continue to use calcium chloride solutions even if it is more expensive. You may even suggest a cheaper alternative to calcium chloride that will be as effective in road de-icing. Provide your answers below.