11 M%6WaterEthanolF5The molality of the solution isThe freezing point of the solution isSubmit AnswerThe freezing point of water is 0.00 °C at 1 atmosphere.A student dissolves 10.57 grams of copper(II) nitrate, Cu(NO3)2 (187.6 g/mol), in 231.2 grams of water. Use the table of boilingand freezing point constants to answer the questions below.SolventFormulaKb(°C/m) Kf(°C/m)1.861.990.5121.22Chloroform3.67BenzeneC6H62.53Diethyl ether CH3 CH₂ OCH2 CH3 2.026HYH₂OCH3 CH₂OHCHCI,NF6Retry Entire GroupCengage Learning | Cengage Technical SupportMacBook Air&7UMF7*8m.K°C.o?locator=assignment-take8 more group attempts remainingDIIFB<[Review Topics][References]Use the References to access important values if needed for this question.(905.12L)0prodo OWLVPF10{eF11Macon11 +PreviousF12Chapt OWLVNextSave and ExitdeleteAChapt OWLVUSRelau ONDThe molality of the solution isSubmit Answer%The boiling point of the solution is5TGThe boiling point of water is 100.00 °C at 1 atmosphere.A student dissolves 10.98 grams of chromium(III) sulfate, Cr₂(SO4)3 (392.2 g/mol), in 177.8 grams of water. Use the table ofboiling and freezing point constants to answer the questions below.SolventWalEthanolChloroformBenzeneBF5FormulaH₂OCH3CH₂OHCHCl3C6H6Diethyl ether CH₂CH₂OCH₂CH36YHMacBook AirCengage Learning Cengage Technical SupportF6NRetry Entire Group 8 more group attempts remaining&7Um.F7M°C.8[Review Topics][References]Use the References to access important values if needed for this question.Kb (°C/m) Kf (°C/m)1.861.99cator assignment-take0.5121.223.672.532.021FBK5.12.(9OF9)0AOWLVPF10MaconF11+1Chapt OWLV{ar[111Previous Next>Û SSave and ExitChapt OWLYdeletereturnRela

Answered: Image /qna-images/answer/004ea909-95c1-4334-83d2-10ce17e246ef.jpg

zing point of water is 0.00 °C at 1 atmosphere. A student dissolves 10.57 grams of copper(II) nitrate, Cu(NO3)2 (187.6 g/mol), in 231.2 grams of water. Use the e and freezing point constants to answer the questions below. Solvent Formula Kb(°C/m) Kr(°C/m) H₂O 0.512 CH3CH₂OH 1.22 Chloroform CHCI, 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH₂ CH3 2.02 Water Ethanol The molality of the solution is The freezing point of the solution is Submit Answer Retry Entire Group m. [Review Topics] [References) Use the References to access important values if needed for this question. °C. 1.86 1.99 5.12 8 more group attempts remaining Chapt Owa û W

zing point of water is 0.00 °C at 1 atmosphere. A student dissolves 10.57 grams of copper(II) nitrate, Cu(NO3)2 (187.6 g/mol), in 231.2 grams of water. Use the e and freezing point constants to answer the questions below. Solvent Formula Kb(°C/m) Kr(°C/m) H₂O 0.512 CH3CH₂OH 1.22 Chloroform CHCI, 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH₂ CH3 2.02 Water Ethanol The molality of the solution is The freezing point of the solution is Submit Answer Retry Entire Group m. [Review Topics] [References) Use the References to access important values if needed for this question. °C. 1.86 1.99 5.12 8 more group attempts remaining Chapt Owa û W

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 5ALQ: You have read that adding a solute to a solvent can both increase the boiling point and decrease the...

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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.)
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?
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.
6-21 Are mixtures of gases true solutions or heterogeneous mixtures? Explain.
Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.
Solutions Introduced directly into the bloodstream have to be isotonic with blood; that is, they must have the same osmotic pressure as blood. An aqueous NaCl solution has to be 0.90% by mass to be isotonic with blood. What is the molarity of the sodium ions in solution? Take the density of the solution to be 1.00 g/mL.
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.