9. Compare the equal-molarity solutions of table salt (NaCl) in water and sucrose in water to pure water.Which will have the highest boiling point?(A) NaCl in H2O(B) sucrose in H2O(C) pure H2O(D) NaCl in H20 and sucrose in H2O will both have the same boiling point, slightly elevatedcompared to pure H2O

∆Tb = i×Kf×m ∆Tb = Boiling point of solution - Boiling point of Water i is van't hoff…

9. Compare the equal-molarity solutions of table salt (NaCl) in water and sucrose in water to pure water. Which will have the highest boiling point? (A) NaCl in H;O (B) sucrose in H20 (C) pure H2O (D) NaCl in H2O and sucrose in H;O will both have the same boiling point, slightly elevated compared to pure H;O

9. Compare the equal-molarity solutions of table salt (NaCl) in water and sucrose in water to pure water. Which will have the highest boiling point? (A) NaCl in H;O (B) sucrose in H20 (C) pure H2O (D) NaCl in H2O and sucrose in H;O will both have the same boiling point, slightly elevated compared to pure H;O

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...

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An aqueous solution is prepared by dissolving 1.50 g of hemocyanin, a protein obtained from crabs, in 0.250 L of water. The solution has an osmotic pressure of 0.00342 atm at 277 K. (a) What is the molar mass of hemocyanin? (b) (b) What should the freezing point of the solution be?
If dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.
(d) Determine the freezing point and boiling point of the solution. (Assume density of water = 1.00 g/mL; Kf= 1.86oC/m; Kb= 0.512oC/m; density of EG = 1.114 g/mL
At 45 °C, a solution is prepared by mixing 48.0 g Na2SO4 with 240.0 g water. The vapor pressure of water at 45 °C is 71.9 torr. Assuming total dissociation of the salt, determine: (a) mole fraction of Na2SO4; (b) mole fraction of water; (c) vapor pressure of the solution. (molar mass, g/mol: Na2SO4= 142.04; water = 18.02) (a) XNa2s04 = (b) Xwater = (d) Psoln =
If dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.
The freezing point of ethanol CH3 CH₂OH is -117.30 °C℃ at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is saccharin. How many grams of saccharin, C7H5NO3S (183.2 g/mol), must be dissolved in 278.0 grams of ethanol to reduce the freezing point by 0.300 °C? Refer to the table for the necessary boiling or freezing point constant. Solvent Formula Kb (°C/m) Kf(°C/m) Water H₂O 0.512 Ethanol CH3 CH₂OH 1.22 Chloroform CHCl3 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH₂ OCH₂ CH3 2.02 Mass= || g 1.86 1.99 5.12
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