[Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of ethanol CH3 CH₂OH is 78.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen (estradiol). How many grams of estrogen, C18H24 O2 (272.4 g/mol), must be dissolved in 287.0 grams of ethanol to raise the boiling point by 0.500 °C? Refer to the table for the necessary boiling or freezing point constant. Formula Kb (°C/m) Kf(°C/m) 0.512 Solvent Water Ethanol H₂O CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH2 OCH₂ CH3 2.02 Mass= Submit Answer 9 Retry Entire Group Show Hint 1.86 1.99 5.12 9 more group attempts remaining I narning Cengage Technical Support Previous Next Save and Exit

[Review Topics] [References] Use the References to access important values if needed for this question. The boiling point of ethanol CH3 CH₂OH is 78.50 °C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in ethanol is estrogen (estradiol). How many grams of estrogen, C18H24 O2 (272.4 g/mol), must be dissolved in 287.0 grams of ethanol to raise the boiling point by 0.500 °C? Refer to the table for the necessary boiling or freezing point constant. Formula Kb (°C/m) Kf(°C/m) 0.512 Solvent Water Ethanol H₂O CH3 CH₂OH 1.22 Chloroform CHC13 3.67 Benzene C6H6 2.53 Diethyl ether CH3 CH2 OCH₂ CH3 2.02 Mass= Submit Answer 9 Retry Entire Group Show Hint 1.86 1.99 5.12 9 more group attempts remaining I narning Cengage Technical Support Previous Next Save and Exit

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

Chapter11: 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.)
Concentrated hydrochloric acid contains 1.00 mol HCl dissolved in 3.31 mol H2O. What is the mole fraction of HCl in concentrated hydrochloric acid? What is the molal concentration of HCl?
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.
Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
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Will red blood cells crenate, hemolyze, or remain unaffected when placed in each of the solutions in Problem 8-101?
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Refer to Figure 13.10 ( Sec. 13-4b) to determine whether these situations would result in an unsaturated, saturated, or supersaturated solution. 120. g RbCl is added to 100. g H2O at 50 °C. 30. g KCl is dissolved in 100. g H2O at 70 °C. 20. g NaCl is dissolved in 50. g H2O at 60 °C. Figure 13.10 Solubility of ionic compounds versus temperature.
What would be the freezing point of a solution formed by adding 1.0 mole of glucose (a molecular compound) to the following amounts of water? a. 250 g (0.25 kg) b. 500 g (0.500 kg) c. 1000 g (1.000 kg) d. 2000 g (2.000 kg)
The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?
Fructose, C6H12O6, is a sugar occurring in honey and fruits. The sweetest sugar, it is nearly twice as sweet as sucrose (cane or beet sugar). How much water should be added to 1.75 g of fructose to give a 0.125 m solution?
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?