The normal freezing point of a certain liquid X is-3.30 °C, but when 22. g of iron(III) nitrate (Fe(NO,),) are dissolved in 150. g of X the solution freezes at -7.5 °C instead. Use this information to calculate the molal freezing point depression constant K, of X Round your answer to 2 significant digits. *C-kg mol -0- 0.8

The normal freezing point of a certain liquid X is-3.30 °C, but when 22. g of iron(III) nitrate (Fe(NO,),) are dissolved in 150. g of X the solution freezes at -7.5 °C instead. Use this information to calculate the molal freezing point depression constant K, of X Round your answer to 2 significant digits. *C-kg mol -0- 0.8

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

The freezing point of an aqueous solution containing a non electrolyte solute is -2.79 degree celcius. What is the boiling point of this solution? For water Kb=0.51 degree celcius kg/ mol and Kf=/1.86 degree celcius kg /mol.
Which statement below best explains why the lowering of the vapor pressure by a nonvolatile solute results in a higher boiling point?
A certain substance X' has a normal freezing point of 4.1 °C and a molal freezing point depression constant K, -4.14 °C-kg-mol. A solution is prepared by dissolving some urea ((NH,),CO) ir in 250. g of X. This solution freezes at 0.7 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits. 0. 0.9 ? 11
Arrange the following compound base on its decreasing solubility in water А. B. H H H H HHH H-Ċ-ċ-ċ-H H-Ć- C-C-C-H нн H H H H. H H H H H H. H-C Ċ-H С. D. H. H. H. H. H. A>B>C>D D>C>B>A C>A>B>D B>A>C>D T-
Use the information to answer the following question. The solubility of a substance at varying temperatures is listed: - 1.1 g solute per 100 g solution at 20°C -0.8g of solute per 100 g solution at 30°C - 0.4 g of solute per 100 g solution at 40°C Based on the data, what can you infer about this solute? O A. The solute is a gas. O B The solute is a solid. OC The solute is a liquid. O D. The solute is concentrated.
8. A certain substance X has a normal freezing point of -8.4 °C and a molal freezing point depression constant K, = 2.33 °C·kg-mol Calculate the freezing point of a solution made of 63.48 g of urea ((NH2),CO) dissolved in 700. g of X. Round your answer to 3 significant digits. 0c Submit Assignment Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibility II Finder F11 F12 F9 F10 F8
A solution of propylene glycol (antifreeze) in the car's radiator has a freezing point of -20°c. What is the molality of the solution?
A solution of a nonelectrolyte solution contains 39.0 g of solute dissolved in 242.0 g of water. The freezing point of the water is observed to be -4.00˚C. The Kf for water is 1.86 ˚C/m and normal freezing point of 0.00˚C. What is the molar mass of the substance? -2.50˚C. The Kf for water is 1.86 ˚C/m and normal freezing point of 0.00˚C. What is the molar mass of the substance?
Determine the molar mass of the solute if a solution contains 25 grams of an unknown non-volatile, non-dissociating solute is dissolved in 250 grams of water. The freezing point of the solution is –0. 356 C. Given = Required = Equation = Solution = Answer =
* 00 LL LI #3 The normal freezing point of a certain liquid X is -2.70 °C, but when 43.3 g of potassium bromide (KBr) are dissolved in 400. g of X the solution freezes at -9.6 °C instead. Use this information to calculate the molal freezing point depression constant K, of X. Round your answer to 2 significant digits. °C-kg K. mol Check Save For Later Submit Assignme O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Center Accessibil MacBook Pro 114 F8 F3 F4 $4 3. 5. 6. P. A G H. K. B alt alt option command command option
A certain substance X has a normal freezing point of - 10.2 °C and a molal freezing point depression constant (NH.), CO): K, = 3.63 °C kg mol . A solution is prepared by dissolving some urea in 150. g of X. This solution freezes at - 16.4 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits. I Don't Know Submit 72022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center Accessibility tv 23 DII 80 F9 esc F6 F7 F8 F4 F5 F2 F3
An aqueous solution containing 17.5 g of an unknown molecular (nonelectrolyte) compound in 100.0 g of water has a freezing point of -1.8 degrees celsius. Calculate the molar mass of the unkown compound.