The freezing point of a solution that contains 1.1 g of an unknown compound, (A),dissolved in 12 g of benzene is found to be 2.97 °C.The freezing point of pure benzene is 5.48 °C. The freezing point depression constantof benzene is 5.12 °C/molal. What is the molecular weight of the unknowncompound?

The freezing point of solvent decreases on addition of non volatile solute as the solute occupies…

Answered: The freezing point of a solution that…

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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A chemist is studying the properties of a small organic compound. One of the properties under study is the effect on osmotic pressure. (A) When 0.517 g of the compound are dissolved in enough water to make a total volume of 50.0 mL, the resulting solution has an osmotic pressure of 4.18 atm at 23.0°C. What is the molar mass of the organic compound? Assume the compound does not dissociate in water and is nonvolatile. (B) Analysis shows that the compound is 59.96% C, 13.42% H, and the rest O by mass. Determine the empirical formula of the compound. (Hint: See Chapter 4.) (C) Draw two potential Lewis structures for the compound based on the formula from (B). One of the Lewis structures should be able to form H-bonds, while the other should not. Clearly identify which structure is which.
A certain liquid X has a normal freezing point of -4.00 °C and a freezing point depression constant K = 6.25 °C-kg-mol some iron(III) chloride (FeCl3) in 600. g of X. This solution freezes at -5.2 °C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits. g . A solution is prepared by dissolv 0 || cue X
Identify the following statements about the principles of solubility. Each statement refers to the solubility of the solute mentioned. Increasing the temperature of a solution of a salt that has an enthalpy of solution of 0.0 kJ/mol. Increasing the overall pressure on a solution of NaCl dissolved in water. Reducing the partial pressure of nitrogen gas over a solution of nitrogen dissolved in hexane. Changing the solvent for a solution of C5H12 from methanol (CH3OH) to pentanol (C5H11OH). Changing the solvent for a solution of CH3OH from pentanol(C5H11OH) to ethanol(C2H5OH) Increasing the temperature of a solution of KOH dissolved in water. This salt has an exothermic enthalpy of solution. Raising the partial pressure of CO2 gas on a solution of CO2 dissolved in water.
When 40.0 grams of an unknown compound are dissolved in 500. grams of benzene, the freezing point of the resulting solution is 3.77°C. The freezing point of pure benzene is 5.48 °C, and the Kf for benzene is 5.12°C/m. What is the molecular weight of the unknown compound?
A 3.40-g sample of a mixture of naphthalene (C₁₀H₈) and pyrene (C₁₆H₁₀) is dissolved in 35.0 g benzene (C₆H₆). The freezing point of the solution is 2.29°C. What is the mass (in grams) of the naphthalene in the sample mixture? The freezing point of benzene is 5.51°C and Kf is 5.12°C･kg/mol.
An online study examined the lowering of freezing point when 0.222 g of an unknown molecular solute was dissolved in 11.45 g of cyclohexane. The freezing point of pure cyclohexane was 6.6oC and the freezing point of the solution of the unknown was 3.3oC. The freezing point lowering constant, Kf, for cyclohexane is 20.0oC*(kg/mol). What is the molar mass of the unknown in g/mol? Enter your answer without units.
When 498. mg of a certain molecular compound X are dissolved in 25.0 g of dibenzyl ether ((C6H-CH₂)₂O), the freezing point of the solution is measured to be 0.8 °C. Calculate the molar mass of X. If you need any additional information on dibenzyl ether, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits. 0 8 0.2 ロ・ロ X G
When 571. mg of a certain molecular compound X are dissolved in 60.0 g of benzene (CH), the freezing point of the solution is measured to be 4.8 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits. 0 X x10 S
When 6.31 g of a certain nonvolatile solute is dissolved in 505 g of water, the freezing point of the resultant aqueous solution is 0.55˚C lower than that of pure water. The cryoscopic constant for water is Kf = 1.856. Given this information, what is the molar mass of the solute species, in g/mol?
15.2 g of camphor dissolved in naphthalene lower the freezing temperature of naphthalene from 80.0 °C to 75.0 °C. What is the mass of naphthalene? The molal freezing depression point constant for naphthalene is: Kf = 7.00 °C/m . Both naphthalene and camphor are non-electrolytes, and the molar mass of camphor is about 152 g/mol.
If 3.42 grams of a nonpolar molecular compound, dissolved in 41.8 grams benzene, begins to freeze at 1.17 °C, what is its molar mass? The freezing point of pure benzene is 5.50 °C, and the freezing point depression constant is 5.12 K kg mol-1.
The solubility limit of a solute at 20. °C and 1.0 atm is 13.8 g of solute per 1 L of water. What will MOST likely happen when 12.0 g of solute are added to 1 L of pure water and the solution is mixed well (at the same conditions)?

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