Consider a solution of the solute CHCI3 in the solvent CHBR3. If the molality of the solution is 0.430 m, what is the freezing point ofthe solution ?Use only some of the following dataPure SubstanceFreezing PointKfCHCI3-63.40°C4.70°C/mCHBR38.70 °C15.00°C/m2.25°C-65.4°C-61.4°C6.45°CОООС

Dipression in freezing point (∆Tf) for any solution is directly proportional to the molality (m) of…

Answered: Consider a solution of the solute CHCI3…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.3QE

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Calculate the freezing point and normal boiling points of each of the following aqueous solutions. (a) 2.63 m acetic acid (b) 33.0 % by mass lactose, C12H22O11 (c) 32.15 mL of ethylene glycol, C2H6O2(d=1.113g/mL) in 624 mL of water (d=1.00g/mL)
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?
Juice (d=1.0g/mL) from freshly harvested grapes has about 24% sucrose by mass. What is the molality of sucrose, C12H22O11, in the grape juice after 25% (by mass) of the water content has been removed? Assume a volume of 15.0 L.
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 C. (a) What is the average molar mass of starch? (The result is an average because not all starch molecules are identical.) (b) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
An aqueous solution of a molecular compound freezes at 0.086C. What is the molality of the solution?
Which of the following will have the lowest total vapor pressure at 25C? a. pure water (vapor pressure = 23.8 torr at 25C) b. a solution of glucose in water with C6H12O6=0.01 c. a solution of sodium chloride in water with NaCl = 0.01 d. a solution of methanol in water with CH3OH=0.2 (Consider the vapor pressure of both methanol [143 torr at 25C] and water.)
Calculate the vapor pressure of water over each of the following ethylene glycol (C2H6O2) solutions at 22C (vppurewater=19.83mmHg). Ethylene glycol can be assumed to be nonvolatile. (a) Xethyleneglycol=0.288(b) percentethyleneglycolbymass=39.0(c) 2.42 m ethylene glycol
Vodka is advertised to be 80 proof. That means that the ethanol (C2H5OH) concentration is 40% (two significant figures) by volume. Assuming the density of the solution to be 1.0 g/mL, what is the freezing point of vodka? The density of ethanol is 0.789 g/mL.
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?

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