The freezing point of water is 0.00°C at 1 atmosphere. How many grams of calcium iodide (293.9 g/mol), must be dissolved in 207.0 grams of water to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. | Kp C/m) Kf(°C/m) Solvent Formula Water H20 0.512 1.86 Ethanol CH;CH,OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g calcium iodide.

The freezing point of water is 0.00°C at 1 atmosphere. How many grams of calcium iodide (293.9 g/mol), must be dissolved in 207.0 grams of water to reduce the freezing point by 0.400°C ? Refer to the table for the necessary boiling or freezing point constant. | Kp C/m) Kf(°C/m) Solvent Formula Water H20 0.512 1.86 Ethanol CH;CH,OH 1.22 1.99 Chloroform CHCI3 3.67 Benzene 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02 g calcium iodide.

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 12.98QE

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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.)
Calcium chloride, CaCl2, has been used to melt ice from roadways. Given that the saturated solution is 32% CaCl2 by mass, estimate the freezing point.
An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of 5.20C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
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