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Unformatted text preview: rose (kmr2427) Homework 2 fakhreddine (51615) 1 This printout should have 31 questions. Multiplechoice questions may continue on the next column or page find all choices before answering. 001 1.0 points The mole fraction of a certain nonelectrolyte compound in a solution containing only that substance and water is 0.100. The molecular weight of water is 18.0 g/mol. What addi tional information is needed to determine the molality of the solution? 1. The mole fraction of water in the solu tion. 2. The density of the solution. 3. No additional information; the molality can be calculated from the information given. correct 4. The density of the solute. 5. The molecular weight of the compound. Explanation: Here we can assume that we have 1 mol total. (In fact, we can choose any number of moles, but the math is easier if you choose 1 mol.) If the mole fraction of the substance is 0.100, you can then assume that you have 0.100 mol of the substance, and the remaining 0.900 mol is H 2 O. The molality of a solution is determined by the following formula: m = mol solute kg solvent Weve already assumed that we have 0.100 mol of solute, and we can determine the kg of H 2 O in the usual way: . 900 mol H 2 O parenleftbigg 18 . 0 g 1 mol parenrightbiggparenleftbigg 1 kg 1000 g parenrightbigg = 0.0162 kg, and we can calculate the molality of this solu tion: m = . 100 mol . 0162 kg H 2 O = 6.17 m So, it is possible to determine the molality of this solution without any additional informa tion. 002 1.0 points What additional information, if any, would enable you to calculate the molality of a 7.35 molar solution of a nonelectrolyte solid dis solved in water? 1. None is needed. 2. Only the density of the solution would be needed. 3. Both the density of the solution and the molecular weight of the solute would be needed. correct 4. Only the density of water would be needed. 5. Only the molecular weight of the solute would be needed. Explanation: molarity = mol solute L solution molality = mol solute kg solvent The density of the solution can be used to convert volume (1 L) of solution into mass of solution. Then the molecular weight of the solute (given or calculated from the formula) can be used to convert the number of moles solute in 1 L solution into mass of solute in grams. The mass of the solvent is the difference between the mass of the solution and the mass of the solute (both of which have been calculated). Substitute the values into the molality formula and calculate. 003 1.0 points A solution is 40.0% silver nitrate (AgNO 3 ) by mass. The density of this solution is 1.48 grams/mL. The formula weight of AgNO 3 is 170 grams/mol. Calculate the molality of AgNO 3 in this solution....
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This note was uploaded on 03/01/2011 for the course CH 302 taught by Professor Holcombe during the Spring '07 term at University of Texas at Austin.
 Spring '07
 Holcombe

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