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Given this, if 2.5 g of a certain ionic compound that breaks into three ions is added to 150. mL of water (1.0 g/mL density) the Tr of the resulting solution is -1.5 °C. What is the molality of this solution? What is the molar mass of the ionic compound? Remember to account for the number of ions, we place an "i" in the equation from before: ATf=i Kt m. Can you suggest a compound that this "certain ionic compound" could be?

Given this, if 2.5 g of a certain ionic compound that breaks into three ions is added to 150. mL of water (1.0 g/mL density) the Tr of the resulting solution is -1.5 °C. What is the molality of this solution? What is the molar mass of the ionic compound? Remember to account for the number of ions, we place an "i" in the equation from before: ATf=i Kt m. Can you suggest a compound that this "certain ionic compound" could be?

Chemistry
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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. Freezing Point Depression may be used to find the molar mass of a solid. The way this is done is that the Tr for a solution of the solid is measured. From the ATf and the known value of Kr, the molality is found. (It would have to be known how many particles the compound breaks into on dissolving). Since molality is moles solute per kg solvent, it follows that multiplying molality by the kg of solvent yields the number of moles. Dividing the grams solute used to make the solution by moles gives the molar mass. Given this, if 2.5 g of a certain ionic compound that breaks into three ions is added to 150. mLof water (1.0 g/mL density) the Tr of the resulting solution is -1.5 °C. What is the molality of this solution? What is the molar mass of the ionic compound? Remember to account for the number of ions, we place an "i" in the equation from before: ATr= i Kt m. Can you suggest a compound that this "certain ionic compound" could be?
Transcribed Image Text:. Freezing Point Depression may be used to find the molar mass of a solid. The way this is done is that the Tr for a solution of the solid is measured. From the ATf and the known value of Kr, the molality is found. (It would have to be known how many particles the compound breaks into on dissolving). Since molality is moles solute per kg solvent, it follows that multiplying molality by the kg of solvent yields the number of moles. Dividing the grams solute used to make the solution by moles gives the molar mass. Given this, if 2.5 g of a certain ionic compound that breaks into three ions is added to 150. mLof water (1.0 g/mL density) the Tr of the resulting solution is -1.5 °C. What is the molality of this solution? What is the molar mass of the ionic compound? Remember to account for the number of ions, we place an "i" in the equation from before: ATr= i Kt m. Can you suggest a compound that this "certain ionic compound" could be?
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