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Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant Kf for water is 1.86 °C/m. Assume density of water is 1 g/ml.

Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant Kf for water is 1.86 °C/m. Assume density of water is 1 g/ml.

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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Data and Calculations: Pure Water Methanol in Water Volume of Water (ml) Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT, Calculate the molality m (K = 1.86 °C/m for water) Calculate number of moles 10.00 10.00 1.00 Tsolution= -5 Tsolvent = 0.7 AT, = Tsolvent – Tsolution = AT; = Kf.m → m = AT;/Kg = m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = Calculate the molar mass of methanol moles methanol = mass methanol / molar mass methanol → molar mass methanol = mass methanol / moles methanol molar mass methanol = 1.00 g / moles methanol %3D % error (actual molar mass of methanol = % error =[ |actual – experimental|/ actual ] x 100% 32.04 g/mol) Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant K, for water is 1.86 °C/m. Assume density of water is 1 g/ml.
Transcribed Image Text:Data and Calculations: Pure Water Methanol in Water Volume of Water (ml) Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT, Calculate the molality m (K = 1.86 °C/m for water) Calculate number of moles 10.00 10.00 1.00 Tsolution= -5 Tsolvent = 0.7 AT, = Tsolvent – Tsolution = AT; = Kf.m → m = AT;/Kg = m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = Calculate the molar mass of methanol moles methanol = mass methanol / molar mass methanol → molar mass methanol = mass methanol / moles methanol molar mass methanol = 1.00 g / moles methanol %3D % error (actual molar mass of methanol = % error =[ |actual – experimental|/ actual ] x 100% 32.04 g/mol) Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 mL of water? The freezing point depression constant K, for water is 1.86 °C/m. Assume density of water is 1 g/ml.
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