Data and Calculations: Pure Water Methanol in Water Volume of Water (ml) 10.00 10.00 Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT- Calculate the molality m (K, = 1.86 °C/m for water) 1.00 Tsolvent = 1 AT, = Tsolvent – Tsotution = AT; = Kr.m → m = AT;/Kf = Tsotution= -4.5 m = moles methanol/ Kg solvent → moles methanol m x Kg solvent = Calculate number of moles 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 % 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 Kf for water is 1.86 °C/m. Assume density of water is 1 g/ml.

Data and Calculations: Pure Water Methanol in Water Volume of Water (ml) 10.00 10.00 Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT- Calculate the molality m (K, = 1.86 °C/m for water) 1.00 Tsolvent = 1 AT, = Tsolvent – Tsotution = AT; = Kr.m → m = AT;/Kf = Tsotution= -4.5 m = moles methanol/ Kg solvent → moles methanol m x Kg solvent = Calculate number of moles 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 % 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 Kf for water is 1.86 °C/m. Assume density of water is 1 g/ml.

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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i app.101edu.co Question 6 of 20 Submit A solution is made from 220.0 g sucrose (C12H»O11, MM = 342.3 g/mol) dissolved to a total volume of 551 mL of water at a temperature atm of 52.0 °C. Calculate the osmotic pressure of solution.R= 0.08206 L·atm/K-mol 1 3 4 9. +/- x 100 Showal Question 8pg 27207792011jpg -Question 15jpg 656 PM 77F Mostly coudy a 2/12/202 O Type here to search
A 0.25g of a certain substance is dissolved in 60g of water. The freezing point of thesolution is - 0.050 °C. Knowing that the substance has a van't Hoff factor of 1 and isnon-volatile, what is the molar mass of the substance? (Freezing point depression of water =- 1.86 °C/m)A. 0,00016 g/molB. 156.25 g/molC. 186.54 g/molD. 1.86 g/molWhat is the osmotic pressure (at 20 °C) of a solution made by dissolving 13g of sucrosein 117g of water? The total volume of the solution is 125mL at 20 °C.A. 7.31 atmB. 0.30 atmC. 342 atmD. 0.08 atm
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