You were tasked explore the different colligative properties of solution in your Chem 16.1 Lab class. The experiments you did were based from your Chem 16.1 lab manual. The results from your experiment are shown in your data sheet below. Complete your data sheet. A. FREEZING POINT DEPRESSION Kf (°C/m) of water 1.86 Freezing Point of Water, °C 0.00 SOLVENT 100.0 g water Mass / Volume added Added reagentMolecular Weight van't Hoff Factor m Freezing Point 20.0 g Naci 58.44 25.0 g Li2S04 109.94 0.150 M 10.0 mL ethanol B. BOILING POINT ELEVATION Kb (°C/m) of water 0.5121 Boiling Point of Water, °C 100.0 SOLVENT 100.0 g water Mass / Volume added Added reagentMolecular Weight van't Hoff Factor m Boiling Point 20.0 g Nacl 58.44 25.0 g AI(NO3)3 213 0.200 10.0 mL Mglycerol

You were tasked explore the different colligative properties of solution in your Chem 16.1 Lab class. The experiments you did were based from your Chem 16.1 lab manual. The results from your experiment are shown in your data sheet below. Complete your data sheet. A. FREEZING POINT DEPRESSION Kf (°C/m) of water 1.86 Freezing Point of Water, °C 0.00 SOLVENT 100.0 g water Mass / Volume added Added reagentMolecular Weight van't Hoff Factor m Freezing Point 20.0 g Naci 58.44 25.0 g Li2S04 109.94 0.150 M 10.0 mL ethanol B. BOILING POINT ELEVATION Kb (°C/m) of water 0.5121 Boiling Point of Water, °C 100.0 SOLVENT 100.0 g water Mass / Volume added Added reagentMolecular Weight van't Hoff Factor m Boiling Point 20.0 g Nacl 58.44 25.0 g AI(NO3)3 213 0.200 10.0 mL Mglycerol

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...

See similar textbooks

Similar questions

A solution was prepared by dissolving an unknown amount of carbon tetrachloride into 51.00 g of benzene. The freezing point of the solution was measured at 1.5 °C. What is the mass percent of carbon tetrachloride in the solution? What is the molarity of the CCla solution? The density of the solution is 0.880 g/mL. Use table 13.4, below, for more information. 43. Mass% of carbon tetrachloride: Molarity of carbon tetrachloride solution:
This question is very difficult to me. I need help with this one.
Which property of a pure solvent will increase in the presence of dissolved solute particles? Which colligative property of a solution depends on the mole fraction of the solute particles? Which two properties of a pure solvent decreases in the presence of dissolved solute particles?
4*) Consider the three solutions listed below that are prepared by dissolving 1 mole of the indicated solute in 1 kg of water: Solution 1: 1-mole KBr Solution 2: 1 mole CO(NH2)2Solution 3: 1 mole Na2SO4 a)Which solution will have the lowest vapor pressure of water above it? Explain. b)Which solution will have the highest vapor pressure of water above it? Explain.
For each case,compute the vapor pressure of the solution at 25°C. The vapor pressure of pure water at this temperature is 23.756mmHg. a. 10 g urea in 100g solvent b. 0.25mol ol non volatile solute in 150g solvent
Name Time M T W R F The freezing point of pure benzene (CH,) is 5.50°C. The freezing point of a solution containing 5.00 g of an unknown non-dissociating solute in 444 g of benzene is 5.07°C. K, of benzene = 4.90°C/m. Show complete calculations for each question below. 1. What is the freezing point depression for this solution?
Assuming 100% dissociation, calculate the freezing point and the boiling point of 0.570 mol K3PO4 in 1.00 kg water. You may need the colligative constants for water.
9.)Moles of solute (mol)Use the molality to convert kg of solvent to moles of solute. 10.)Molar mass of the solute (g/mol)Use the mass of solute you weighed out in the simulation and moles of solute calculated in the previous step. 11.)Percent error for the molar mass of the solute % error=∣∣∣true value−experiment valuetrue value∣∣∣×100% error=|true value-experiment valuetrue value|×100 The true value for the molar mass of NaCl is 58.44 g/mol. Information found so far: Mass NaCl (g) 5.8871 Vol of water mL 100.0 Mass ice (g) 51.5023 Freezing point of solution (C) -2.85 Predicted value of i for NaCl is 2 Molarity of solution (m) 0.76612903225806 Mass of solvent in grams 151.5g Mass of solvent in kg 0.1515kg
Fill up and identify the missing :
1. The freezing point datas of pure water and 150 grams of H20 that includes 10 g of sucrose (C12H22011) are given below. According to these datas, calculate the molecular weight of 10 g sucrose (C12H22011) dissolved in 150 g of H2O. a. Freezing point of pure water, Tf = 0 °C Freezing point of solution, Tf = -0. 34 °C Freezing point depression, ATf = ... (0- (-0.34)) = 0.34°C Molal freezing point depression of water, Kf = •.1.86°C kg/mol b. Molality of solution, m = . c. Molecular weight of solute, MWs = .. %3D 2. Find the theoretical molecular weight of solute in literature and calculate the percentage error in molecular weight. MWs, real = Error%=
During an experiment, 0.402 g of an unknown solid was dissolved in 20.1 mL of water. The morality of the solution, 0.250 mom/kg, was determined by freezing point depression. What is the molar mass of the unknown solute? (Assume density of water = 1 g/mL)
Match the following. Drag the terms on the left to the appropriate blanks on the right. Reset Help 0.020 MNH4 Cl solution that is most strongly dependent upon pressure 1. 0.0050 MCO2 2. - highest boiling point 0.050 MC6H12O6 (aqueous) 3. - solution of ionic compound with highest freezing point 0.010 mAl(NO3)3 0.050 mNaCi 4. - solution with AT, 0.026° C 5. - largest van't Hoff factor