A solution is made by mixing 5.40 g of toluene, CHg(1), with 954. mL of chloroform, CHCI3(1). Calculate the concentration of the solute in the solution using the units given below. (Density of = 0.867 g/mL. Density of chloroform = 1.49 g/mL. Assume volumes mix additively.) toluene %3D Enter your answers in decimal form to 3 significant figures. Do not enter units since they are already provided. Molar: M molal: mole fraction: mass percent: %(m/m) percent volume: %(v/v)

A solution is made by mixing 5.40 g of toluene, CHg(1), with 954. mL of chloroform, CHCI3(1). Calculate the concentration of the solute in the solution using the units given below. (Density of = 0.867 g/mL. Density of chloroform = 1.49 g/mL. Assume volumes mix additively.) toluene %3D Enter your answers in decimal form to 3 significant figures. Do not enter units since they are already provided. Molar: M molal: mole fraction: mass percent: %(m/m) percent volume: %(v/v)

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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Part 1. One gram of caffeine dissolves in 55 ml of water; 7 ml of dichloromethane (DCM); 530 ml of diethyl ether; and 100 ml of benzene. Covert the solubility of caffeine in these four solvents into units of mg/ml. a) Solubility of caffeine in mg/ml in water: b) Solubility of caffeine in mg/ml in DCM: c) Solubility of caffeine in mg/ml in Diethyl Ether: d) Solubility of caffeine in mg/ml in Benzene: Which is the optimal solvent to extract caffeine from an aqueous solution? Why? Part 1 Continued: Use intermolecular force (IMF), provide a brief explanation on the solubility of caffeine in water, diethyl ether, observed above. (Hint: draw the skeletal structures for caffeine, DCM and diethyl ether)
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1 4 7 8 When 2.19 g of a certain molecular compound X are dissolved in 100. g of formamide (NH, COH), the freezing point of the solution is measured to be - 0.4 °C. Calculate the molar mass of X. If you need any additional information on formamide, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits. Submit Assign Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acces
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STARTING AMOUNT X What is the molality of lithium ions in an aqueous solution made up of 0.302 m LisPO4 assuming the compound dissociates completely? ADD FACTOR x( ) 0.302 115.79 0.101 DELETE t 35.0 1000 kg solvent m Li³PO4 mol Li³PO4 6.022 x 10²3 1.21 mol Lit g Lit = ANSWER 3 0.906 4 0.001 g solvent g Li3PO4 RESET 3 1 m Lit
Be sure to answer all parts. What are the boiling point and freezing point of a 1.47 m solution of naphthalene in benzene? (The boiling point and freezing point of benzene are 80.1°C and 5.5°C respectively. The boiling point elevation constant for benzene is 2.53°C/m, and the freezing point depression constant for benzene is 5.120°C/m.) Boiling point = Freezing point = °C < Prev Next Ji 14 of 20 arch
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A student determined the average molarity of their sample of acetic acid to be 0.536 M. Calculate the (w/w)% of the solution. Assume the density of this solution is that of pure water, dH2O = 1000. g/L. Enter a number without the '%' symbol. (I'm struggling to find the Volume from the attached equation(s) that are "meant" to be used for this problem)