2. Aon is made by mixing 1.08 g of an unknown non-volatile non-electrolyte withg of benzene. The free10.00zing point of pure benzene is 5.5°C. The molalreezinng point depression constant, K for benzene is 5.12°C/molal. The following datawere obtained in a freezing point depression experimentTime, min Temperature CTemperatureC0.50.10.80.90.80.70.60.50.40.2-0.51.2Time min1.02.03.04.05.06.07.08.09.010.011.012.023.822.120.218.516.614.812.710.89.17.25.53.613.014.015.016.017.018.019.020.021.022.023.024.025.0Plot a graph of time/temperature, using the y-axis for temperature and the x-axisfor time. Determine the freezing point of the solution.A.2 De-tereine tHe alality of the solthon

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Answered: 2. A on is made by mixing 1.08 g of an…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter84: Fractional Distillation, Azeotropes

Section: Chapter Questions

Problem 1P

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The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mL
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal places
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
A. (see pic) B. When an electrolyte solution (such as NaCl) is added to ice, the ions have ____ with water molecules and thus ____ the ability of the water molecules to form a solid ice structure. C. Given that water's freezing pt is 0C and the fp depression constant is 1.86 Ckg/mol, calculate the fp depression for a 3.55 molal soln (moles/kg) of NaCl in water. Assume ideal behavior of the ions. D. Given that water's fp is 0C and fp depression constant is 1.86 Ckg/mol, calculate the fp depression for 3.55 molal solution for CaCl2 in water. Assume ideal behavior of the ions.
A student determines the molar mass of acetone, , She found that the equilibrium temperature of a mixture of ice and water was 1.0C on her thermometer. When she added 11.1g of her sample to the mixture, the temperature, after through stirring, fell to -3.0C. She then poured off the solution through a screen into a beaker. The mass of the solution was 90.4g. a. what was the freezing point depression? b. what was the molarity of the acetone? c. how much aceton was in the decanted solution? d. how much water was in the decanted solution? e. how much acetone would there bein a solution containing 1kg of water and acetone at the same concentration as she has in herexperiment? f. what did she find to be the molar mass of aceton, assumingshe made the calculation properly?
1.0 GRAMS of an electrolyte was dissolved in 29 grams of water, the resulting solution was found to have a molarity of 0.437 mol / L. The freezing point of the solution was determined to be -4.96°C. The freezing point depression constant for water is -1.86°C and pure water may be assumed to freeze at 0°C. If the molecular weight of the electrolyte is 179.7 g/mol and it takes 15 minutes to perform the experiment, how much water was used (grams) ?
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the osmotic pressure in atm.
Calculate the mass of naphthalene required to give a freezing point depression of 2.9°C when dissolved in the amount of cyclohexane specified in the procedure(15mL). For this prelab problem you should use the density of cyclohexane as being 0.7781 g/mL at room temperature.

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