a) What would you expect the magnitude and sign of ΔHSOLUTE, ΔHSOLVENT, and ΔHMIXING to be for CH2Cl2 as solute and acetone as solvent? Circle your choices below. Then, fill in the most important IM force that exists between solute molecules, between solvent molecules and between solute and solvent molecules. Magnitude Sign Most important force between Hsolute small. moderate large pos neg solute&solute Hsolvent small. moderate large pos neg solvent&solvent Hmixing small. moderate large pos neg solute&solvent b) Based on this, what is the overall enthalpy change (HSOLUTION) for dissolving CH2Cl2 in acetone expected to be? (negative/positive/ near zero). Would you expect CH2Cl2 to dissolve in acetone? (yes/no). Explain your answers to both of the questions above. Consider the energy and entropy contributions discussed in class

a) What would you expect the magnitude and sign of ΔHSOLUTE, ΔHSOLVENT, and ΔHMIXING to be for CH2Cl2 as solute and acetone as solvent? Circle your choices below. Then, fill in the most important IM force that exists between solute molecules, between solvent molecules and between solute and solvent molecules. Magnitude Sign Most important force between Hsolute small. moderate large pos neg solute&solute Hsolvent small. moderate large pos neg solvent&solvent Hmixing small. moderate large pos neg solute&solvent b) Based on this, what is the overall enthalpy change (HSOLUTION) for dissolving CH2Cl2 in acetone expected to be? (negative/positive/ near zero). Would you expect CH2Cl2 to dissolve in acetone? (yes/no). Explain your answers to both of the questions above. Consider the energy and entropy contributions discussed in class

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section13.7: Colligative Properties Of Solutions

Problem 13.11PSP

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a) What would you expect the magnitude and sign of ΔHSOLUTE, ΔHSOLVENT, and ΔHMIXING to be for CH2Cl2 as solute and acetone as solvent? Circle your choices below. Then, fill in the most important IM force that exists between solute molecules, between solvent molecules and between solute and solvent molecules. b) Based on this, what is the overall enthalpy change (HSOLUTION) for dissolving CH2Cl2 in acetone expected to be? (negative/positive/ near zero). Would you expect CH2Cl2 to dissolve in acetone? (yes/no). Explain your answers to both of the questions above. Consider the energy and entropy
The osmotic pressure of an aqueous solution at 300K is 250.0 kPa. (1)Calculate the molarity of solute (impurity) M (mol/m3)=[M]; (2) Calculate the molality of solute (impurity) b (mol/kg)=[b]; Calculate the freezing point of the solution T(oC)=[T]. Please pay attention to the sign. The cryoscopic constant Kf=1.86Kkgmol-1
calculate the sulablity Iat 25 Celsius of Ni(OH)2 pure water and then .01 80 M NaOH solution. Ksp of Ni(OH)2 is 5.48x10^16 additional info in the picture
Test Tube Solute Mass of Deionized Water (g) Mass of solute (g) Freezing Point (C) 1 None 4.140g X 0.0 2 NaCl 4.021g 0.235g -3.8 3 Unknown A 4.000g 0.233g -.17 4 Unknown B 4.036g 0.231g -0.6 1. Use the following steps to determine molar mass of the solute in test tubes 2,3 and 4. a. Calculate the freezing point depression for each solution relative to pure water using equation ΔTFP = TFP,solution - TFP,purewater Sample Calulation for test tube 2: Sample Calulation for test tube 3: b. Solve for motility. (ΔTFP =iKfm)
What is the molality in mol/kg of a solution if the temperature difference ΔT between the solvent and the solution is 2? Kf for the solvent used (cyclohexane) is 20.8ºC/m. Enter your answer with THREE decimals places, and do not write the unit. Example: 0.023
For freezing point depression what is delta T mean? Is it the temperature of the solvent minus the temperature of the solution at freezing point?
A 6.2 M aqueous solution of a non-electrolyte (MW=120.0 g/mole) has a density of 1.24 g/ml. Answer the following. Mole fraction water __________________ Molality __________________ % by mass water __________________
Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: T = T(solution) - T(pure solvent) m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb(°C / m) Kf(°C / m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02
Compounds A and B form a liquid solution in all proportions, but do not form solid solutions. The phase diagram of this system is shown in the accompanying photo. 4.65 moles of A and 1.55 moles of B are mixed to form a liquid solution at 75(C. The mixture is then cooled to 35oC. a.) Determine the mole fraction of B in the liquid phase at 35oC. b.) Compute the number of moles of solid A in equilibrium with the liquid solution at 35oC.
ΔHsolution of NaOH(s) Phase Change:Mass of NaOH: 2.330 gΔT for reaction A : 10.0 °C Calculate the total number of calories produced by the solution. (Answer must be in cal) Calculate the ΔHsolution for sodium hydroxide. (Answer must be in kJ mol -1)
In class, we derived the expression:ln XA =(ΔvH/R) ((1/T)-(1/T°))where A represents the solvent (and B would represent the solute, such that XA + XB = 1).Using the approximations given below, derive the expression:∆Tb = XB (RT°2/ΔvH)where ∆Tb is the change in boiling point between the solution and the pure liquid, T − T°.Approximations:ln(1 − X) ≈ −XTT° ≈ T°2Note: this derived expression is often simplified in General Chemistry as ∆Tb = Kbm where Kb is the boiling point elevation constant, and m is the molality.
In the determination of molar mass of an unknown substance by ebullioscopic constant, 30 mL of acetone (C3H6O) was placed in a test tube with thermometer and glass tubing and subjected to water bath. Upon boiling, the temperature reads 56 deg C. For the boiling point of unknown-acetone solution, you prepared the solution by mixing 1.60 g of unknown solute in the 30 mL acetone and subjected it again to water bath. The boiling temperature of the solution is 56.68 deg C. The density of acetone = 0.9849 g/mL and the Kb of acetone = 1.67 degC/kg

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	Magnitude	Sign	Most important force between
Hsolute	small. moderate large	pos neg	solute&solute
Hsolvent	small. moderate large	pos neg	solvent&solvent
Hmixing	small. moderate large	pos neg	solute&solvent