12.7 Let Wbe the weight percent of maltose in an aqueous so-lution. The following freezing-point depressions are observedfor maltose (aq) solutions:W3.006.009.0012.00AT,/°C-0.169-0.352-0.550-0.765(a) Show that the equation AT₁ = -km gives M₁ = -k+WB/(ATW), where w₁ and WA are the masses of B and A in thesolution. (b) Plot the calculated molecular weights vs. W andextrapolate to zero concentration to find the true molecularweight.

Answered: Image /qna-images/answer/4e7927d0-aaf6-4e05-bc92-b4a9eccab4c6.jpg

Answered: 12.7 Let Wbe the weight percent of…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 46P

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The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following: (a) the molality of the solution (b) the weight percent of HCl in the solution
Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/mol
The following table presents the solubilities of severalgases in water at 25 °C under a total pressure of gas andwater vapor of 1 atm. (a) What volume of CH4(g) understandard conditions of temperature and pressure is containedin 4.0 L of a saturated solution at 25 °C? (b) Thesolubilities (in water) of the hydrocarbons are as follows:methane < ethane < ethylene. Is this because ethyleneis the most polar molecule? (c) What intermolecularinteractions can these hydrocarbons have with water?(d) Draw the Lewis dot structures for the three hydrocarbons.Which of these hydrocarbons possess p bonds?Based on their solubilities, would you say π bonds aremore or less polarizable than s bonds? (e) Explain whyNO is more soluble in water than either N2 or O2. (f) H2S is more water-soluble than almost all the other gasesin table. What intermolecular forces is H2S likely to havewith water? (g) SO2 is by far the most water-soluble gasin table. What intermolecular forces is SO2 likely to havewith…
The presence of the radioactive gas radon (Rn) in well waterpresents a possible health hazard in parts of the UnitedStates. (a) Assuming that the solubility of radon in waterwith 1 atm pressure of the gas over the water at 30 °C is7.27 * 10-3 M, what is the Henry’s law constant for radon (c) The free-base form of cocaine has a solubility of 1.00 g in6.70 mL ethanol (CH3CH2OH). Calculate the molarityof a saturated solution of the free-base form of cocaine inethanol.(d) The hydrochloride form of cocaine has a solubility of1.00 g in 0.400 mL water. Calculate the molarity of a saturatedsolution of the hydrochloride form of cocaine inwater.(e) How many mL of a concentrated 18.0 M HCl aqueoussolution would it take to convert 1.00 kilograms(a “kilo”) of the free-base form of cocaine into its hydrochlorideform?
Henry’s law constant for CO2 in the water at 25 °C is 3.1 * 10-2 M atm-1. (a) What is the solubility of CO2 in the water at this temperature if the solution is in contact with air at normal atmospheric pressure?
Can you please answer number 8 and show all of the steps to the solution
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. 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. 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 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)

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