Crystallization is based on the :*Difference in melting pointO Difference in boiling pointDifference in pressureO Difference in solubility

The process in which a solid crystal of a solute is formed from the solution is known as…

Answered: Crystallization is based on the : O…

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 75AP

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Similar questions

Temperature influences solubility. Does temperature have the same effect on all substances? Justify your answer. (Hint: Consider Le Chateliers principle.)
Vapor-pressure lowering is a colligative property, as are freezing-point depression and boiling-point elevation. What is a colligative property? Why is the freezing point depressed for a solution as compared to the pure solvent? Why is the boiling point elevated for a solution as compared to the pure solvent? Explain how to calculate T for a freezing-point depression problem or a boiling-point elevation problem. Of the solvents listed in Table 10-5, which would have the largest freezing-point depression for a 0.50 molal solution? Which would have the smallest boiling-point elevation for a 0.50 molal solution? A common application of freezing-point depression and boiling-point elevation experiments is to provide a means to calculate the molar mass of a nonvolatile solute. What data are needed to calculate the molar mass of a nonvolatile solute? Explain how you would manipulate these data to calculate the molar mass of the nonvolatile solute.
The lattice enthalpy of sodium chloride, H for NaCl(s)Na+(g)+Cl(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCl(aq) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl. That is obtain the sum of H values for Na+(g)Na+(aq)Cl(g)Cl(aq) If the heat of hydration of Cl is 338 kJ/mol, what is the heat of hydration of Na+?
The vapor pressure of an aqueous solution of urea. CH4N2O, is 291.2 mmHg at a measured temperature. The vapor pressure of pure water at that temperature is 355.1 mmHg. Calculate the mole fraction of each component.
A forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?
The solubility of NaCl in water at 100 C is 39.1 g/100. g of water Calculate the boiling point of this solution. (Assume i = 1.85 for NaCl.)
Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?
What is the molar mass of a non-electrolyte when 780 g of this compound is added to 3.0 kg of water and the boiling point increases by 5.1 deg C? Kb for water is 0.51 deg C kg mol-1?.
At a certain temperature the vapor pressure of pure benzene and pure toluene are 380 torr and 130 torr, respectively. If the mole fraction of benzene is 0.48, what is the total vapor pressure.
14) Which of the following is true about the changes in energy associated with solubility? A) The enthalpy is more favorable for solid dissolution in liquids with increasing temperature. B) The enthalpy is more favorable for gas dissolution in liquids with increasing temperature. C) The entropy is more favorable for gas dissolution in liquids with increasing temperature. D) The entropy is more favorable for solid dissolution in liquids with increasing temperature.
Colligative Properties The freezing point of carbon tetrachloride (CCl4) is -23.0C. When a nonvolatile solute is added to this solvent, the temperature decreased to -26.7C. If the molality of the resulting solution is 0.124, what is the kf for CCl4?
A colloidal mixture has which of the following properties? (A) Lowers the vapor pressure of solvent; (B) Increases the boiling point of the solution; (C) Scatters the beam of light passing through the mixture. (D) All the above

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Crystallization is based on the : O Difference in melting point O Difference in boiling point Difference in pressure O Difference in solubility