We obtain the value of the ebulloscopic increase of a solution with respect to the solvent. The measured boiling point for the solvent, with its absolute error, is 177±2°C; and that of the solution, 183±4°C. Indicate the statement that is correct.(A). From this experiment it is not possible to give a significant value for the ebulloscopic increase.(B). The ebulloscopic increase is 6±4°C.(C). The relative error in the measurement of the boiling temperature of the solution is twice the relative error in the measurement of the boiling temperature of the pure solvent.(D). The relative error of ebulloscopic magnification is, in round numbers, 2%.

We obtain the value of the ebulloscopic increase of a solution with respect to the solvent. The measured boiling point for the solvent, with its absolute error, is 177±2°C; and that of the solution, 183±4°C. Indicate the statement that is correct.(A). From this experiment it is not possible to give a significant value for the ebulloscopic increase.(B). The ebulloscopic increase is 6±4°C.(C). The relative error in the measurement of the boiling temperature of the solution is twice the relative error in the measurement of the boiling temperature of the pure solvent.(D). The relative error of ebulloscopic magnification is, in round numbers, 2%.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter7: Equilibria In Multiple-component Systems

Section: Chapter Questions

Problem 7.81E

See similar textbooks

Similar questions

When 14.3 g of a certain molecular compound X are dissolved in 85.0 g of benzene C6H6, the freezing point of the solution is measured to be 0.5 °C. Calculate the molar mass of X. molal freezing point depression constant (Kf)°C·kg·mol−1 of benzen is 5.07 If you need any additional information on benzene, 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.
1. (a) In the experiment carried out to determine the degree of association of benzoic acid in benzene (C6H6), the cooling curves of pure benzene and benzoic acid solution prepared by dissolving 0.358 g benzoic acid in 20 mL of benzene were obtained by using Beckmann thermometer, calibrated before the experiment. The cooling curves are given in the figure below. Calculate the degree of association of benzoic acid in benzene for the given solution. Ky= 5.055 K kg.mol-¹, dbenzene- 0.876 g.cm³, MBenzoic acid=122.12 g.mol-¹ T(°C) 2.88 2.38 Benzene Solution t(min)
It is found that the boiling point of a binary solution of A and B with xA = 0.479 is 88°C. At this temperature the vapor pressures of pure A and B are 130.1 kPa and 74.9 kPa, respectively. (a) Is this solution ideal? (b) What is the initial composition of the vapor above the solution?
(a) Explain why a solution of chloroform and acetone shows negative deviation from Raoult’s law.(b) Phenol associates in benzene to certain extent to form a dimer. A solution containing 20 g of phenol in 1.0 kg of benzene has its freezing point lowered by 0.69 K. Calculate the fraction of phenol that has dimerised. [Given Kf for benzene = 5.1 Km-1]
At 20 °C, the vapor pressure of benzene 1C6H62 is 75 torr, and that of toluene 1C7H82 is 22 torr. Assume that benzene and toluene form an ideal solution. (a) What is the composition in mole fraction of a solution that has a vapor pressure of 35 torr at 20 °C? (b) What is the mole fraction of benzene in the vapor above the solution described in part (a)?
The addition of 5.00 g of a compound to 250 g of naphthalene lowered the freezing point of the solvent by 0.780 K. Calculate the molar mass of the compound.
The addition of 100 g of compound A to 1 kg of benzene lowered the freezing point of the solvent by 2.56 K. Calculate the molar mass of compound A.
The molal freezing point depression constant =Kf·7.96°C·kgmol−1 for a certain substance X. When 5.40g of urea NH22CO are dissolved in 200.g of X, the solution freezes at −4.9°C. Calculate the freezing point of pure X. Round your answer to 2 significant digits.
The addition of 100 g of a compound to 750 g of CCl4 lowered the freezing point of the solvent by 10.5 K. Calculate the molar mass of the compound.
When 2.60 g of a substance that contains only indium andchlorine is dissolved in 50.0 g of tin(IV) chloride, the normal boiling point of the tin(IV) chloride is raised from 114.1°C to 116.3°C. If Kb = 9.43 K kg mol-1for SnCl4, what are the approximate molar mass and the probablemolecular formula of the solute?
(1a) Pure benzophenane freezes at 66.6 °C. A solution of 7.75 g of biphenyl (C12H10; molar mass = 154.2g/mol) plus 200.08 g of benzophenane froze at 59.9 °C. Calculate the Kf of benzophenane in °C*kg/mol. (b) An unknown solution with possible cations (Ag+, Hg22+, Pb2+) is treated with 6M HCl and a white precipitate forms. Hot water is added to the precipitate, and a white solid remains after filtration. The white solid is treated with aqueous NH3, and the precipitate turns grey or black. The resulting solution is treated with HNO3 and no precipitate forms. What cations can you determine to be present, absent or maybe present? Explain your reason
(a) State Raoult’s law for a solution containing volatile components. How does Raoult’s law become a special case of Henry’s law?(b) 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (Kyfor benzene = 5.12 K kg mol-1)