14:00Boiling point elevation and freezing point depression | Chemistry | Khan AcademyKhan Academy526views
25:23Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic PressureThe Organic Chemistry Tutor431views
Multiple ChoiceHow many moles of ethylene glycol, C2H6O2, must be added to 1,000 g of water to form a solution that has a freezing point of –10ºC?960views3rank1comments
Multiple ChoiceAn ethylene glycol solution contains 28.3 g of ethylene glycol, C2H6O2 in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.2966views4rank
Multiple ChoiceWhen 825 g of an unknown is dissolved in 3.45 L of water, the freezing point of the solution is decreased by 2.89°C. Assuming that the unknown compound is a non-electrolyte, calculate its molar mass.730views
Multiple ChoiceCalculate the mass of KCl used to prepare a solution in 3.00 L of water with a freezing point of –1.20 °C. Assume that the density of water = 1.00 g/mL.318views
Textbook QuestionHow many kilograms of ethylene glycol (automobile anti- freeze, C2H6O2) dissolved in 3.55 kg of water are needed to lower the freezing point of water in an automobile radiator to - 22.0 °C? The molal freezing point depression constant for water is Kf = 1.86 1°C kg2>mol. (LO 13.13) (a) 0.865 kg (b) 0.0420 kg (c) 9.01 kg (d) 2.61 kg431views
Textbook QuestionUsing data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 0.240 mol of naphthalene 1C10H82 in 2.45 mol of chloroform, g glucose 1C6H12O62 in 188 g of water.1122views
Textbook QuestionUsing data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 20.0 g of decane, C10H22, in 50.0 g CHCl3;1571views
Textbook QuestionWhat is the freezing point of an aqueous solution that boils at 105.0 °C?2066views2rank
Textbook QuestionA glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing point and boiling point of the solution.3170views
Textbook QuestionLauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 °C. What is the molar mass of lauryl alcohol from this data?2255views
Textbook QuestionCalculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. c. 5.5% NaNO3 by mass (in water)2326views
Textbook QuestionCalculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. b. 21.5 g of CuCl2 in 4.50 * 102 g water1425views
Textbook QuestionWhat mass of salt (NaCl) should you add to 1.00 L of water in an ice cream maker to make a solution that freezes at -10.0 °C? Assume complete dissociation of the NaCl and density of 1.00 g>mL for water.2750views
Textbook QuestionUse the van't Hoff factors in Table 13.9 to calculate each colligative property: a. the melting point of a 0.100 m iron(III) chloride solution1643views1rank
Textbook QuestionWhen 9.12 g of HCl was dissolved in 190 g of water, the freezing point of the solution was - 4.65 °C. What is the value of the van't Hoff factor for HCl?646views
Textbook QuestionA small cube of lithium 1density = 0.535 g/cm32 measuring 1.0 mm on each edge is added to 0.500 L of water. The following reaction occurs: 2 Li1s2 + 2 H2O1l2 ¡ 2 LiOH1aq2 + H21g2 What is the freezing point of the resulting solution, assuming that the reaction goes to completion?435views
Textbook QuestionWhen HNO2 is dissolved in water, it partially dissociates according to the equation HNO2ΔH+ + NO2- . A solution is prepared that contains 7.050 g of HNO2 in 1.000 kg of water. Its freezing point is -0.2929 °C. Calculate the fraction of HNO2 that has dissociated.2974views
Textbook QuestionA solution prepared by dissolving 3.00 g of ascorbic acid (vitamin C, C6H8O6) in 50.0 g of acetic acid has a freez- ing point that is depressed by ΔT = 1.33 °C below that ofpure acetic acid. What is the value of the molal freezing- point-depression constant for acetic acid?451views
Textbook QuestionA solution contains 10.05 g of unknown compound dissolved in 50.0 mL of water. (Assume a density of 1.00 g>mL for water.) The freezing point of the solution is -3.16 °C. The mass percent composition of the compound is 60.97% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?1433views
Textbook Question124. A 50.0-mL solution is initially 1.55% MgCl2 by mass and has a density of 1.05 g>mL. What is the freezing point of the solution after you add an additional 1.35 g MgCl2? (Use i = 2.5 for MgCl2.)687views
Textbook QuestionThe van't Hoff factor for CaCl2 is 2.71. What is its mass % in an aqueous solution that has Tf = - 1.14 °C?3379views1rank
Textbook QuestionElemental analysis of b@carotene, a dietary source of vitamin A, shows that it contains 10.51% H and 89.49% C. Dissolving 0.0250 g of b@carotene in 1.50 g of camphor gives a freezing- point depression of 1.17 °C. What are the molecular weight and formula of b@carotene? [Kf for camphor is 37.7 1°C kg2>mol.]540views
Textbook QuestionTreatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (e) What are the formula and molecular weight of MClx?287views
Textbook QuestionTreatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (c) What is the molality of particles (ions) in the solution of MClx?322views
Textbook QuestionTreatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (f) What is the identity of the metal M?408views
Textbook QuestionA solution prepared by dissolving 100.0 g of a mixture of sugar 1C12H22O112 and table salt (NaCl) in 500.0 g of water has a freezing point of - 2.25 °C. What is the mass of each individual solute? Assume that NaCl is completely dissociated.967views
Open QuestionDetermine the freezing point depression of a solution that contains 30.7 g glycerin (C3H8O3, molar mass = 92.09 g/mol) in 376 ml of water. Some possibly useful constants for water are kf = 1.86°C/m and kb = 0.512°C/m.230views
Open QuestionDetermine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 ml of benzene (d = 0.877 g/ml). pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C/m.311views
Open QuestionWhat mass of glucose (C6H12O6) should be dissolved in 12.0 kg of water to obtain a solution with a freezing point of -5.8∘C?301views
Open QuestionCalculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform208views