14:00Boiling point elevation and freezing point depression | Chemistry | Khan AcademyKhan Academy678views
25:23Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic PressureThe Organic Chemistry Tutor620views
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?1049views3rank1comments
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.3095views4rank
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.789views
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.418views
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.327views
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.434views
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?421views
Open QuestionCalculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform308views
Open QuestionAn ethylene glycol solution contains 21.2 g of ethylene glycol (C2H6O2) in 85.4 mL of water. Determine the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)
Open QuestionCalculate the freezing point and boiling point of a solution containing 10.0 g of naphthalene (C10H8) in 100.0 mL of benzene. Benzene has a density of 0.877 g/cm³.
Open QuestionCalculate the freezing point and boiling point of a solution containing 7.55 g of ethylene glycol (C2H6O2) in 85.7 mL of ethanol. Ethanol has a density of 0.789 g/cm³.
Open QuestionCalculate the molar mass of an unknown compound given that an aqueous solution containing 17.5 g of the compound in 100.0 g of water has a freezing point of -1.8 °C.
Open QuestionCalculate the molar mass of an unknown molecular (nonelectrolyte) compound in an aqueous solution containing 35.9 g of the compound in 150.0 g of water with a freezing point of -1.3 °C.
Open QuestionIs the question formulated correctly for calculating the freezing point and boiling point of each solution, assuming complete dissociation of the solute? For the following: a. 10.5 g FeCl3 in 1.50 * 10^2 g water b. 3.5% KCl by mass (in water) c. 0.150 m MgF2.
Open QuestionA 0.95 m aqueous solution of an ionic compound with the formula MX has a freezing point of -3.0 °C. Calculate the van’t Hoff factor (i) for MX at this concentration.
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