25:23Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic PressureThe Organic Chemistry Tutor620views
Multiple ChoiceThe osmotic pressure of blood is 5950.8 mmHg at 41°C. What mass of glucose, C6H12O6, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.1039views4rank
Multiple ChoiceDetermine the osmotic pressure at 22.5 °C of a 2.5 L aqueous solution that contains 50.0 g of sucrose (molar mass = 342.3).358views
Open QuestionA 150.0 mL sample of an aqueous solution at 25°C contains 15.2 mg of an unknown nonelectrolyte compound. if the solution has an osmotic pressure of 8.44 torr, what is the molar mass of the unknown compound?437views1rank
Open QuestionIntravenous, or IV, solutions used in medicine must exert the same osmotic pressure as blood to prevent a net flow of water into or out of the blood cells. the proper concentration for an intravenous NaCl solution is 0.90 g NaCl per 100. ml of solution (sometimes referred to as 0.90% m/v). If the van't hoff factor of NaCl is 𝑖=1.8, what is the osmotic pressure of blood at body temperature, 37∘C?418views
Open QuestionWhat is the osmotic pressure of a 0.850 M solution of glucose in water at 35 °C?303views
Multiple ChoiceThe osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25ºC. What is the molar mass of insulin? (1 atm = 760 torr)91views
Open QuestionCalculate the osmotic pressure of a solution containing 24.6 g of glycerin (C3H8O3) in 250.0 mL of solution at 298 K.
Open QuestionWhat mass of sucrose (C12H22O11) would you combine with 5.00 * 10^2 g of water to make a solution with an osmotic pressure of 8.55 atm at 298 K? (Assume a density of 1.0 g/mL for the solution.)
Open QuestionA solution containing 27.55 mg of an unknown protein per 25.0 mL was found to have an osmotic pressure of 3.22 torr at 25 °C. What is the molar mass of the protein?
Open QuestionCalculate the osmotic pressure of a solution containing 18.75 mg of hemoglobin in 15.0 mL of solution at 25 °C. The molar mass of hemoglobin is 6.5 x 10^4 g/mol.
Open QuestionUsing the van’t Hoff factors in Table 13.9, calculate the mass of solute required to make each aqueous solution: a. a sodium chloride solution containing 1.50 * 10^2 g of water that has a melting point of -1.0 °C; b. 2.50 * 10^2 mL of a magnesium sulfate solution that has an osmotic pressure of 3.82 atm at 298 K; c. an iron(III) chloride solution containing 2.50 * 10^2 g of water that has a boiling point of 102 °C.
Open QuestionIs the question asking for the calculation of the van’t Hoff factor (i) for KBr at a given concentration, based on the provided osmotic pressure, correct?
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