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Calculate 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.
Ch.13 - Solutions
Chapter 13, Problem 83
Calculate the osmotic pressure of a solution containing 24.6 g of glycerin (C3H8O3) in 250.0 mL of solution at 298 K.
Verified step by step guidance1
Calculate the molar mass of glycerin (C_3H_8O_3) by adding the atomic masses of its constituent atoms: 3 carbon atoms, 8 hydrogen atoms, and 3 oxygen atoms.
Convert the mass of glycerin (24.6 g) to moles using its molar mass.
Determine the molarity of the solution by dividing the number of moles of glycerin by the volume of the solution in liters (0.250 L).
Use the formula for osmotic pressure: \( \Pi = iMRT \), where \( i \) is the van't Hoff factor (which is 1 for glycerin, a non-electrolyte), \( M \) is the molarity, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin (298 K).
Substitute the values into the osmotic pressure formula to calculate \( \Pi \).
Related Practice
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Calculate 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.
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Calculate 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.
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What 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.)
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A 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?
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Calculate 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.