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Ch.13 - Properties of Solutions
All textbooksBrown 14th EditionCh.13 - Properties of SolutionsProblem 77
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Chapter 13, Problem 77

What is the osmotic pressure formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water at 25 °C?

Verified step by step guidance
1
Step 1: Convert the mass of aspirin from milligrams to grams by dividing by 1000. This will make it easier to work with in subsequent calculations.
Step 2: Calculate the number of moles of aspirin using its molar mass. The molar mass of aspirin (C9H8O4) can be found by adding the atomic masses of all the atoms in the formula.
Step 3: Determine the molarity of the aspirin solution by dividing the number of moles of aspirin by the volume of the solution in liters.
Step 4: Use the formula for osmotic pressure, \( \Pi = iMRT \), where \( i \) is the van't Hoff factor (which is 1 for non-electrolytes like aspirin), \( M \) is the molarity, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin. Convert the temperature from Celsius to Kelvin by adding 273.15.
Step 5: Substitute the values for \( i \), \( M \), \( R \), and \( T \) into the osmotic pressure formula to find the osmotic pressure.
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