**Osmotic Pressure and Molar Concentration Calculation** When 3.49 g of a nonelectrolyte solute is dissolved in water to make 755 mL of solution at 27 °C, the solution exerts an osmotic pressure of 879 torr. **Questions:** 1. **What is the molar concentration of the solution?** - **Concentration:** ___________ M 2. **How many moles of solute are in the solution?** - **Moles of solute:** ___________ mol 3. **What is the molar mass of the solute?** - **Molar mass:** ___________ g/mol **Instructions:** - Use the ideal gas law equation for osmotic pressure: \(\Pi = iMRT\), where: - \(\Pi\) = osmotic pressure (in atms, convert torr to atm) - \(i\) = van't Hoff factor (for nonelectrolytes, \(i = 1\)) - \(M\) = molarity (moles/L) - \(R\) = ideal gas constant (\(0.0821 \, \text{L atm/mol K}\)) - \(T\) = temperature in Kelvin - Convert the temperature from Celsius to Kelvin. - Calculate the molar concentration from the given osmotic pressure. - Calculate the number of moles of solute using the molarity and volume. - Determine the molar mass using the mass of the solute and the number of moles calculated.

Osmotic Pressure and Molar Concentration Calculation When 3.49 g of a nonelectrolyte solute is dissolved in water to make 755 mL of solution at 27 °C, the solution exerts an osmotic pressure of 879 torr. Questions: 1. What is the molar concentration of the solution? - Concentration: _____ M 2. How many moles of solute are in the solution? - Moles of solute: _ mol 3. What is the molar mass of the solute? - Molar mass: _______ g/mol Instructions: - Use the ideal gas law equation for osmotic pressure: \(\Pi = iMRT\), where: - \(\Pi\) = osmotic pressure (in atms, convert torr to atm) - \(i\) = van't Hoff factor (for nonelectrolytes, \(i = 1\)) - \(M\) = molarity (moles/L) - \(R\) = ideal gas constant (\(0.0821 \, \text{L atm/mol K}\)) - \(T\) = temperature in Kelvin - Convert the temperature from Celsius to Kelvin. - Calculate the molar concentration from the given osmotic pressure. - Calculate the number of moles of solute using the molarity and volume. - Determine the molar mass using the mass of the solute and the number of moles calculated.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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