**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.

When 3.61 g of a nonelectrolyte solute is dissolved in water to make 375 mL of solution at 29 °C, the solution exerts an osmotic pressure of 821 torr. What is the molar concentration of the solution? concentration: How many moles of solute are in the solution? moles of solute: What is the molar mass of the solute? molar mass: M mol g/mol

Calculate the molality of a solution formed by adding 2.60 g NHCl to 19.1 g of water. molality: m NH₂Cl

A student dissolves 6.7 g of biphenyl (C12H10) in 425. mL of a solvent with a density of 1.05 g/mL. The student notices that the volume of the solvent does not change when the biphenyl dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits. molarity Ox10 olo Ar molality 미