When 4.54 g of a nonelectrolyte solute is dissolved in 565 mL of water at 29 °C, the resulting solution exerts an osmotic pressure of 835 torr.
What is the molar concentration of the solution?
How many moles of solute are in the solution?
What is the molar mass of the solute?
pi = MRT
Use pi in atm and T in kelvin. R is 0.08206. Solve for M = molarity.
mols = M x L = ?
Then n = grams/molar mass. You know mols and grams, solve for molar mass.
To determine the molar concentration of the solution, you can use the formula:
Molar Concentration (M) = Moles of Solute / Volume of Solution (in liters)
To find the moles of solute in the solution, you can use the formula:
Moles of Solute = (Osmotic Pressure * Volume of Solution) / (0.0821 * Temperature in Kelvin)
To find the molar mass of the solute, you can use the formula:
Molar Mass (g/mol) = Mass of Solute (g) / Moles of Solute
Now, let's go through the calculations step by step:
Step 1: Convert the volume of the solution to liters.
565 mL = 565 / 1000 = 0.565 L
Step 2: Convert the temperature from Celsius to Kelvin.
Temperature in Kelvin = 29 + 273 = 302 K
Step 3: Calculate the moles of solute.
Moles of Solute = (Osmotic Pressure * Volume of Solution) / (0.0821 * Temperature in Kelvin)
Moles of Solute = (835 torr * 0.565 L) / (0.0821 * 302 K)
Step 4: Calculate the molar concentration of the solution.
Molar Concentration (M) = Moles of Solute / Volume of Solution (in liters)
Molar Concentration = Moles of Solute / 0.565 L
Step 5: Calculate the molar mass of the solute.
Molar Mass (g/mol) = Mass of Solute (g) / Moles of Solute
Molar Mass = 4.54 g / Moles of Solute
Now, plug in the values into the respective formulas and perform the calculations to find the molar concentration, moles of solute, and molar mass of the solute.