Osmotic Pressure | Example #1

The video tutorial explains how to solve a problem involving osmotic pressure to find the molar mass of a solute, specifically hemoglobin. It begins with the basic formula for osmotic pressure and shows how to substitute moles with mass over molecular weight. The tutorial then sets up a problem involving hemoglobin, providing the necessary data and demonstrating how to rearrange the equation to solve for molar mass. It includes unit conversion and calculation steps, emphasizing the importance of using consistent units throughout the process.

What is the primary goal when given an osmotic pressure in a problem?

• To calculate the volume of the solution

• To determine the molar mass of the solute

• To find the temperature of the solution

• To measure the pressure in pascals

Which relationship is crucial for inter-converting between osmotic pressure and molecular weight?

• Volume is equal to mass times temperature

• Moles is equal to mass divided by molecular weight

• Pressure is equal to temperature divided by volume

• Molecular weight is equal to pressure times volume

In the osmotic pressure formula, what does the symbol 'n' represent?

• Molecular weight of the solute

• Temperature in Celsius

• Volume of the solution

• Number of moles of the solute

What is the osmotic pressure of the hemoglobin solution given in the example?

• 7.51 atm

• 7.51 torr

• 0.263 torr

• 10 milliliters

Why is it necessary to convert milliliters to liters in the calculation?

• Because the gas constant is in liters

• To simplify the calculation

• To match the units of temperature

• To convert grams to moles

What is the final unit of the calculated molar mass of hemoglobin?

• Grams per liter

• Moles per gram

• Grams per mole

• Liters per mole

What is the approximate molar mass of hemoglobin calculated in the example?

• 6.51 x 10^3 g/mol

• 0.263 g/mol

• 6.51 x 10^4 g/mol

• 7.51 x 10^4 g/mol