Multiple Choice
Calculate the osmotic pressure of a solution containing 19.35 mg of hemoglobin in 14.5 mL of solution at 23 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Assume the solution behaves ideally. (R = 0.0821 L·atm/mol·K)
14. Solutions
Osmotic Pressure
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the osmotic pressure (in atm) of an aqueous solution that contains 162.1 g of glucose (C₆H₁₂O₆) in 1.50 L of solution at 295 K? (R = 0.0821 L·atm/mol·K, Molar mass of glucose = 180.18 g/mol)
A
3.67 atm
B
1.82 atm
C
0.98 atm
D
2.45 atm
Verified step by step guidance1
First, calculate the number of moles of glucose in the solution. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \). Here, the mass of glucose is 162.1 g and the molar mass is 180.18 g/mol.
Next, determine the molarity of the solution. Molarity (M) is defined as moles of solute per liter of solution. Use the formula: \( M = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \). The volume of the solution is 1.50 L.
Now, apply the formula for osmotic pressure: \( \Pi = MRT \), where \( \Pi \) is the osmotic pressure, \( M \) is the molarity, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin (295 K).
Substitute the values for molarity, R, and T into the osmotic pressure formula to find \( \Pi \).
Finally, ensure the units are consistent and check your calculations to verify the osmotic pressure value.
1:13mWatch next
Master Osmotic Pressure Formula with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Osmotic Pressure practice set
Problem sets built by lead tutorsExpert video explanations