객관식
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)
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14. Solutions
Osmotic Pressure
객관식
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
검증된 단계별 안내1
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.
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