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Calculate the osmotic pressure of a solution containing 18.95 mg of hemoglobin in 16.6 mL of solution at 18 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Express your answer in atmospheres.
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14. Solutions
Osmotic Pressure
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What is the osmotic pressure of a solution containing 14 g of urea (H₂NCONH₂) in 300 mL of water at 217°C? (R = 0.0821 L·atm/mol·K)
A
20.7 atm
B
15.8 atm
C
12.5 atm
D
18.3 atm
Guida verificata passo dopo passo1
First, calculate the number of moles of urea (H₂NCONH₂) using its molar mass. The molar mass of urea is approximately 60.06 g/mol. Use the formula: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
Next, convert the volume of the solution from milliliters to liters, as osmotic pressure calculations require the volume in liters. Use the conversion: \( 300 \text{ mL} = 0.300 \text{ L} \).
Use the formula for osmotic pressure: \( \Pi = \frac{nRT}{V} \), where \( n \) is the number of moles, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), \( T \) is the temperature in Kelvin, and \( V \) is the volume in liters. First, convert the temperature from Celsius to Kelvin using \( T(K) = T(°C) + 273.15 \).
Substitute the values into the osmotic pressure formula: \( \Pi = \frac{n \times R \times T}{V} \). Ensure all units are consistent: moles for \( n \), L for \( V \), atm for \( R \), and K for \( T \).
Finally, solve the equation to find the osmotic pressure. This will give you the pressure in atmospheres (atm).
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