Open Question
Is the question asking for the calculation of the van’t Hoff factor (i) for KBr at a given concentration, based on the provided osmotic pressure, correct?
14. Solutions
Osmotic Pressure
Multiple Choice
Calculate the osmotic pressure of a solution containing 19.45 mg of hemoglobin in 16.8 mL of solution at 18 °C. The molar mass of hemoglobin is 6.5×10^4 g/mol. Assume the solution behaves ideally and use R = 0.0821 L·atm/mol·K.
A
1.200 atm
B
0.0012 atm
C
0.012 atm
D
0.120 atm
Verified step by step guidance1
Convert the mass of hemoglobin from milligrams to grams by dividing by 1000. This is necessary because the molar mass is given in grams per mole.
Calculate the number of moles of hemoglobin using the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \).
Convert the volume of the solution from milliliters to liters by dividing by 1000, as the gas constant R is given in L·atm/mol·K.
Use the formula for osmotic pressure: \( \Pi = \frac{nRT}{V} \), where \( n \) is the number of moles, \( R \) is the gas constant, \( T \) is the temperature in Kelvin, and \( V \) is the volume in liters. First, convert the temperature from Celsius to Kelvin by adding 273.15.
Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the osmotic pressure formula to calculate \( \Pi \).
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