Calculate the osmotic pressure of a solution containing 18.30 mg of hemoglobin in 15.1 ml of solution at 26 ∘c . the molar mass of hemoglobin is 6.5×104 g/mol

Chemistry
1

calculate the osmotic pressure of a solution containing 18.30 mg of hemoglobin in 15.1 ml of solution at 26 ∘c . the molar mass of hemoglobin is 6.5×104 g/mol .

2

To calculate the osmotic pressure of a solution, we need to use the formula:

Osmotic pressure (π) = (n/V)RT

Where:
n = number of moles of solute
V = volume of the solution in liters
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin

First, let’s calculate the number of moles of hemoglobin in the solution.

Given:
Mass of hemoglobin = 18.30 mg
Molar mass of hemoglobin = 6.5×104 g/mol

Step 1: Convert mass to grams
18.30 mg = 0.0183 g

Step 2: Convert grams to moles
Number of moles of hemoglobin = (0.0183 g) / (6.5×104 g/mol)

Now, let’s calculate the osmotic pressure.

Step 3: Convert volume to liters
Volume of solution = 15.1 ml = 0.0151 L

Step 4: Convert temperature to Kelvin
Temperature = 26 °C + 273.15 = 299.15 K

Now we have all the values to calculate the osmotic pressure.

Osmotic pressure (π) = (n/V)RT

Substituting the values:
Osmotic pressure (π) = [(0.0183 g) / (6.5×104 g/mol)] * (0.0821 L·atm/(mol·K)) * (299.15 K) / (0.0151 L)

Calculating this expression will give us the osmotic pressure of the solution.