Calculate the osmotic pressure (in torr) of a solution containing 17.15 mg of hemoglobin (molar mass 6.5 x 104 g/mol) in 12.8 mL of solution at 25 degrees C.

pi = MRT

M = moles/L.
moles = g/molar mass
Use AR = 0.08206
pi will come out in atm, convert to torr.

To calculate the osmotic pressure, we can use the equation:

Π = n/VRT

where:
Π is the osmotic pressure,
n is the number of moles of solute,
V is the volume of the solution,
R is the ideal gas constant (0.08206 L·atm/(mol·K)),
T is the temperature in Kelvin.

First, let's convert the given quantities to the required units:

Mass of hemoglobin = 17.15 mg
Molar mass of hemoglobin = 6.5 x 10^4 g/mol
Volume of solution = 12.8 mL
Temperature = 25 degrees C = 298 K

Step 1: Convert mass to moles
To calculate the number of moles (n) of hemoglobin, we use the formula:

n = mass / molar mass

n = 17.15 mg / (6.5 x 10^4 g/mol)

n = 0.000264 moles

Step 2: Convert volume to liters
To calculate the volume (V) in liters, we divide the given volume by 1000:

V = 12.8 mL / 1000

V = 0.0128 L

Step 3: Calculate the osmotic pressure
Now we can substitute the values into the osmotic pressure equation:

Π = (0.000264 moles) / (0.0128 L) * (0.08206 L·atm/(mol·K)) * (298 K)

Π ≈ 52.76 atm

To convert this to torr, we use the conversion factor:

1 atm = 760 torr

Π ≈ 52.76 atm * 760 torr/atm

Π ≈ 40086.56 torr

Therefore, the osmotic pressure of the solution is approximately 40086.56 torr.

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

π = MRT

Where:
π is the osmotic pressure
M is the molarity of the solution (moles of solute per liter of solution)
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature in Kelvin

First, we need to find the molarity of the hemoglobin solution. To do this, we need to determine the number of moles of hemoglobin present in the solution.

Step 1: Calculate the number of moles of hemoglobin:
Number of moles = Mass of hemoglobin / Molar mass of hemoglobin

Mass of hemoglobin = 17.15 mg = 0.01715 g
Molar mass of hemoglobin = 6.5 x 10^4 g/mol

Number of moles = 0.01715 g / (6.5 x 10^4 g/mol) = 2.638 x 10^(-7) mol

Step 2: Calculate the molarity of the solution:
Molarity = Number of moles / Volume of solution

Volume of solution = 12.8 mL = 0.0128 L

Molarity = (2.638 x 10^(-7) mol) / (0.0128 L) = 2.057 x 10^(-5) M

Now, we have the molarity of the hemoglobin solution (M = 2.057 x 10^(-5) M).

Step 3: Convert the temperature to Kelvin:
25 degrees Celsius = 25 + 273.15 = 298.15 K

Now we have the values for M, R, and T, so we can calculate the osmotic pressure (π).

π = (2.057 x 10^(-5) M) x (0.0821 L·atm/mol·K) x (298.15 K)

Calculating the value on a calculator, we get:

π = 0.504 atm

To convert the osmotic pressure to torr, we multiply by the conversion factor:

1 atm = 760 torr

π(torr) = 0.504 atm x 760 torr/atm

π(torr) = 383.04 torr

Therefore, the osmotic pressure of the hemoglobin solution is approximately 383.04 torr.

Calculate the osmotic pressure of a solution containing 16.50 mg of hemoglobin in 13.9 mL of solution at 29 ∘C . The molar mass of hemoglobin is 6.5×104 g/mol.