the osmotic pressure of blood at 37 degrees is 7.56atm. what mass of glucose should be dissolved per litre of solution for an intravenous injection to be isotonic with blood?
See your other two posts.
To determine the mass of glucose required to make an intravenous injection isotonic with blood, we need to use the concept of osmotic pressure and the ideal gas law.
The osmotic pressure of a solution is related to the concentration of solute particles in the solution. In this case, glucose is the solute.
First, let's calculate the molar concentration of the solution (C) using the ideal gas law:
PV = nRT
Where:
P = osmotic pressure (7.56 atm)
V = volume of the solution (1 L)
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature in Kelvin (37°C + 273.15 = 310.15 K)
n = number of moles of solute we want to calculate
Rearranging the equation:
n = PV / RT
n = (7.56 atm * 1 L) / (0.0821 L·atm/(mol·K) * 310.15 K)
Now, we need to convert moles to mass using the molar mass of glucose.
The molar mass of glucose (C6H12O6) is:
C: 12.01 g/mol
H: 1.008 g/mol (x 12 atoms = 12.096 g/mol)
O: 16.00 g/mol (x 6 atoms = 96.00 g/mol)
Total molar mass of glucose: 12.01 g/mol + 12.096 g/mol + 96.00 g/mol = 180.106 g/mol
Finally, we can calculate the mass of glucose dissolved per liter of solution:
Mass = n (moles) * molar mass
Mass = (7.56 atm * 1 L) / (0.0821 L·atm/(mol·K) * 310.15 K) * 180.106 g/mol
Simplifying and rounding the result to an appropriate number of significant figures will give you the mass of glucose needed per liter of solution to make it isotonic with blood.