Intravenous, or IV, solutions used in medicine must exert the same osmotic pressure as blood to prevent a net flow of water into or out of the blood cells. The proper concentration for an intravenous NaCl solution is 0.90 g NaCl per 100. mL of solution (sometimes referred to as 0.90 % m/v). If the van't Hoff factor of NaCl is i = 1.8 , what is the osmotic pressure of blood at body temperature, 37 ∘ C?

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Tringa0 Tringa0 · Answer 1 · 2019-12-09T06:41:28+01:00

Answer:

The osmotic pressure of blood at 37°C is 7.04 atm.

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

[tex]\pi=icRT[/tex]

where:

[tex]\pi[/tex] = osmotic pressure of the solution

i = Van't hoff factor

c = concentration of solute

R = Gas constant = [tex]0.0820\text{ L atm }mol^{-1}K^{-1}[/tex]

T = temperature of the solution

We have:

Mass of NaCl = 0.90 g

Moles of NaCl =[tex]\frac{0.90 g}{58.5 g/mol}=0.01538 mol[/tex]

Volume of NaCl solution = V = 100.0 mL = 0.1 L

Concentration of NaCl solution = [tex]\frac{0.01538}{0.1 L}=0.1538 mol/L[/tex]

i = 1.8 , T = 37°C = 310.15 K

[tex]\pi =1.8\times 0.1538 mol/L\times 0.0820\text{ L.atm }mol^{-1}K^{-1}\times 310.15 K[/tex]

[tex]\pi =7.0407 atm\approx 7.04 atm[/tex]

The osmotic pressure of blood at 37°C is 7.04 atm.