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stellarik [79]
3 years ago
7

Calculate the osmotic pressure (in torr) of 6.00 L of an aqueous 0.958 M solution at 30.°C, if the solute concerned is totally i

onized into three ions (e.g., it could be Na2SO4 or MgCl2).
Chemistry
1 answer:
cluponka [151]3 years ago
7 0

<u>Answer:</u> The osmotic pressure is 54307.94 Torr.

<u>Explanation:</u>

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

\pi=iCRT

where,

\pi = osmotic pressure of the solution = ?

i = Van't hoff factor = 3

C = concentration of solute = 0.958 M

R = Gas constant = 62.364\text{ L Torr }mol^{-1}K^{-1}

T = temperature of the solution = 30^oC=[30+273]K=303K

Putting values in above equation, we get:

\pi=3\times 0.958mol/L\times 62.364\text{ L. Torr }mol^{-1}K^{-1}\times 303K\\\\\pi=54307.94Torr

Hence, the osmotic pressure is 54307.94 Torr.

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