The osmotic pressure of seawater at 20∘c. = 3.12 atm
Further explanation
Osmotic pressure is the minimum pressure applied to the solution so that there is no osmotic transfer from a thinner solution to a more concentrated solution.
General formula:
[tex]\large {\boxed {\bold {\pi\: = \: M \: x \: R \: x \: T}}}[/tex]
π = osmosis pressure (atm)
M = concentration of solution (mol / l)
R = constant = 0.08205 L atm mol-1 K-1
T = Temperature (Kelvin)
The full question should be:
Seawater contains 3.8g of salts for every liter of solution.
Assuming that the solute consists entirely of NaCl (over 90% is), calculates the osmotic pressure of seawater at 20 degrees Celsius.
mole NaCl = 3.8 gram: 58.5 (molar mass of NaCl)
mole NaCl = 0.065
so the molarity = 0.065 M
For NaCl electrolyte solutions, the van't Hoff factor (i) is taken into account. And the value of i for strong electrolytes such as NaCl which has a degree of ionization = 1 then i = n = 2 (NaCl ionizes into 2 ions namely Na + and Cl-)
Temperature = 20° C+ 273 = 293 K
then
π = M. R. T. i
π = 0.065. 0.082. 293. 2
π = 3.12 atm
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Keywords: osmotic pressure, electrolyte solution
