Question

We dissolve 345 g of calcium acetate in enough water to make 1.2 L of solution. What is the osmotic pressure of this solution at 54 ∘C? Express your answer in atm.Π

Answer 1

Answer:

$\Pi=146.3atm$

Explanation:

Hello.

In this case, since the osmotic pressure is computed via:

$\Pi =i*c*RT$

Whereas the van't Hoff's factor of calcium acetate (molar mass = 158.17 g/mol) is 3 as it dissociates in one calcium ion and two acetate ions, the concentration is:

$c=\frac{345g*\frac{1mol}{158.17g} }{1.2L}=1.82mol$

Therefore, the osmotic pressure is:

$\Pi =3*1.82mol*0.082\frac{atm*L}{mol*K}*(54+273.15)K\\\\\Pi=146.3atm$

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