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Question
Which of the following 0.1 M aqueous solutions will exert the highest osmotic pressure?
Options
Al2(SO4)3
Na2SO4
MgCl2
KCl
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Solution
Al2(SO4)3
Explanation:
Osmotic pressure depends on the number of solute particles in a solution. When Al2(SO4)3 dissolves, it dissociates into two aluminum ions (Al3+) and three sulfate ions \[\ce{(SO^2-_4)}\], resulting in a total of five ions per molecule, giving it the highest number of particles compared to the other options:
\[\ce{Al2SO4 -> 2Al3+ + 3SO^2-_4}\] (5 particles)
\[\ce{Na2SO4 -> 2Na+ + SO^2-_4}\] (3 particles)
\[\ce{MgCl2 -> Mg^2+ + 2Cl-}\] (3 particles)
\[\ce{KCl -> K + Cl-}\] (2 particles)
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