Which of the following aqueous solutions has the highest osmotic pressure at 25°C?Group of answer choices0.2 M Na2SO4 0.2 M ethanol0.2 M KBr0.2 M KCl
Question
Solution
The osmotic pressure of a solution is directly proportional to its molarity and temperature and also depends on the number of particles the solute forms in solution.
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Na2SO4 is a strong electrolyte and will dissociate completely in solution to form 3 particles: 2 Na+ ions and 1 SO4^2- ion.
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Ethanol is a non-electrolyte and will not dissociate in solution, so it forms only 1 particle.
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KBr is a strong electrolyte and will dissociate completely in solution to form 2 particles: 1 K+ ion and 1 Br- ion.
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KCl is also a strong electrolyte and will dissociate completely in solution to form 2 particles: 1 K+ ion and 1 Cl- ion.
Therefore, the 0.2 M Na2SO4 solution will have the highest osmotic pressure because it forms the most particles in solution.
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