Which of the following aqueous solutions would have the greatest osmotic pressure?

Question

Quizplus · Accepted Answer

Osmotic pressure is directly proportional to the molar concentration of the solute particles in solution. Therefore, the solution with the highest molar concentration of solute particles will have the greatest osmotic pressure. 
Calculation of the number of solute particles:
A) Urea (CO(NH2)2) is a non-electrolyte, so it will not dissociate into ions. Therefore, the solution will have 1 mol of solute particles for every 1 mol of urea. 
B) NaCl will dissociate into Na+ and Cl- ions, so the solution will have 2 mol of solute particles for every 1 mol of NaCl. 
C) CaCl2 will dissociate into Ca2+ and 2Cl- ions, so the solution will have 3 mol of solute particles for every 1 mol of CaCl2. 
D) ScCl3 will dissociate into Sc3+ and 3Cl- ions, so the solution will have 4 mol of solute particles for every 1 mol of ScCl3. 
E) KCl will dissociate into K+ and Cl- ions, so the solution will have 2 mol of solute particles for every 1 mol of KCl. 
Therefore, the solution with the greatest osmotic pressure will be solution C, 0.030 M CaCl2, which has the highest number of solute particles in solution.

Which of the Following Aqueous Solutions Would Have the Greatest