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Consider the separate solution of 0.500 M C2H5OH (aq), 0.100 M Mg3(P04)2(aq), 0.250 M KBr (aq) and 0.125 M Na3P04(aq) at 25° C. Which statement is true about these solutions, assuming all salts to be strong electrolytes?
(JEE Main 2014)
  • a)
    They all have same osmotic pressure
  • b)
    0.100 M Mg3(P04)2 (aq) has the highest osmotic pressure
  • c)
    0.125 M Na3P04(aq) has the highest osmotic pressure
  • d)
    0.5000 M C2H5OH (aq) has the highest osmotic pressure
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Consider the separate solution of 0.500 M C2H5OH (aq), 0.100 M Mg3(P04...
 (a)
Salts have been assumed as stronge lectrolytes, van’t Hoff factor,
/ = [1 + (y - 1)x]
y = number of ions from one mole of salt,
x = degree of ionisation = 1
C2H5OH is a non-electrolyte hence, y = 1
Thus, π ∝ Mi.RT being constant. Greater the value of Mi, greater the osmotic pressure.
Thus, π ∝ Mi, have equal values.
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Most Upvoted Answer
Consider the separate solution of 0.500 M C2H5OH (aq), 0.100 M Mg3(P04...
Introduction:
Osmotic pressure is a colligative property that depends on the concentration of solute particles in a solution. In this question, we are given four separate solutions: 0.500 M C2H5OH (aq), 0.100 M Mg3(P04)2(aq), 0.250 M KBr (aq), and 0.125 M Na3P04(aq). We need to determine which statement is true about these solutions in terms of their osmotic pressure.

Explanation:
To compare the osmotic pressures of these solutions, we need to consider the concentration of solute particles in each solution. The osmotic pressure of a solution is directly proportional to the concentration of solute particles. Therefore, the solution with the highest concentration of solute particles will have the highest osmotic pressure.

Calculating the concentration of solute particles:
To determine the concentration of solute particles in each solution, we need to consider the dissociation of each compound into its constituent ions.

1. C2H5OH (aq):
Ethanol (C2H5OH) does not dissociate into ions in water. Therefore, the concentration of solute particles in this solution is equal to the concentration of the ethanol molecules, which is 0.500 M.

2. Mg3(P04)2(aq):
Mg3(P04)2 dissociates into three Mg2+ ions and two PO4^3- ions.
Therefore, the concentration of solute particles in this solution is 3 * 0.100 M + 2 * 0.100 M = 0.300 M + 0.200 M = 0.500 M.

3. KBr (aq):
KBr dissociates into one K+ ion and one Br- ion.
Therefore, the concentration of solute particles in this solution is 0.250 M + 0.250 M = 0.500 M.

4. Na3P04(aq):
Na3P04 dissociates into three Na+ ions and one PO4^3- ion.
Therefore, the concentration of solute particles in this solution is 3 * 0.125 M + 0.125 M = 0.375 M + 0.125 M = 0.500 M.

Conclusion:
From the above calculations, we can see that all the solutions have the same concentration of solute particles, which is 0.500 M. Therefore, all the solutions have the same osmotic pressure. Hence, the correct statement is option 'A': They all have the same osmotic pressure.
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Consider the separate solution of 0.500 M C2H5OH (aq), 0.100 M Mg3(P04)2(aq), 0.250 M KBr (aq) and 0.125 M Na3P04(aq) at 25 C. Which statement is true about these solutions, assuming all salts to be strong electrolytes?(JEE Main 2014)a)They all have same osmotic pressureb)0.100 M Mg3(P04)2 (aq) has the highest osmotic pressurec)0.125 M Na3P04(aq) has the highest osmotic pressured)0.5000 M C2H5OH (aq) has the highest osmotic pressureCorrect answer is option 'A'. Can you explain this answer?
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