Question:
Which of 0.1 M urea and 0.1 M NaCl will have more osmotic pressure? Explain with reason.
Which of 0.1 M urea and 0.1 M NaCl will have more osmotic pressure? Explain with reason.
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Electrolytes give higher colligative properties due to dissociation (\(i>1\)).
Updated On: Oct 7, 2025
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Solution and Explanation
Step 1: Recall osmotic pressure formula.
\[ \pi = i C R T \] where \(i\) = van’t Hoff factor.
Step 2: For urea.
Urea is non-electrolyte → \(i=1\).
Step 3: For NaCl.
NaCl dissociates completely → \(i=2\). So effective concentration doubles.
Step 4: Conclusion.
Osmotic pressure of NaCl solution is higher than that of urea.
\[ \pi = i C R T \] where \(i\) = van’t Hoff factor.
Step 2: For urea.
Urea is non-electrolyte → \(i=1\).
Step 3: For NaCl.
NaCl dissociates completely → \(i=2\). So effective concentration doubles.
Step 4: Conclusion.
Osmotic pressure of NaCl solution is higher than that of urea.
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