While preparing a 0.5 molal solution, more solvent mass was taken by mistake. What happens to the actual molality?
Answer and explanation
Correct answer: Actual molality becomes lower
Molality is m = nsolute / mass of solvent in kilograms. If the solute amount remains fixed but more solvent is used, the denominator increases, so the calculated molality decreases below the intended 0.5 m. This differs from molarity because molality depends on solvent mass rather than final solution volume.
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What is the correct answer to this question?
Actual molality becomes lower
Why is this the correct answer?
Molality is m = nsolute / mass of solvent in kilograms. If the solute amount remains fixed but more solvent is used, the denominator increases, so the calculated molality decreases below the intended 0.5 m. This differs from molarity because molality depends on solvent mass rather than final solution volume.
Which subject and chapter does this question cover?
This is a Class 11 Chemistry question. Chapter: Chapter 01: Solutions.
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