Question:
Calculate \(\Delta T_b\) of a \(0.45\) m solution of a nonvolatile solute in solvent if molal elevation constant of solvent is \(3.0\) K kg mol\(^{-1}\)
Calculate \(\Delta T_b\) of a \(0.45\) m solution of a nonvolatile solute in solvent if molal elevation constant of solvent is \(3.0\) K kg mol\(^{-1}\)
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Delta Tb = Kb times m for a nonvolatile solute.
Updated On: Oct 1, 2026
- \(0.94\) K
- \(2.69\) K
- \(3.21\) K
- \(1.35\) K
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The Correct Option is D
Solution and Explanation
Step 1: Understanding the Concept:
Adding a nonvolatile solute raises the boiling point of the solvent. This is a colligative property, depending only on the number of solute particles.
Step 2: Key Formula:
\[ \Delta T_b = K_b \times m \]
Step 3: Detailed Explanation:
With \(K_b = 3.0\) K kg mol\(^{-1}\) and \(m = 0.45\) mol kg\(^{-1}\):
\[ \Delta T_b = 3.0 \times 0.45 = 1.35 \text{ K} \]
No van't Hoff factor is needed because the solute is not stated to ionise.
Step 4: Why the other options are wrong.
The values 0.94, 2.69 and 3.21 K do not equal the product of 3.0 and 0.45. For example 3.21 K would need a molality of 1.07.
Final Answer:
The elevation in boiling point is \(1.35\) K, option (D). \[ \boxed{1.35 \text{ K}} \]
Adding a nonvolatile solute raises the boiling point of the solvent. This is a colligative property, depending only on the number of solute particles.
Step 2: Key Formula:
\[ \Delta T_b = K_b \times m \]
Step 3: Detailed Explanation:
With \(K_b = 3.0\) K kg mol\(^{-1}\) and \(m = 0.45\) mol kg\(^{-1}\):
\[ \Delta T_b = 3.0 \times 0.45 = 1.35 \text{ K} \]
No van't Hoff factor is needed because the solute is not stated to ionise.
Step 4: Why the other options are wrong.
The values 0.94, 2.69 and 3.21 K do not equal the product of 3.0 and 0.45. For example 3.21 K would need a molality of 1.07.
Final Answer:
The elevation in boiling point is \(1.35\) K, option (D). \[ \boxed{1.35 \text{ K}} \]
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