Explanation 1. Concept: Boiling point elevation is a colligative property, so it does not depend on the identity of the solute particles. It only depends on their number of solute particles present. As the number of solute particles increases, the boiling point of solution also increases. We are given three aqueous solutions of different substance and their concentration. Each solvent has its own sensitivity to the presence of solute particles among its own molecules, so each solvent has its own boiling point elevation constant K b . This constant is used to relate boiling point elevation Δ T b to the concentration of solute particles expressed in molality or i × m where I is van’t Hoff factor of the solute in a solution in which its molal concentration is m. Δ T b = K b × i × m Δ T b = T b ( s o l u t i o n ) - T b ( p u r e s o l v e n t ) Where ∆ T b is the elevation in boiling point, defined as the boiling point of solution minus the boiling point of pure solvent; K b is the boiling point elevation constant, which depends only on the solvent; i is the van’t Hoff factor, which takes into account the number of particles produced by a compound when dissolved in solution; m is the molality of the solution; T b s o l u t i o n is the boiling point of solution; T b ( p u r e s o l v e n t ) is the boiling point of pure solvent. In the question, we are given three ionic compounds with different concentration values. Each of the compounds will dissociate and form different amount of number of particles as follows: NH 4 NO 3 , will produce two particles (i = 2) when dissolved in water as follows: N H 4 N O 3 a q → N H 4 + a q + N O 3 - a q LiCl will produce two particles (i = 2) when dissolved in water as follows: L i C l a q → L i + a q + C l - ( a q ) Cu(NO 3 ) 2 will produce three particles (i = 3) when dissolved in water as follows: C u N O 3 2 a q → C u 2 + a q + 2 N O 3 - 1 ( a q ) For different ionic compounds, find the product ( i × m ) . The higher the product, higher is the boiling point of that solution. 2. Formula: The formula, which we will use for calculating the boiling point of each solution, is Δ T b = K b × i × m K b of water is 0.52 0 C m o l since we are using water as the solvent for each solution. A mole is the SI unit of amount chemical substance. When writing units, it is written as “mol”. 3. Calculation: a) Boiling point of 0.0400 m N H 4 N O 3 s o l u t i o n , i × m = 2 × 0.0400 = 0.08 Δ T b = K b × i × m Δ T b = 0.52 0 C m o l × 2 × 0.0400 = 0.0416 ℃ Δ T b = T b ( s o l u t i o n ) - T b ( p u r e s o l v e n t ) 0

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Chapter 11, Problem 11.53QA

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We need to find the highest boiling point of given three aqueous solutions.

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