QuestionJune 22, 2025

Which of these is a possible boiling point for a 1.0 M solution of sugar in water?The normal boiling point of water is 100^circ C -0.3^circ C 100.3^circ C 99.7^circ C

Which of these is a possible boiling point for a 1.0 M solution of sugar in water?The normal boiling point of water is 100^circ C -0.3^circ C 100.3^circ C 99.7^circ C
Which of these is a possible boiling point for a 1.0 M solution of sugar in water?The normal boiling point of water is 100^circ C -0.3^circ C 100.3^circ C 99.7^circ C

Solution
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Answer

100.3^{\circ}C is a possible boiling point, as it rounds down from 100.512^{\circ}C. Explanation 1. Determine Boiling Point Elevation Formula The boiling point elevation is calculated using \Delta T_b = i \cdot K_b \cdot m, where i is the van't Hoff factor (1 for sugar), K_b is the ebullioscopic constant of water (0.512^{\circ}C/m), and m is molality (1.0 M). 2. Calculate Boiling Point Elevation \Delta T_b = 1 \cdot 0.512^{\circ}C/m \cdot 1.0\, m = 0.512^{\circ}C 3. Determine New Boiling Point Add the boiling point elevation to the normal boiling point: 100^{\circ}C + 0.512^{\circ}C = 100.512^{\circ}C

Explanation

1. Determine Boiling Point Elevation Formula<br /> The boiling point elevation is calculated using $\Delta T_b = i \cdot K_b \cdot m$, where $i$ is the van't Hoff factor (1 for sugar), $K_b$ is the ebullioscopic constant of water ($0.512^{\circ}C/m$), and $m$ is molality (1.0 M).<br /><br />2. Calculate Boiling Point Elevation<br /> $\Delta T_b = 1 \cdot 0.512^{\circ}C/m \cdot 1.0\, m = 0.512^{\circ}C$<br /><br />3. Determine New Boiling Point<br /> Add the boiling point elevation to the normal boiling point: $100^{\circ}C + 0.512^{\circ}C = 100.512^{\circ}C$
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