Boiling Point Elevation in Solutions溶液中沸点升高
The boiling point of pure water is 100°C, but that boiling point can be elevated by the adding of a solute such as a salt. A solution typically has a measurably higher boiling point than the pure solvent. 纯水的沸点是100°C，但加入溶质如盐后，沸点会升高。通常来说，溶液的沸点比纯溶剂高得多。
A treatment of boiling point elevation is given by Ebbing. The boiling point elevation ΔTb is a colligative property of the solution, and for dilute solutions is found to be proportional to the molal concentration cm of the solution: Ebbing 对沸点升高进行了论述。溶液的沸点升高 ΔT_b 是一种依存性质，对于稀溶液，发现它与溶液的molal浓度 c_m 成正比：
ΔTb = Kbcm Where Kb is called the boiling-point-elevation constant. 其中Kb称为沸点升高常数。
Solutions may be produced for the purpose of raising the boiling point and lowering the freezing point, as in the use of ethylene glycol in automobile cooling systems. The ethylene glycol (antifreeze) protects against freezing by lowering the freezing point and permits a higher operating temperature by raising the boiling point. 溶液可以被制备以升高沸点和降低冰点，例如在汽车冷却系统中使用乙二醇。乙二醇（防冻剂）通过降低冰点来防止冻结，并通过升高沸点允许更高的工作温度。
|
Index Chemistry concepts Reference Ebbing Sec. 12.6 化学概念索引 参考 Ebbing 第12章第6节 | ||
|
Go Back
返回 |