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Boiling Point Elevation Formula:
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The boiling point elevation formula calculates the increase in boiling point of a solvent when a non-volatile solute is added. It's a colligative property that depends on the number of solute particles in the solution.
The calculator uses the boiling point elevation formula:
Where:
Explanation: The formula shows that boiling point elevation is directly proportional to the molality of the solution and the van't Hoff factor, which accounts for solute dissociation.
Details: Calculating boiling point elevation is important for determining molecular weights of solutes, understanding colligative properties, and various industrial applications including food processing and antifreeze formulations.
Tips: Enter the van't Hoff factor (i), ebullioscopic constant (K_b), and molality (m). All values must be positive numbers.
Q1: What is the van't Hoff factor?
A: The van't Hoff factor (i) represents the number of particles a solute dissociates into in solution. For non-electrolytes, i = 1; for electrolytes, it depends on the degree of dissociation.
Q2: What are typical values for K_b?
A: Common values include 0.512 °C kg/mol for water, 2.53 °C kg/mol for acetic acid, and 3.63 °C kg/mol for benzene. The constant is specific to each solvent.
Q3: Why use molality instead of molarity?
A: Molality is used because it's temperature-independent (based on mass), unlike molarity which is volume-based and changes with temperature.
Q4: Does boiling point elevation work for all solutions?
A: The formula applies to ideal solutions with non-volatile solutes. For concentrated solutions or volatile solutes, deviations may occur.
Q5: What are practical applications of boiling point elevation?
A: Applications include determining molecular weights, calculating solute concentrations, and designing industrial processes like distillation and antifreeze systems.