A 1.2 m aqueous solution of an ionic compound with the formula MX₂ has a boiling point of 101.4 °C. Calculate the van't Hoff factor (i) for MX₂ at this concentration.

검증된 단계별 안내

insert step 1> Determine the boiling point elevation (ΔT_b) using the formula: ΔT_b = T_b(solution) - T_b(pure solvent). Here, T_b(solution) is 101.4 °C and T_b(pure solvent) for water is 100.0 °C.

insert step 2> Use the boiling point elevation formula: ΔT_b = i * K_b * m, where i is the van't Hoff factor, K_b is the ebullioscopic constant for water (0.512 °C kg/mol), and m is the molality of the solution (1.2 m).

insert step 3> Rearrange the formula to solve for the van't Hoff factor (i): i = ΔT_b / (K_b * m).

insert step 4> Substitute the known values into the equation: i = (101.4 °C - 100.0 °C) / (0.512 °C kg/mol * 1.2 m).

insert step 5> Calculate the value of i to determine the van't Hoff factor for the ionic compound MX2.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

도움이 되었나요?

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Colligative Properties

Colligative properties are physical properties of solutions that depend on the number of solute particles in a given amount of solvent, rather than the identity of the solute. These properties include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure. In this context, the boiling point elevation of the solution is used to determine the van't Hoff factor.

Boiling Point Elevation

Boiling point elevation is a colligative property that describes how the boiling point of a solvent increases when a solute is dissolved in it. The change in boiling point can be calculated using the formula ΔT_b = i * K_b * m, where ΔT_b is the boiling point elevation, i is the van't Hoff factor, K_b is the ebullioscopic constant of the solvent, and m is the molality of the solution. This concept is crucial for solving the given problem.

van't Hoff Factor (i)

The van't Hoff factor (i) represents the number of particles into which a solute dissociates in solution. For ionic compounds, this factor is typically greater than one, as they dissociate into multiple ions. For the compound MX2, which dissociates into one M ion and two X ions, the expected van't Hoff factor would be 3. Calculating i involves using the observed boiling point elevation to find the effective number of particles in solution.

A 1.2 m aqueous solution of an ionic compound with the formula MX2 has a boiling point of 101.4 °C. Calculate the van't Hoff factor (i) for MX2 at this concentration.