When 1.0 mol of HF is dissolved in 1.0 kg of water, the boiling point of the resulting solution is 100.5 °C. Is HF a strong or weak electrolyte? Explain.

Verified step by step guidance

1. Determine the boiling point elevation (ΔT_b) by subtracting the boiling point of pure water (100.0 °C) from the boiling point of the solution (100.5 °C). This gives ΔT_b = 0.5 °C.
2. Use the boiling point elevation formula: $\Delta T\_b\; =\; i\; \times \; K\_b\; \times \; m$, where $i$ is the van 't Hoff factor, $K\_b$ is the boiling point elevation constant for water (0.512 °C·kg/mol), and $m$ is the molality of the solution.
3. Calculate the molality ($m$) of the solution using the formula . Here, the moles of HF are 1.0 mol, and the mass of water is 1.0 kg, so $m\; =\; 1.0\; \backslash ,\; ext\{mol/kg\}$.
4. Rearrange the boiling point elevation formula to solve for the van 't Hoff factor ($i$): . Substitute the known values: $\Delta T\_b\; =\; 0.5\; \backslash ,\; ext\{°C\}$, $K\_b\; =\; 0.512\; \backslash ,\; ext\{°C·kg/mol\}$, and $m\; =\; 1.0\; \backslash ,\; ext\{mol/kg\}$.
5. Interpret the value of $i$. If $i$ is close to 1, HF is a weak electrolyte because it does not fully dissociate in water. If $i$ is significantly greater than 1, HF is a strong electrolyte because it dissociates into ions completely.

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They can be classified as strong or weak based on their degree of ionization. Strong electrolytes completely dissociate into ions, while weak electrolytes only partially dissociate, resulting in fewer ions in solution.

Boiling Point Elevation

Boiling point elevation is a colligative property that describes how the boiling point of a solvent increases when a solute is added. The extent of this elevation depends on the number of solute particles in the solution. In this case, the increase in boiling point from 100 °C to 100.5 °C indicates that the solute (HF) contributes to the solution's overall particle concentration.

HF as an Electrolyte

Hydrofluoric acid (HF) is classified as a weak electrolyte because it only partially ionizes in solution. When HF dissolves in water, it produces a mixture of HF molecules and ions (H⁺ and F⁻), but not all HF molecules dissociate. The observed boiling point elevation suggests that HF does contribute to the solution's ionic strength, but its incomplete dissociation confirms its status as a weak electrolyte.