* Boiling Point Elevation: The boiling point of a solution is higher than the boiling point of the pure solvent (in this case, water). This phenomenon is called boiling point elevation and is a colligative property, meaning it depends only on the number of solute particles present, not their identity.
* Dissociation: Both KOH and KCl are strong electrolytes, meaning they fully dissociate into ions when dissolved in water.
* KOH → K⁺ + OH⁻
* KCl → K⁺ + Cl⁻
* Van't Hoff Factor (i): The van't Hoff factor represents the number of ions a solute dissociates into. Both KOH and KCl have a van't Hoff factor of 2 because they produce two ions each.
* The Key Difference: While both have the same molality and van't Hoff factor, KOH produces hydroxide ions (OH⁻), which are stronger bases than chloride ions (Cl⁻). The stronger interaction between hydroxide ions and water molecules leads to a greater elevation of the boiling point compared to the weaker interaction between chloride ions and water.
In summary: Even though both solutions have the same molality and van't Hoff factor, the stronger interaction of hydroxide ions with water molecules in the KOH solution results in a higher boiling point compared to the KCl solution.
