Final answer:
Compounds such as KI, MgSO₄, NaOH, and possibly FeCl3 (assuming FeCl is an error) are strong electrolytes and would create conductive aqueous solutions due to their complete dissociation into ions. CH3OH, being a nonelectrolyte with no dissociation into ions, would not create a conductive solution. Water itself is not an electrolyte but provides the medium for other substances to dissolve and be conductive.
option c is the correct
Step-by-step explanation:
The question asks which compounds would be conductive when in an aqueous solution, and to classify these compounds as electrolytes or nonelectrolytes. An electrolyte is a substance that produces ions when dissolved in water, thus allowing the solution to conduct electricity. A nonelectrolyte does not dissociate into ions in solution and therefore, does not conduct electricity.
KI (potassium iodide), MgSO₄ (magnesium sulfate), and NaOH (sodium hydroxide) are all strong electrolytes which dissociate completely into ions in aqueous solutions. When these substances dissolve in water, they provide a conductive medium due to the movement of these ions within the solution. KI dissociates into K+ and I- ions, MgSO₄ into Mg2+ and SO42- ions, and NaOH into Na+ and OH- ions, thus making their aqueous solutions good conductors of electricity.
FeCl is likely a typographical error meant to represent a form of iron (III) chloride, possibly FeCl3. As a salt of a metal and a halogen, it would also be a strong electrolyte when dissolved in water, breaking up into Fe3+ and Cl- ions, leading to a conductive solution. The compound CH3OH (methanol), however, is a nonelectrolyte as it does not dissociate into ions in solution, and its aqueous solution would not conduct electricity.
H₂O (water) itself is not an electrolyte and does not become conductive unless ions are present. However, it is the medium in which other compounds dissolve to create a conductive solution. We already expect water to have minimal conductivity due to its autodissociation into H+ and OH- ions, but the presence of these ions is typically too low to result in significant conductivity.