Question

Which of the following compounds would be conductive when in an aqueous solution?

A. FeCl₃
B. H₂O
C. NaOH
D. CH₃OH
E. MgSO₄
F. KI

Answer 1

Ionic compounds like FeCl₃, NaOH, MgSO₄, and KI will conduct electricity when dissolved in water because they dissociate into ions. H₂O and CH₃OH are nonelectrolytes and will not conduct electricity in their aqueous solutions.

Step-by-step explanation:

Conductivity of compounds in aqueous solutions depends on the presence of ions that can move freely and carry an electric current. Among the given compounds, substances that will conduct electricity when dissolved in water are:

1. FeCl₃ (iron(III) chloride) - Dissociates into Fe³⁺ and Cl⁻ ions, both of which are conductive.
2. NaOH (sodium hydroxide) - Dissociates into Na⁺ and OH⁻ ions, both of which are conductive.
3. MgSO₄ (magnesium sulfate) - Dissociates into Mg²⁺ and SO₄²⁻ ions, both of which are conductive.
4. KI (potassium iodide) - Dissociates into K⁺ and I⁻ ions, both of which are conductive.

• Meanwhile, H₂O (water) and CH₃OH (methanol) do not dissociate into ions that can conduct electricity when dissolved in water and are considered nonelectrolytes.

In summary, ionic compounds and strong acids/bases in water solution tend to be conductive due to the ions they produce. Covalent compounds like methanol do not typically produce ions, hence they are not conductive when dissolved.