Which of the following compounds conducts electricity when dissolved in water?

• A. NaCl
• B. CCl_4
• C. C_6H_{12}O_6 (glucose)
• D. CH_3OH (methanol)

Answer: (A)

Verified step by step guidance

1. Understand that electrical conductivity in aqueous solutions depends on the presence of ions that can move freely and carry charge.
2. Identify which compounds are ionic and which are molecular: NaCl is an ionic compound, while CCl_4, C_6H_{12}O_6 (glucose), and CH_3OH (methanol) are molecular compounds.
3. Recall that ionic compounds like NaCl dissociate into ions (Na^+ and Cl^-) when dissolved in water, allowing the solution to conduct electricity.
4. Recognize that molecular compounds such as CCl_4, glucose, and methanol do not dissociate into ions in water; they dissolve as neutral molecules and therefore do not conduct electricity.
5. Conclude that among the given options, only NaCl conducts electricity in aqueous solution due to its ionic nature and dissociation into ions.