Let's examine the options: A) HCl (Hydrochloric acid): A strong acid. Dissolves in water to form H⁺ and Cl⁻ ions, conducting electricity. Forms an acidic solution (high concentration of H⁺). B) CH₃COOH (Acetic acid): A weak acid. Partially dissociates in water to form H⁺ and CH₃COO⁻ ions, conducting electricity weakly. Forms an acidic solution. C) CH₃OH (Methanol): An alcohol. Does not ionize in water. Does not conduct electricity. Forms a neutral solution. D) NaOH (Sodium hydroxide): A strong base. Dissolves in water to form Na⁺ and OH⁻ ions, conducting electricity well. Forms a basic solution (high concentration of OH⁻). Only NaOH satisfies both conditions: conducting electricity (due to ion formation) and forming a basic solution (due to OH⁻ production).
Which compound, when dissolved in water, conducts electricity and forms a basic solution ?
Asked in UPSC NDA 2 2017 · Topic: Acid, Base and Salt (Physical and Chemical Properties of Bases)
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