Ionic Equilibria in Solutions

Michael Faraday classified substances into electrolytes and non-electrolytes based on their ability to conduct electricity in aqueous solutions. Electrolytes are further divided into strong and weak electrolytes. Strong electrolytes, like sodium chloride, fully ionize in water, while weak electrolytes, like acetic acid, only partially ionize. In weak electrolytes, an equilibrium is established between unionized molecules and ions, known as ionic equilibrium.

What are the two categories of substances classified by Michael Faraday based on their ability to conduct electricity?

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How do strong electrolytes differ from weak electrolytes in terms of ionization when dissolved in water?

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What is the composition of the aqueous solution of sodium chloride?

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What is the percentage of ionization for acetic acid compared to sodium chloride?

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Explain the concept of ionic equilibrium in the context of weak electrolytes.

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