The relationship between acids and protons is central to the understanding of acid-base chemistry. Here are the accurate statements:
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Acids can donate protons (H⁺ ions): According to the Brønsted-Lowry theory, acids are defined as substances that can donate protons to bases during a reaction. For example, hydrochloric acid (HCl) can donate a proton to water, forming hydronium ions (H₃O⁺).
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Acids and bases: The distinction between acids and bases is often made in terms of their proton content during reactions. While acids donate protons, bases accept protons. This means that in any acid-base reaction, the acid will be the proton donor and the base will be the proton acceptor.
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Proton count in terms of strength: While it's not accurate to say that acids inherently contain more or fewer protons than bases, the ability to donate protons defines an acid. Some acids may contain multiple protons (like sulfuric acid, H₂SO₄), but the defining characteristic is their ability to release H⁺ ions in solution.
Hence, the correct assertion is: An acid can donate protons to a base when they react.