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# Acid & Bases ## The Arrhenius Theory of Acids and Bases * An acid is a substance that dissociates in water to produce hydrogen ions $H^{+}$. * $HBr(aq) \to H^{+}(aq) + Br^{-}(aq)$ * A base is a substance that dissociates in water to form hydroxide ions, $OH^{-}$. * $LiOH(aq) \to Li^{+}(aq) + OH^...

# Acid & Bases ## The Arrhenius Theory of Acids and Bases * An acid is a substance that dissociates in water to produce hydrogen ions $H^{+}$. * $HBr(aq) \to H^{+}(aq) + Br^{-}(aq)$ * A base is a substance that dissociates in water to form hydroxide ions, $OH^{-}$. * $LiOH(aq) \to Li^{+}(aq) + OH^{-}(aq)$ ## Limitations of the Arrhenius Theory: * $H^{+}$ are always hydrated, so a hydrated proton is called hydronium $H_{3}O^{+}$. * Ammonia does not contain hydroxide ions BUT, it does produce them when reacted with water. ## The Brønsted-Lowry Theory * An acid is a proton donor: ($H^{+}$ ion) can be removed. * A base is a proton acceptor – accepts a proton ($H^{+}$ ion). * Theory Requirements: One substance provides a proton, and another substance receives the proton. ## Conjugate Acid-Base Pair * Two molecules that are related by the transfer of a proton are called a conjugate acid-base pair.