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Acid-Base Reactions

Acid-Base Reactions. Bronsted-Lowry theory. An acid is a substance from which a proton (H + ion) can be removed A base is a substance that can remove a proton (H + ion) from an acid An acid-base reaction involves the transfer of a proton. Conjugate acid-base pair.

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Acid-Base Reactions

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  1. Acid-Base Reactions

  2. Bronsted-Lowry theory • An acid is a substance from which a proton (H+ ion) can be removed • A base is a substance that can remove a proton (H+ ion) from an acid • An acid-base reaction involves the transfer of a proton

  3. Conjugate acid-base pair Two molecules or ions that are related by the transfer of a proton (H+) are called a conjugate acid-base pair. (conjugate means “linked”)

  4. Example:HBr(aq) + H20(l) -> H30+(aq) + Br-(aq) Conjugate base of an acid is the particle that remains when a proton is removed from the acid (in this example: Br-(aq) Conjugate acidof a base is the particle that results when the base receives the proton from the acid (in this example: H30+(aq)

  5. Ammonia is a pungent gas at room temperature. Its main use is in the production of fertilizers and explosives. It is very soluble in water. It forms a basic solution that is used in common products such as glass cleaners. Identify the conjugate acid-base pairs in the reaction between aqueous ammonia and water. NH3(g) + H2O(l)  NH4+(aq) + OH-(aq) Step 1: Identify the proton provider on the left side of the equation as the acid. Identify the proton receiver as the base. H2O(l) is the acid, NH3(g) is the base. Step 2: Identify the conjugate acid and base on the right side of the equation by the difference of a single proton from the acid and base on the left side. OH-(aq) is the conjugate base NH4+(aq) is the conjugate acid

  6. Arrhenius Acid Any substance that dissociates to form H+ in aqueous solution Base Any substance that dissociates to form 0H- in aqueous solution Bronsted-Lowry Acid Any substance that provides a proton to another substance Base Any substance that receives a proton from an acid Comparing the Arrhenius Theory and the Bronsted-Lowry Theory

  7. Neutralization Reactions • Reaction between an acid and a base produces an ionic compound (a salt) and water acid + base -> a salt + water Examples: HCl (aq) + NaOH(aq) -> H20(l) + NaCl(aq) H2CO3(aq) + 2KOH(aq) -> 2H20(l) + K2CO3(aq)

  8. 2. Reaction between an acid and a carbonate produces an ionic compound, water and carbon dioxide Acid + carbonate -> carbon dioxide + water + ionic salt Examples: 2HCl(aq) + Na2CO3(aq) -> CO2(g) + H20(l) + 2NaCl(aq) HBr(aq) + KHCO3 (aq) -> CO2(g) + H20(l) + KBr(aq)

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