1 / 8

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.

adli
Télécharger la présentation

Acid-Base Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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)

More Related