1 / 6

Acid & Base Definitions

Acid & Base Definitions. Arrhenius Theory Acid -substance that contains hydrogen and produces H + in aqeous solution (soln.) any protonic acid is an Arrhenius acid: H 2 SO 4 , HCl, HNO 3 ....

aknepp
Télécharger la présentation

Acid & Base Definitions

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 Definitions • Arrhenius Theory • Acid-substance that contains hydrogen and produces H+ in aqeous solution (soln.) • any protonic acid is an Arrhenius acid: H2SO4, HCl, HNO3 .... • Base-substance that contains the hydroxyl (OH) group and produces hydroxide ions (OH-) in aqeous soln. • Metal hydroxides (hydroxyl bases) are Arrhenius bases • Neutralization: H+(aq) + OH-(aq) H2O(l) • HA(aq)+ OH-(aq) H2O(l) + A-(aq)

  2. Brønsted-Lowry Theory • Acids-Proton donor • Any hydrogen containing compound capable of releasing a proton: All acids that we have discussed so far. • Bases-Proton acceptor • Metal hydroxides, ammonia, ammonia derivatives and more. • Acid-Base Rxns: HA(aq) + B(aq) A-(aq) + BH+(aq) • acid base • HNO3 + H2O - + H3O+ • proton transfer • H2O + NH3 OH- + NH4+

  3. Lewis Theory • Acids - lone pair acceptor • any electron deficient compound: BF3 • Bases - lone pair donor • any compound with a lone pair for donation: NH3, CO, O2 , ... • Acid-Base rxn involves the formation of a coordinate covalent bond • Coordinate Covalent Bond

  4. Lewis Acid-Base Reaction

  5. Autoionization • H2O + H2O  H3O+ + OH- • acid base • What kind of acid is shown in the above reaction? Base? • Arrhenius, Brønsted-Lowry & Lewis Acid • Arrhenius, Brønsted-Lowry & Lewis Base

  6. Amphoterism • Amphoterism - the ability of a substance to act as an acid or a base. • A substance that exhibits amphoterism is said to be amphoteric • Water is amphoteric because it can act as an acid or a base. • Specifically, water is amphiprotic because it can either be a proton donar or acceptor (Brønsted-Lowery definition or an acid & base) • Many insoluble metal hydroxides are amphoteric: • Cu(OH)2(s) + 2H+(aq) Cu2+(aq)+ 2 H2O • base acid • Cu(OH)2(s)+2OH-(aq) Cu(OH)42-(aq) • acid base

More Related