1 / 12

Chapter 16: Equilibrium in Acid-Base Systems

Chapter 16: Equilibrium in Acid-Base Systems. 16.2a: Bronsted-Lowry Acid-Base Concept. Definition of Acid and Base. Bronsted-Lowry independently created by two scientists around the same time (1923) looked at how acid/base acted in reactions instead of their properties in aqueous solutions

tierra
Download Presentation

Chapter 16: Equilibrium in Acid-Base Systems

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. Chapter 16: Equilibrium in Acid-Base Systems 16.2a: Bronsted-Lowry Acid-Base Concept

  2. Definition of Acid and Base Bronsted-Lowry independently created by two scientists around the same time (1923) looked at how acid/base acted in reactions instead of their properties in aqueous solutions theoretical definitions based upon proton transfer during a reaction

  3. Proton transfer concept • Acid: molecule or ion that is a proton (H+) donor • HCl + H2O  H3O+ + Cl- • Base: molecule or ion that is a proton (H+) acceptor • NH3 + H2O  NH4+ + OH-

  4. Bronsted-Lowry concept • B-L acid a proton donor; B-L base a proton acceptor • B-L neutralization is a competition for protons from the SA to the SB • B-L rxtn. eqtn. is an eqtn. that shows this transfer of protons from one entity to another

  5. Acids or Bases? C5H5N base (weak) Mg(OH)2 base (strong) HF acid (weak) NH3 base (weak) H2CO3 acid (weak) H2SO4 acid (strong) KOH base (strong) CH3NH2 base (weak) HC2H3O2 acid (weak) HI acid (strong)

  6. Acid – Base Reactions Identify the acids and bases of the following reactions C6H5NH2 + H2O  C6H5NH3+ + OH- B A HNO3 + H2O  H3O+ + NO3- A B HCH3COO + H2O  H3O+ + CH3COO- A B

  7. Acid-Base Reactions Amphoteric Substances proper term used in B-L reactions a substance that can react as either acid or base depending on what they are mixed with example: water, HSO4- Amphiprotic incorrect term to use with B-L rxtns. refers to an entity (ion or molecule)

  8. Amphoteric Water Water as a base (proton acceptor) Water as an acid (proton donor)

  9. Conjugate Acid-Base PairsConjugate acids and bases are always created by a B-L reaction (as products) Conjugate base an acid that has lost a H+ missing a hydrogen ex: H2PO4-, OH-, Cl- Conjugate acid a base that has gained a H+ has an extra hydrogen NH4+, C6H5NH3+, H3O+ A pair of substances with formulas that differ only by a proton is called a conjugate acid-base pair

  10. Identify the parts of these reactions C6H5NH2 + H2O  C6H5NH3+ + OH- base acid CA CB HNO3 + H2O  H3O+ + NO3- acid base CA CB HCH3COO + H2O  H3O+ + CH3COO- acid base CA CB NH3 + H2O  NH4+ + OH- base acid CA CB

  11. Homework • Textbook p724 #1-6 • Textbook p726 #7 • LSM 16.2A summary 1

More Related