1 / 22

Sections 16.1-2 Acids and Bases and pH

Sections 16.1-2 Acids and Bases and pH. Bill Vining SUNY Oneonta. Equilibrium systems. Acid base Precipitation Complexation Simultaneous Equilibria. Acid-Base Equilibria pH and pOH Relationship of Conjugate Pair acid-base strength. When acids or bases control pH: determine K

nelly
Download Presentation

Sections 16.1-2 Acids and Bases and pH

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. Sections 16.1-2Acids and Bases and pH Bill Vining SUNY Oneonta

  2. Equilibrium systems Acid base Precipitation Complexation Simultaneous Equilibria

  3. Acid-Base Equilibria • pH and pOH • Relationship of Conjugate Pair acid-base strength. • When acids or bases control pH: • determine K • predict pH • When pH controls acid/base state: • predict acid/base state • use acid/base state to determine pH • Buffer action • pH titration curves

  4. Bronsted Acids and Bases Bronsted Acid: H+ (proton) donor Bronsted Base: H+ acceptor Acid-Base reactions: H+ transfer reaction Conjugate Acid-Base Pairs: acid conjugate base HF F- NH4+ NH3

  5. What is the conjugate base of HNO2? • H2NO2+ • HNO3 • NO2-

  6. What is the conjugate acid of HPO42-? • H2PO4- • H3PO4 • PO43-

  7. What is the conjugate base of HPO42-? • H2PO4- • H3PO4 • PO43- What is the conjugate acid of HPO42-? • H2PO4- • H3PO4 • PO43-

  8. pH/pOHRelationships and Calculations [H3O+][OH-] = 1.0 x 10-14 pH = -log[H3O+] pOH= -log[OH-] [H3O+] = 10-pH [OH-] = 10-pH pH + pOH = 14.00

  9. Neutral, Acidicand Basic Solutions Neutral Acidic Basic

  10. What is [H3O+] when [OH-] = 5.4 x 10-3 M?

  11. What is the pH of a solution with [H3O+] = 4.6 x 10-5 M?

  12. What is [H3O+] in a solution with pH = 8.24?

  13. What is the pOH of a solution with [OH-] = 3.3 x 10-4 M?

  14. What is the pH of a solution with [OH-] = 2.4 x 10-3 M?

  15. Strong acids and bases For strong acid solutions, [H3O+] = [acid] (except for H2SO4) For strong bases LiOH, NaOH, KOH, RbOH, [OH-] = [base] For strong bases Ca(OH)2, Ba(OH)2, etc., [OH-] = 2 x [base]

  16. What is the pH of a 0.150 M solution of HCl?

  17. What is the pH of a 0.150 M solution of Ca(OH)2?

More Related