1 / 11

Bases

Acids. and. Bases. Definitions. Acids – produce H + Bases - produce OH - Acids – donate H + Bases – accept H +. Arrehenius. Bronsted-Lowry. Examples. Acids. HCl Lemon Juice Soda NaOH Bleach Soap. H 2 SO 4 Acid Rain Vinegar KOH Ammonia M.O.M. Bases. Properties of Acids.

leeljohnson
Download Presentation

Bases

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. Acids and Bases

  2. Definitions Acids – produce H+ Bases - produce OH- Acids – donate H+ Bases – accept H+ Arrehenius Bronsted-Lowry

  3. Examples Acids HCl Lemon Juice Soda NaOH Bleach Soap H2SO4 Acid Rain Vinegar KOH Ammonia M.O.M Bases

  4. Properties of Acids • pH < 7.0 • Taste Sour • React with metals • Turn litmus paper red

  5. Properties of Bases • pH > 7.0 • Taste Bitter • Slippery, soapy feeling • Turn litmus paper blue

  6. Acids & Bases • Conduct electricity (electrolytes) • React with indicators

  7. Universal Indicator Indicators Chemicals which change colors when they are put into acids or bases.

  8. Acid/Base Reactions (Neutralization Reactions) Acid +BaseWater + Ionic Compound HCl + KOH  HOH + KCl H2SO4 + 2KOH  2H2O + K2SO4

  9. pH Scale H+ OH- Acid Neutral Base 0 1 4 6 7 8 10 11 13 2 3 5 9 12 14 Urine Blood Saliva Bleach Ammonia Sea Water Pure Water Baking Soda Gastric Juice Tomato Juice Black Coffee Milk of Magnesia Battery Acid, HCl Orange Juice, Soda Lemon Juice, Vinegar Liquid Draino, NaOH

  10. What is pH? • measures the concentration of H+ ions (How acidic or basic a solution is) pH = -log[H+] If [H+] = 1 x 10-4, then pH = 4 If [H+] = 1 x 10-13, then pH = 13

  11. pH and pOH pH + pOH = 14 If [OH-] = 10-8 M, what is the pH? • the pOH = 8 • so the pH must be 14 – 8 • So the pH = 6

More Related