1 / 12

I. Introduction to Acids & Bases (p. 453 - 473)

Ch. 15 & 16 - Acids & Bases. I. Introduction to Acids & Bases (p. 453 - 473). electrolytes  electrolytes. A. Properties. ACIDS. BASES. bitter taste. sour taste. turn litmus red. turn litmus blue. react with metals to form H 2 gas. slippery feel.

aristotle-olson
Download Presentation

I. Introduction to Acids & Bases (p. 453 - 473)

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. Ch. 15 & 16 - Acids & Bases I. Introduction toAcids & Bases(p. 453 - 473)

  2. electrolytes electrolytes A. Properties ACIDS BASES • bitter taste • sour taste • turn litmus red • turn litmus blue • react with metals to form H2 gas • slippery feel • vinegar, milk, soda, apples, citrus fruits • ammonia, lye, antacid, baking soda ChemASAP

  3. H H – + O O Cl Cl H H H H B. Definitions • Arrhenius - In aqueous solution… • Acidsform hydronium ions (H3O+) HCl+ H2O  H3O+ + Cl– acid

  4. H H – + N O O N H H H H H H H H B. Definitions • Arrhenius - In aqueous solution… • Bases form hydroxide ions (OH-) NH3+ H2O  NH4+ + OH- base

  5. conjugate base conjugate acid B. Definitions • Brønsted-Lowry • Acidsare proton (H+) donors. • Bases are proton (H+) acceptors. HCl + H2O  Cl– + H3O+ acid base

  6. B. Definitions H2O + HNO3 H3O+ + NO3– B A CA CB

  7. B. Definitions NH3 + H2O  NH4+ + OH- B A CA CB • Amphoteric - can be an acid or a base.

  8. F - H2PO4- H2O HF H3PO4 H3O+ B. Definitions • Give the conjugate base for each of the following: • Polyprotic - an acid with more than one H+

  9. Br - HSO4- CO32- HBr H2SO4 HCO3- B. Definitions • Give the conjugate acid for each of the following:

  10. B. Definitions • Lewis • Acidsare electron pair acceptors. • Bases are electron pair donors. Lewis base Lewis acid

  11. - + C. Strength • Strong Acid/Base • 100% ionized in water • strong electrolyte HCl HNO3 H2SO4 HBr HI HClO4 NaOH KOH Ca(OH)2 Ba(OH)2

  12. - + C. Strength • Weak Acid/Base • does not ionize completely • weak electrolyte HF CH3COOH H3PO4 H2CO3 HCN NH3

More Related