Acids and Bases Chapter 19.

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Presentation transcript:

Acids and Bases Chapter 19

Characteristics of Acids Sour tasting – vinegar, lemons React with metals and produce H2 (g) React with metal carbonates to produce CO2 Blue Litmus Paper  Red Conductive H+ ions > OH- ions pH < 7

Characteristics of Bases Bitter tasting (soap) Slippery Red Litmus Paper  Blue Conductive OH- ions > H+ ions pH > 7

Pure Water is Neutral

Arrhenius Acid Donates a H+ ion in an aqueous solution

Model doesn’t explain why ammonia is a base. Arrhenius Base Donates a OH- in an aqueous solution Model doesn’t explain why ammonia is a base.

Bronsted-Lowry Model Acid – donates a H+ Base –accepts a H+

Forms when the base accepts a H+ ion Forms when the acid donates a H+ ion to a base

Conjugate Acid? Conjugate Base? Which is the acid? Base? Conjugate Acid? Conjugate Base?

Bronsted-Lowry Expands the range of acids and bases. Amphoteric – acts as an acid and a base (water)

Monoprotic and Polyprotic Acids Mono – donates only one H+ HCl, HNO3, CH3COOH Not covalently bonded, ionizable Poly – donates more than one H+ Diprotic – H2SO4 Triprotic – H3PO4

Phosphoric Acid is triprotic

Acid Strength Strong acids completely ionize Weak acids do not completely ionize

Base Strength Strong Bases dissociate into metal ions and hydroxide ions Weak base partially ionizes in dilute aqueous solutions

Strong Base Weak Acid

What is pH?