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Acids and Bases Chapter 19.

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Presentation on theme: "Acids and Bases Chapter 19."— Presentation transcript:

1 Acids and Bases Chapter 19

2 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

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

4 Pure Water is Neutral

5 Arrhenius Acid Donates a H+ ion in an aqueous solution

6 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.

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

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

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

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

11 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

12 Phosphoric Acid is triprotic

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


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

16 Strong Base Weak Acid

17 What is pH?

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