1. Acids, Bases and Salts

2. All three types of compounds dissociate in water (form ions)
All three are electrolytes
Conduct electricity as aqueous solutions

3. pH Scale 1 7 14 Acid Neutral Base pH = -log[H+]
Acid Neutral Base
High H+ conc Low H+ conc
Low OH- conc High OH- conc
pH scale measures the hydronium ion (H3O+)
Concentration [H3O+]
pH = -log[H+]

4. Acids and Bases

5. Arrhenius theory
Acid- a substance that produces only H+ ions when dissociated in water
Base- a substance that ionizes to produce OH- ions in solution

6. Example
Acid HCl  H+ (aq) + Cl- (aq)
Base NaOH  Na+ (aq) + OH- (aq)

7. Bronsted-Lowry Theories
Acid- in a chemical reaction, any substance that donates a proton
Base- in a chemical reaction, any substance that accepts a proton

8. Examples:
HCl(g) + H2O(l)  H3O+ (aq) + Cl- (aq)
HCl(g) + NH3 (g)  NH Cl-

9. Water is amphoteric
Has the ability to act as either an acid or a base
Water H2O  H3O+ + OH-
The H+ ion is never found free due to the strong attraction to a water molecules oxygen’s non bonded e- pairs, so is found as the hydronium ion H3O+

10. Describe an acid –base reaction as follows:
Acid + Base  conjugate base conjugate acid
(particle that remains (particle that remains
after a proton is that accepts the
released by an acid) proton released by acid)
Acid HCl H2O  H3O Cl-
Acid base conjugate acid conjugate base
Base NH3 + H2O  NH OH-
Base acid conjugate acid conjugate base

11. Lewis Theories
Acid- any substance that can accept an electron pair(electron-pair receptor)
Base- any substance that can donate an electron pair (electron-pair donor)
Applies to reactions that may not include H or H+ ions

12. Acidic anhydride- nonmetallic oxide
Acids and bases form naturally in nature by the reactions of anhydrides with water
Acidic anhydride- nonmetallic oxide
CO2 + H2O  H2CO3 carbonic acid in soda
SO2 + H2O  H2SO3 sulfurous acid rain
Base anhydride- metal oxide
Na2O + H2O  2NaOH

13. Properties of Acids
Are electrolytes
Neutralize bases
React with active metals to produce H2 gas
Change color of indicators
Taste sour

14. Properties of Bases
Are electrolytes
Neutralize acids
Change color of indicators
Are slippery to the touch
Taste bitter

15. Properties of Salts
Ionic compounds containing a pos.ion other than H+ and a neg.ion other than OH-
Products of a neutralization reaction
Product of reaction between metallic and nonmetallic oxide
Can be formed from single and double displacement reactions or direct combinations of elements

16. Indicator
Any substance that changes color in the presence of an acid or a base
Acids and bases change the colors of indicators
Phenolthalene, litmus paper(red and blue), pH paper(pools), red cabbage juice

17. Titration
Process where a known volume of a known concentration of an acid or base is added to a known volume of the opposite to find its concentration
Equivalence point
Point where the concentrations of H+ and OH- ions are equal(pH=7)
Determined by pH meter or indicator color change
MAVA =MBVB
M= molarity V= volume A= acid B= base