1. ACIDS + BASES

3. ACIDS
Properties: (other than tasting sour and being corrosive) 1) React with metals 2) React with carbonates 3) Conduct electricity 4) Turn blue litmus paper red 5) Neutralize bases ACIDS ARE CORROSIVE

4. 1) ACIDS REACT WITH METALS
If you swallowed a penny, what would happen? (DON’T TRY THIS AT HOME!!!)
penny hydrochloric acid
penny HCl
penny acid

5. 1) ACIDS REACT WITH METALS
2HCl(aq) + Zn(s)  H2(g) + ZnCl2(aq)

6. 2) ACIDS REACT WITH CARBONATES
What happens when you put baking soda (sodium bicarbonate) into vinegar?
HC2H3O2(aq) + NaHCO3(aq)  CO2(g) + H2O(l) + NaC2H3O2(aq)

7. 3) ACIDS CONDUCT ELECTRICITY
Acids are made of ions, so in water these ions separate and can conduct electricity
Hydrogen ion is what makes an acid acidic
HCl(aq)  H+(aq) + Cl-(aq)

8. IONIZATION IN WATER H+
Cl- H+
Cl- H+
Cl-
Strong acids ionize completely in water, while weak acids only ionize slightly

9. NEGATIVELY-CHARGED ELECTRODE POSITIVELY-CHARGED ELECTRODE
IONIZATION IN WATER - + H+ H+
NEGATIVELY-CHARGED ELECTRODE
Cl-
POSITIVELY-CHARGED ELECTRODE
Cl- H+
Cl-
Cl- H+

10. 4) ACIDS TURN BLUE LITMUS PAPER RED
Blue litmus paper is an indicator and turns red when it touches acid

11. 5) ACIDS NEUTRALIZE BASES
Acids can neutralize bases, so adding an acid to a base can neutralize their caustic nature
HCl(aq) + NaOH(aq)  H2O(l) + NaCl(aq) Hydrochloric acid + sodium hydroxide  water + salt (sodium chloride)
Corrosive + caustic  non-corrosive + non-corrosive

12. BASES
Properties: (other than tasting bitter, feeling slippery) 1) Conduct electricity 2) Turn red litmus paper blue
3) Turns phenolphthalein pink 4) Neutralize acids BASES ARE CAUSTIC

13. 1) BASES CONDUCT ELECTRICITY
Bases are made of ions, so in water these ions separate and can conduct electricity
hydroxide ion makes bases basic
NaOH(aq)  Na+(aq) + OH-(aq)

14. 2) BASES TURN RED LITMUS PAPER BLUE
Red litmus paper is an indicator and turns blue when it touches base

15. 3) BASES TURN PHENOLPHTALEIN PINK
Phenolphtalein is colourless, and turns pink in bases (above pH 8.2) while remaining colourless in acids.

16. 4) BASES NEUTRALIZE ACIDS
Bases can neutralize acids, so adding a base to an acid can eliminate their corrosiveness Example: Antacids to neutralize stomach acid
2HCl(aq) + CaCO3(aq)  CaCl2(aq) + H2CO3(aq) H2CO3(aq)  H2O(l) + CO2(g)

17. HOW TO MAKE ACIDS + BASES
ACIDS: 1) Non-metal + oxygen  non-metal oxide 2) Non-metal oxide + water  ACID! EXAMPLE: N2 + 2O2  2NO2 NO2 + H2O  HNO3 BASES: 1) Metal + oxygen  Metal oxide 2) Metal oxide + water  BASE! EXAMPLE: 2Mg + O2  2MgO MgO + H2O  Mg(OH)2

18. ACID-BASE INDICATORS
Indicators change color depending on whether a substance is acidic or basic

19. Different indicators change colour at specific pH ranges
ACID-BASE INDICATORS
Different indicators change colour at specific pH ranges

20. The strength of an acid or base is measured with pH
power
hydrogen
pH = power of hydrogen

21. pH = -log [H+] pH Logarithm with base 10
Calculating pH
pH = -log [H+]
Logarithm with base 10
Concentration of hydrogen ions

22. At 25°C: From 0 to 14, with 7 being NEUTRAL
pH Scale
At 25°C: From 0 to 14, with 7 being NEUTRAL
pH < 7  acidic
pH = 7  neutral
pH > 7  basic

23. pH Scale

24. pH Scale Every pH level is 10x more concentrated than the level above.
i.e. pH 4 is 10x more concentrated than pH 5
pH 3 is 100x more concentrated than pH 5

25. Recall: Polyatomic ions have modified names in acids
ACID NAMING
Recall: Polyatomic ions have modified names in acids
Polyatomic ion name
Acid anion name
Example
sulfate
sulfuric
H2SO4 sulfuric acid
chlorate
chloric
HClO3 chloric acid
carbonate
carbonic
H2CO3 carbonic acid
phosphate
phosphoric
H3PO4 phosphoric acid

26. Recall: Most acids have hydrogen
ACID NAMING
Recall: Most acids have hydrogen
1) Naming:
HCl(aq)
H2SO4(aq)
Sulfuric acid
Hydrochloric acid
OXYACID
BINARY ACID

27. H BrO3 = HBrO3(aq) bromic acid ACID NAMING
2) Writing the chemical formula:
bromic acid 1 + 1 - H
BrO3
= HBrO3(aq)

28. ACID NAMING
Oxyacids with polyatomic ions that end in “ite” are given the ending “ous”
Polyatomic ion name
Acid anion name
Example
sulfite
sulfurous
H2SO3 sulfurous acid
chlorite
chlorous
HClO2 chlorous acid
carbonite
carbonous
H2CO2 carbonous acid
phosphite
phosphorous
H3PO3 phosphorous acid

29. ACID NAMING
1) Naming:
HNO2(aq)
nitrite
= nitrous acid

30. H BrO2 = HBrO2(aq) bromous acid ACID NAMING
2) Writing the chemical formula:
bromous acid 1 + 1 - H
BrO2
= HBrO2(aq)

31. HOMEWORK
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