This document provides information about acids and bases. It discusses the key properties of acids, including that they react with metals, carbonates, conduct electricity, turn litmus paper red, and neutralize bases. Properties of bases are also outlined, such as conducting electricity, turning litmus paper blue, and neutralizing acids. The document explains how acids and bases are formed, how pH is measured, and how to name acids based on their polyatomic ions.

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!!!)

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
HCl(aq)  H+
(aq) + Cl-
(aq)
Hydrogen ion is what
makes an acid acidic

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

9. NEGATIVELY-CHARGEDELECTRODE
POSITIVELY-CHARGEDELECTRODE
IONIZATION IN WATER
H+
Cl-
H+Cl-
H+
Cl-
H+
Cl-
- +

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. BASESProperties: (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
NaOH(aq)  Na+
(aq) + OH-
(aq)
hydroxide ion makes
bases basic

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:
Mg + O2  MgO
MgO + H2O  Mg(OH)2

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

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

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

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

22. 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. ACID NAMING
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
Recall: Polyatomic ions have modified names in acids

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

27. bromic acid
BrO3H
1 1+ -
= HBrO3(aq)
2) Writing the chemical formula:
ACID NAMING

28. ACID NAMING
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
Oxyacids with polyatomic ions that end in “ite” are
given the ending “ous”

29. H2NO2(aq)
1) Naming:
ACID NAMING
nitrite
= nitrous acid

30. bromous acid
BrO2H
1 1+ -
= HBrO2(aq)
2) Writing the chemical formula:
ACID NAMING

31. HOMEWORK
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