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!!!)
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
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
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
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”