1. Acids and Bases
Chapter 23

2. Common Acids and Name Formula Strong/Weak Where is it found?
Hydrochloric acid
HCl
Strong
The stomach, in the lab.
Sulphuric acid
H2SO4
Acid rain, car batteries, the lab.
Nitric acid
HNO3
Acid rain, in the lab.
Ethanoic (acetic) acid
CH3COOH
Weak
Vinegar
Methanoic (formic) acid
HCOOH
Ant & nettle stings, descalers
Citric Acid
C6H8O7
Citrus fruits

3. Acids Acids are H+ or proton donors: Properties
Acids taste sour (e.g. vinegar, lemon juice).
Acids are harmful to living cells.
Aqueous solutions of all acids contain hydrogen ions, H+.

4. Water is needed

5. Common Bases Name Formula Where is it found?
Sodium hydroxide (caustic soda)
NaOH
Oven cleaners, in the lab.
Calcium hydroxide
Ca(OH)2
Soil lime, limewater
Magnesium oxide (magnesia)
MgO
Indigestion tablets
Calcium carbonate
CaCO3
Limestone, soil lime
Sodium hydrogencarbonate (bicarbonate)
NaHCO3
Baking powder
Ammonia
NH3
Cleaning fluids, in the lab.

6. Base properties
Most bases are oxides, hydroxides or carbonates of metals
Soluble bases are known as alkalis.
Aqueous solutions of alkalis contain hydroxide ions, OH-.
Bases taste bitter. .
Bases feel slippery

7. Base and indicators
Bases turn red litmus blue.  A common indicator, used to detect the presence of a base, is phenolphthalein which, when mixed with a base, turns pink.
Bases release hydroxide ions in water solutions. 
NaOH (s)  +  H2O (l)   à   Na1+ (aq)   +   OH1- (aq)
NH4OH  (aq)  ß -> NH41+ (aq)  +  OH1-  (aq)   

8. pH scale Water is defined as having a pH value of 7- neutral.
Acidic solutions have pH values below 7.
Alkaline (basic) solutions have pH values above 7.
pH is a measure of the number of hydronium or hydroxide ions
Logrithimic scale

9. pH scale

10. Reactions of Acids With metals
 Metals above copper in the reactivity series will react with acids, giving off hydrogen gas. The metal dissolves, forming a salt. 
 METAL + ACID ® SALT + HYDROGEN
ex. Mg(s) + H2SO4(aq) ® MgSO4(aq) + H2(g)
This is why acids corrode metals, and must be stored in glass containers.

11. Base reactions With bases (metal oxides and hydroxides)
 The base dissolves in the acid and neutralises it. A salt is formed.
ACID + BASE ® SALT + WATER
ex.       H2SO4(aq) + CuO(s) ® CuSO4(aq) + H2O(l)
With metal carbonates
 Metal + Base Salt + water + CO2
2HCl(aq) + CaCO3(s) ® CaCl2(s) + H2O(l) + CO2(g)

12. Indicators
Indicators- an organic compound that turns color in the presence of an acid or base

13. Naming Acids Prefix is always hydro
Name the second element with the suffix -ic
HCl – hydrochloric
HF- Hydrofluoric

14. For the acid containing the most common polyatomic ion of its group simply use the first part of the polyatomic name and follow with the suffix ic.
For the acid containing the polyatomic with one less oxygen than the ic, use the suffix ous.
For the acid containing the polyatomic with two less oxygens than the ic, use the prefix hypo and the suffix ous.
For an acid containing the polyatomic with one more oxygen than the ic, use the prefix per and the suffix ic.

15. Naming Bases and Salts
Follow regular naming rules

16. Acid Reactions ACID + BASE  SALT WATER Hydrochloric Acid
Sodium Hydroxide
Sodium Chloride
Water
HCl
NaOH
NaCl
H2O

17. ACID +
METAL 
SALT
HYDROGEN GAS
Hydrochloric Acid
Magnesium
Magnesium Chloride
Hydrogen
HCl Mg
MgCl2 H2

18. ACID +
CARBONATE
SALT
WATER
CARBON DIOXIDE GAS
Hydrochloric Acid
Calcium Carbonate
Calcium Chloride
Water
Carbon Dioxide

19. Molarity Molarity indicates the concentration
Given in the unit Moles/Liters
Moles is the SI unit for quantity- it indicates x1022 atoms or molecules of a substance
It is equal to the atomic weight of the element in grams
Ex g of O is one mole
32.00 g of O2 one mole