1. Chapter 15 Acids and Bases

2. I. Acids A. General Properties 1. Sour taste
2. Contain hydrogen, some react with metal ----> H2(g)
3. React with base ---> salt + H2O
4. Electrolytes
5. Changes blue litmus paper red

3. B. Definition 1. Traditional (Arrhenius)
Arrhenius acid - A chemical compound that contains hydrogen and ionizes in aqueous solution to form hydronium ions
Example:
HNO3(l) + H2O  H3O NO3-1

4. 2. Bronsted-Lowry Acid A molecule or ion that is a proton donor.
Example:

5. 3. Lewis Acid
An atom, ion, or molecule that is an electron pair acceptor
Example:

6. 4. Types of Acids a. Strong acid - strong electrolyte - ionizes 100%
Weak acid - weak electrolyte - ionizes very little
b. Monoprotic - 1 hydrogen ion - HCl
Diprotic - 2 hydrogen ions - H2SO4
Triprotic - 3 hydrogen ions - H3PO4

7. d. Mineral acids - made from minerals -
c. Organic acids - organic compounds that contain a carboxyl group (-COOH)
d. Mineral acids - made from minerals -
H2SO4, H3PO4, HCl, HNO3

8. C. Names and Structure of the Common Acids
1. Binary acids - hydrogen ion + nonmetal
hydro - __________-ic
hydrochloric HCl
2. Oxyacids - hydrogen ion + polyatomic ion
Polyatomic ion change ending
-ate to ic
nitrate nitric HNO3
-ite to ous
chlorite chlorous HClO2

9. D. Some Common Acids 1. Top 3 Industrial acids - H2SO4 H3PO4 HNO3
2. Uses
a. H2SO4 : fertilizer, petroleum, metallurgy, production of metals, paints, paper, dyes, battery acid
b. H3PO4 : flavorings in beverages, cleaning agent, manufacture of detergents, ceramic

10. c. HNO3 : explosives, rubber, plastics,dyes, drugs
d. HCl : pickling of Fe and steel, cleaning agent, food processing
e. HC2H3O2 : plastics

11. II. Bases and Acids - Base Reactions
A. General Properties of Aqueous Bases
1. Taste bitter
2. Feel slippery
3. Change colors in indicators (red litmus turns blue)
4. Reacts with acid ---> salt + H2O
5. Electrolytes

12. B. Definitions of Bases and Acid-Base Reactions
1. Traditional (Arrhenius)
Arrhenius Base- A solution that contains OH- and dissociates to give OH- in an aqueous solution - ionic compounds: metal + OH-
Example:

13. 2. Bronsted – Lowry Base-
A molecule or ion that is a proton acceptor
3. Lewis Base
An atom, ion, or molecule that is an electron pair donor

14. 4. Reactions
a. Neutralization - reaction of H3O+ and OH- to form H2O and a salt.
Salt - ionic compound composed of a metal cation (from base) and a nonmetal anion (from acid)
Acid + Base > salt H2O
HCl + NaOH ----> NaCl + H2O

15. b. Bronsted-Lowry acid-base reactions:
proton transfer from acid to base
Example
c. Lewis acid-base reactions:
formation of one or more covalent bonds between an electron pair donor (base) and an electron pair acceptor (acid)

16. C. Types of Bases 1. Strong bases - metals from Group 1 and 2
2. Weak bases - ammonia

17. III. Relative Strength of Acids and Bases
A. Bronsted- Lowry Acid -Base Pairs
1. Conjugate base - the species that remains after a Bronsted acid has given up a proton
2. Conjugate acid - the species formed when a Bronsted base gains a proton

18. HF + H2O --------> F- + H3O+
|____________|______________________|___________________|
acid base conjugate base conjugate acid
The stronger the acid, the weaker the conjugate base.
The stronger the base, the weaker the conjugate acid.

19. B. Relative Strength of Acids and Bases in Chemical Reactions
1. Proton-transfer reactions favor the production of the weaker acid and the weaker base

20. 2. To determine which direction will be favored:
a. Identify all compounds as acid or base
b. Determine which acid is stronger and which base is stronger (look on reference table)
c. The side favored is the one having the weaker acid and the weaker base

21. 3. Amphoteric - any species that can react as either an acid or base[H2O]

22. IV. Oxides, Hydroxides and Acids
A. Hydroxides, Acids, and Periodic Trends
1. OH- + metal ----> base
metal - large radii, low ionization, low electronegativity
2. OH- + nonmetal -----> acid
3. OH- + intermediate electronegativity and size ---> amphoteric
4. More O-2 increase acidity

23. For a compound to be acidic a water molecule must be able to attract a hydrogen from –OH group. This occurs easier when O-H is very polar.

24. V. Chemical Reactions of Acids, Bases, and Oxides
1. Acid +metal ----> salt + H2(g)
2HCl + Zn ---> ZnCl2+ H2(g)
2. Acid + metal oxide ----> salt + H2O
2HCl + MgO ---> MgCl2+ H2O
3. Acid + carbonate > salt H2O + CO2
2HCl + MgCO > MgCl2 +H2O + CO2

25. 4. Hydroxide + nonmetal oxide ---> salt or salt + H2O
NaOH + SO2--->NaHSO3 or
2NaOH + SO2---> Na2SO3 +H2O
5. Metal oxide + nonmetal oxide ---> oxygen-containing salt
MgO + SO2 ---> MgSO3

26. Examples 1. Write a balanced rxn for each: a. BaCO3 + HCl 
b. HNO3 + KOH 

27. 2. Zinc reacts with 250 mL of 6.00 M cold hydrobromic acid through single replacement.
How many grams of zinc bromide will be produced in the reaction?

28. 3. Calcium reacts with hydrochloric acid.
How many liters of hydrogen gas would be released at STP if 455 mL of 2.5M hydrochloric acid?