Chapter 14 Notes
Naming Acids (page 230)
Binary Acids- acids that consist of two elements, usually hydrogen and one of the halogens.
a. Naming: Hydro-(Base word of anion)-ic Acid
b. Examples:
HCl-
Hydrochloric Acid
HF- Hydrofluoric Acid
Oxyacid- acids that contain a polyatomic ion
a. Naming: __________________ ic (or ous) Acid
b. Polyatomic ions ending in –ate, will have an –ic ending.
Example: H2SO4
Sulfuric Acid
c. Polyatomic ions ending in –ite, will have an –ous ending.
Example: H2SO3
Sulfurous Acid
Properties of Acids and Bases (Section 14.1, page 467-476)
Acids
1. Aqueous solutions of acids have a Sour taste.
2. Acids change the color of acid-base indicators.
3. Some acids react with active metals and release hydrogen gas
a. Zn(s) + 2 HCl(aq)  ZnCl2(aq) + _H2_(g)
4. Acids react with bases to produce salts and water.
a. HCl(aq) + NaOH(aq)  _NaCl_(aq) + _H2O__(l)
5. Acids conduct electric current
-Industrial uses for Acids (answers may vary See page 470-471)
a. Sulfuric Acid-Refining petroleum and in the manufacture of fertilizers. Removes water
(dehydrating).
b. Nitric Acid- Stains and explosives
c. Phosphoric Acid- manufacturing fertilizers and animal feed
d. Hydrochloric Acid- removes surface impurities
e. Acetic Acid-Vinegar
Chapter 14 Notes
Bases
1.
2.
3.
4.
5.
Aqueous solutions of bases taste __Bitter_ (very dangerous to skin-cause burns)
Bases change the color of acid-base indicators
Dilute aqueous solutions of bases feel __Slippery____
Bases react with acids to produce salts and water
Bases conduct electrical currents
Learning Check
How are acids and bases similar and different? You may want to refer to pages 467-472 in your
textbook.
Different- Taste and reactions. Same- Change color of indicators, conduct electricity
Acid-Base Theories (Section 14.2, page 478-482)
Arrhenius Acids and Bases
Arrhenius Acids- Increase the concentration of H+ ions or H3O+ ions (Hydronium ions)
Example: HNO3(l) + H2O(l)  ___H3O+ (aq) + ____NO3-__ (aq)
Arrhenius Bases- Increase the concentration of OH- ions.
Example: KOH (s)  ___K+__ (aq) + ___OH-___(aq)
Strength of Acids
A strong acid is one that ionizes completely in aqueous solutions.
-
See Table 3 on page 474 and record some common strong acids and weak acids
Strong Acids
Weak Acids
HI, HClO4, HBr, HCl, H2SO4, HClO3
HSO4-, H3PO4, HF, H2S. etc..
*In general, organic acids (Ones that contain hydrogen, oxygen, and carbon) are weak acids.
Strength of Bases
Strong bases completely dissociate in water and for aqueous OH- ions.
-
See Table 4 on page 475 and record some common strong acids and weak acids
Strong Bases
Weak Bases
Metal Hydroxides
Non- metal bases
Not all bases are ionic compounds- Example NH3 ammonia.
Chapter 14 Notes
Bronsted-Lowry Acids and Bases
Acid-base Reaction
Acid + Base ↔ Cation + Anion
Acids- As a reactant, acids are proton (H+) donors
Monoprotic- donates one proton
Polyprotic-donates more than one proton
Diprotic- 2 protons/molecule, Triprotic- 3 protons/molecule
Bases- As a reactant, bases are proton (H+) acceptors
Example Reaction-Record Example from page 478 in Textbook and Label which reactant is the base and
which reactant is the acid:
Lewis Acids and Bases
Lewis Acid- an atom, ion, or molecule that __accepts__ an electron pair from a covalent bond
Lewis Base- an atom, ion, or molecule that ___donates___ an electron pair to form a covalent bond
Lewis Acid-Base Reaction
Example Reaction-Record Example from page 482 in Textbook and Label which reactant is the base and
which reactant is the acid: (Answers May Vary)
Acid Base Reaction Theories Review:
Complete the table below (use notes above or see page 482 for help!)
Type
Acid
Base
Arrhenius
H+ or H3O+ Producer
OH- producer
Bronsted-Lowry
Proton donor
Proton Acceptor
Lewis
Electron pair acceptor
Electron pair Donor
Chapter 14 Notes
Acid-Base Reactions (Section 14.3, page 483-498)
*In this section we will use the Bronsted-Lowry description for acids and base reactions.
Conjugate Acids and Bases
The species that remains after a bronsted-lowry acid has given up a proton in the_____conjugate_____
__base___ of that ____acid___.
Example: Label the acid and conjugate base in the example below
HF + H2O ↔ F- + H3O+
Conjugate Acid the species that is formed when a base gains a proton.
Why are there two acids and bases in each Bronsted-Lowry reaction?
One acid and base as a reactant, then form an acid and base as a product—which then can react and
form the reactants again.
Strength of Conjugate Acids and Bases
1. The ___stronger___ the acid is, the ____weaker__ its conjugate base; the __stronger__ a base
is, the weaker its conjugate acid.
2. Proton transfer favors the production of the __weaker_ acid and ___weaker__ base.
Amphoteric Compounds
Any species that can react as either an acid or a base is described as ___Amphoteric________.
Water is a common amphoteric compound.
In the reactions below, determine which reaction uses water as an acid and which uses water as a base.
Circle your answer.
Acid or Base
Acid or Base
H2SO4 (aq) + H2O(l)  H3O+ (aq) + HSO4- (aq)
NH3(g) + H2O(l) ↔ NH4+ (aq) + OH- (aq)
OH_ in a Molecule
As the number of _oxygen__ atoms _____increase____, so does the acidity of the compound.
Chapter 14 Notes
Neutralization Reactions
When an acid and a base react to form a neutral substance, a neutralization reaction has occurred.
1. Strong acid-strong base neutralization
a. Hydrochloric acid and sodium hydroxide combine to form water and sodium chloride
b. Balanced Equation: _______HCl + NaOH  H2O + NaCl _____
2. Acid Rain
a. When a gas combines with water in the atmosphere to produce an acidic solution.
b. Examples of gases that form acid rain: NO, NO2, CO2, SO2,SO3__
c. Example reaction- Write the balanced equation for the acid rain reaction between
sulfate gas and water:
SO3(g) + H2O (l)  H2SO4 (aq)