The Chemistry of
Acids & Bases
Properties of Acids
• Dilute solution have a _____taste
Lemons
have citric
acid!
Vinegar has
acetic acid!
• Aqueous solutions conduct an electric current
 What do we call substances that can conduct electric currents?
_________________
**The greater the # of ions in solution, the greater the electrical conductivity.
• Acids react with bases to form a water & salt
 _____________________
• Acids react with certain metals to produce H2 gas
 Table J: _____________________________
• Acids cause acid-base indicators to change color
Strong acid =
Weak acid =
Properties of Bases
• Bases have a bitter taste.
• Bases have a slippery or soapy feeling.
• Bases conduct an electric current.
Strong base=
Weak base =
• Bases react with acids to form water & salt.
• Bases cause acid-based indicators to change color.
Arrhenius Theory
Arrhenius Acid
= ______________________________________
______________________________________
- Ex:
**Some notes on the hydrogen ion!:
 H+ is really just a _________!
 In a water solution, the positively charged proton is
attracted to an unshared pair of electrons in the water
molecules.
http://hogan.chem.lsu.edu/matt
er/chap26/animate3/an26_037.
mov
Proton ends up covalently bonding with water to form
_______________________
So, acids dissolve in water & react to produce
______________ & ________________.
H2SO4 
2H3O+ (aq) +
SO4 2- (aq)
H3SO4 
3H3O+ (aq) +
SO4 2- (aq)
Arrhenius Theory
Arrhenius Base:
= _____________________________________________
_____________________________________________
- Remember: hydroxide ion = OH-
NaOH  Na+ (aq) +
KOH
http://hogan.chem.lsu.edu/matter
/chap26/animate3/an26_038.mov
OH- (aq)
 K+ (aq) + OH- (aq)
Other Acid/Base Definitions
Brønsted – Lowry Acids = _____________
Brønsted – Lowry Bases = _____________
Note: A “proton” is really just a hydrogen atom that has lost it’s electron!
Lewis acid = _____________________________
Lewis base = _____________________________
Neutralization Reactions
= an Arrhenius acid reacts with an Arrhenius base to produce
water & a salt
=
- General reaction:
**All neutralization reactions have the same net equation:
http://www.chem.iastate.edu/group/Gre
enbowe/sections/projectfolder/animation
s/HClandNaOHtgV8.html
Acid-Base Titration
= the process of adding measured volumes of an acid or base of known
concentration to an acid or base of unknown concentration until
neutralization takes place
- Through a titration, it is possible to calculate the concentration of the
unknown solution:
MAVA = MBVB
http://www.chem.i
astate.edu/group/
Greenbowe/sectio
ns/projectfolder/fla
shfiles/stoichiomet
ry/acid_base.html
Monoprotic Acid: H+ molarity = molarity of acid solution
- Ex: 2.5M HCl = 2.5M H+
Diprotic Acid: H+ molarity = 2 x molarity of acid solution
- Ex: 2.5M H2SO4 = ___ H+
Triprotic Acid: H+ molarity = 3 x molarity of acid solution
- Ex: 2.5M H3SO4 = ___ H+
Monohydroxy Bases: OH- molarity = molarity of base solution
- Ex: 3.0M NaOH = ___ OHDihydroxy Bases: OH- molarity = 2 x molarity of base solution
- Ex: 3.0M Ba(OH)2 = ___ OH-
Acidity vs. Alkalinity
** These terms refer to the relative strength of the acid or
base in terms of H+ and OH- concentrations.**
- Acidity  ___________________________
- Alkalinity  _________________________
[H+] > [OH-] :_________
[H+] < [OH-] :_________
pH Scale
 The pH scale expresses [H+] as a number from 0 to 14
 Each pH unit represents a tenfold increase or decrease in [H+] and
[OH-].
 As [H+] increases, [OH-] decreases (and vice-versa).
Acid-Base Indicators
Indicator
= ____________________________________
____________________________________
**REMEMBER: Everything you need to know about acidbase indicators is on Table M in the reference tables!!**
http://hogan.chem.lsu.edu/
matter/chap27/demos/dm
27_010.mov