Properties of Acids• Dilute solution have a _____taste
• 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
Lemons have citric acid!
Vinegar has acetic acid!
_________________
Strong acid =
Weak acid =
Properties of Bases
• Bases have a bitter taste.
• Bases have a slippery or soapy feeling.
• Bases conduct an electric current.
• Bases react with acids to form water & salt.
• Bases cause acid-based indicators to change color.
Strong base=
Weak base =
Arrhenius TheoryArrhenius 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.
Proton ends up covalently bonding with water to form
_______________________
http://hogan.chem.lsu.edu/matter/chap26/animate3/an26_037.mov
So, acids dissolve in water & react to produce ______________ & ________________.
H2SO4 2H3O+ (aq) + SO4 2-
(aq)
H3PO4 3H3O+ (aq)
+ PO4 3- (aq)
Arrhenius TheoryArrhenius Base:
= _____________________________________________ _____________________________________________- Remember: hydroxide ion = OH-
NaOH Na+ (aq) + OH- (aq)
KOH K+ (aq) + OH- (aq)
http://hogan.chem.lsu.edu/matter/chap26/animate3/an26_038.mov
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/Greenbowe/sections/projectfolder/animations/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.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/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 H3PO4 = ___ H+
Monohydroxy Bases: OH- molarity = molarity of base solution- Ex: 3.0M NaOH = ___ OH-
Dihydroxy 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).