Acids, Bases, and Salts: Unit 6 Outline
Characteristics of Acids
• Molecular substances that ______________ in water.
a. ___________ difference is less that 1.8
b. It’s a non-polar covalent molecule
c. Creates ___________ in solution
• Acids react with ___________ metals to create hydrogen gas.
a. Active metals include, ______________________.
b. Cu, Ag, Au, Pt. DO NOT react with acids
c. Metal + Acid  ___________+ H2 (g)
• Affect the color of ___________.
• React with bases  more neutral solution of H2O + ___________
• Edible acids have a ___________ taste<don’t try this!>
Arrhenuis Acids
• A solution that yields an ___________ (a ____________) as one of its
components in solutions.
• H + Ions are always ___________.
• Strong acids have:
a. 1 H+ proton = 1 ______________________
• Weak acids have more ___________ molecules for every H+
Ionization of Acids
• The higher the rate of ionization, the more ___________ the acid.
• Strong: HCl: nearly ___________ ionized.
•
sulfuric acid(H2SO4) ___________ ionized.
• Weak: Hydrofluoric acid (HF): ___________ions
•
Hydrosulfuric acid: ___________ions.
Properties of Bases
• ___________
• Cause ___________ to turn colors
• Neutralize acids and produce a ___________+ H2O
• ___________ taste, ___________ feel
• Soap in the mouth?
Arrhenuis Bases
• Contribute a OH- (___________) in solution.
• OH-, unlike H+, does not attach to other molecules UNLESS it has a
___________ charge
Ionization of Bases
• Ionize similar to acids, except that Bases tend to be ___________ compounds.
• The OH- ion is ___________, while the metal attached is bonded ___________
• Strong Bases: ___________ (almost 100%)
a. Weak Bases: Ammonia compounds: ___________
Salts
•
•
•
•
Ionic compounds that have Ions other than ___________ and ___________.
SOLID=___________
Conduct ___________ when molten OR in solution
Tend to have ___________ melting points
The Ionization of Water
• Water ionizes itself
• For any sample of water:
•
H2O  H3O+ + OH• H2O = 1 mole; H3O+ = ___________mole and OH- = ___________mole
• In 10,000 L of H2O, there would be ___________of H2O- one drop from a
dropper!
Ionization of Water… continued
• There are ___________amount of H3O+ and OH- ions.
• This allows water to:
a. Be perfectly neutral
b. Neutralize other substances through self ionization.
•
- If an ___________ion pops in, the OH- can ___________ it to a certain
extent.
•
- Most solutes are combinations of ___________and ___________, so,
water dissolves and separates them.
Ionization of Water… continued
• Kw= OH- x H3O+
• In any sample:
___________ =
1.0x10-7
•
___________ =
1.0x10-7
• Then Multiply:
___________ =
1.0x10-14
• Soooooooooooooooooooo… for a solution to be perfectly ___________, it must
have ___________ ___________ of OH- and H3O+ions.
The pH Scale
• A measure of the ___________ or ___________ of a solution, based on the
concentration of the ___________in solution.
• pH= “pouvoir Hydrogen” = Power of Hydrogen
• The pH of a given solution is: equal to the ___________of the Hydrogen Ion
___________ in a given solution.
a. ___________scale
b. Small # = ___________
c. Large # = ___________
• The p OH scale: OPPOSITE of the pH scale.
a. pH + p OH = 14; Why?
• Because we want to compare pH to ___________—which always
has
___________
So—[H+] [OH-] = Kw and Kw= 1.0x 0^-14
Another View of Acids and Bases
• Bronsted- Lowry
a. Acids: ___________
b. Bases: ___________
• NH3 + H2O  NH4+ + OHa. Draw Lewis dot structures
b. ___________ Acids and Bases
c. Strengths of acids chart: P.565
More Acids and Bases
• ___________= Ionization Constant for an acid.
•
Strong Acids (HCl, H2SO4, HNO3, etc.) -all of the compound will
___________.
a. Weak Acids all ___________at various rates: HC2H3O2 will ionize at
lower rate than the strong acids. This affects acid strength.
• ___________= same thing, except for bases instead of acids.
• The ionization constants tell you the number of moles of the acid (Ka, H+) or base
(Kb, OH-) in ___________of a ___________ solution.
• More simply, it’s the ___________of a particular ion in solution.
Key Terms
• ___________, ___________ (and complete…)
• ALL refer to a compound breaking apart into the ions that make the compound
up.
• Simple Reactions:
a. Adding an acid to a metal will produce?
b. Adding a base to an acid will produce?
• Any reaction that makes an acid or base from its constituent parts is called Acid
(or base) Formation.
a. H + Cl = HCl.
• Neutralization- An acid + base reacts to produce a salt plus water.
Net Ionic Equations
• Net Ionic Equations*- In some instances, only a few certain elements are involved
in a reaction. To ‘simplify’ the equation, all the inactive parts are removed from
the equation.
• HCl (aq) + Zn (s)  H2 (g) + ZnCl (aq)
• H changes from a ___________ to a ______________________.
•
Zinc does the opposite
•
But what does the chlorine do?
• We write:
•
H+ + Zn0  H20 + Zn +
• Since the Cl stays a ___________ ___________, we can leave it off for this type
of equation.
• Net Ionic Equations only occur in a special type of reaction, called ___________
Redox
• Redox is short for ______________________reaction.
•
Redox Reactions are an important part of chemistry.
•
Redox Reactions are a result of ______________________.
• In our example above, electrons are taken from the Zinc, and given to Hydrogen.
This makes Zinc an ion, and Hydrogen a free element—the opposite of what they
were before the reaction.
•
Reduction is the ___________of electrons. Why do we call it reduction?
•
Oxidation is the ___________of electrons.
To remember this:
“LEO says GER”
______________________= Oxidation;
______________________= Reduction