Acid/Base Review
List the properties of Acids
• Sour, H3O+ ions, strong acids conduct,
react with metals to form H2 gas,
neutralize bases to form salt + water.
Acids Ionize with water to form H3O+,
litmus red
List the properties of bases
• Bitter, slippery, OH- ions, strong bases
conduct, , neutralize acids to form salt +
water. Strong bases dissociate (water on
arrow), litmus blue
Give two examples of weak acids
and one example of a weak base
• H2S-Hydrosulfuric Acid
• HCH3COO-acetic acid
• NH3 – ammonia (weak base)
List the 6 strong acids
•
•
•
•
•
•
HBr
HI
HCl
HNO3
H2SO4
HClO4
• Remember these acids ionize completely
in water creating a strong electrolyte!
Explain the difference between an
oxyacid and a binary acid and give
an example of each
• Oxyacid has oxygen in the compound
H2SO4
• Binary acid means that there are two
compounds present
HCl
List common acids that we have
talked about
• Phosphoric Acid-found in soda/used to
make fertilizer
• HCl-found in the stomach
• Acetic Acid-vinegar
List the strong bases
• Anything in column 1 & 2 bonded with an
OH-
Explain the Arrhenius Acid Definition
• Acids produce H+ in solution
• Acid – produces H+ in water
• HCl + H2O  H3O+ + Cl• H2SO4 + H2O  2H3O+ + SO42• Remember H+ can also mean H3O+ (Hydronium
Ion)
Explain the Arrhenius Base Definition
• Base – produces OH- in water
NaOH  Na+ + OHNH3 + H2O  NH4+ + OH-
Explain the Bronsted-Lowrey
Definition of Acids/Bases
• Acids are H+ donors,
• bases are proton (H+ ) acceptors.
• HCl + H2O  Cl + H3O+
acid base
• Bronsted-Lowry is a way to study proton
transfer!!
Explain conjugate Acid/Base
• Conjugate Acid – formed when BL base
gains a proton
• Conjugate Base – formed when BL acid
looses a proton
•
HCl + NH3
 NH4+ + Cl•
a
b
ca
cb
•
H2SO4 + 2H2O  2 H3O+ + SO42a
b
ca
cb
If I have a strong acid what is the
strength of the conjugate base?
• The stronger the acid, the weaker its
conjugate base; the stronger the
base, the weaker its conjugate acid
Study your conjugate acid/base
worksheet as there are a few
questions on recognizing a/cb
and b/ca pairs
What is an amphoteric substance
and give an example
• Water:
• can react as either an acid or base
• HCl + Water 
H3O + + Cl proton acceptor(water)
• Water + NH3
 NH4 + + OH Water(proton donor)
Complete the following Reactions
• 3KOH
+ H3PO4 →
K3PO4 +
3 H 2O
• Mg(OH)2 + 2 HCl →
2H2O
+ MgCl2
Are strong acids/bases strong or
weak electrolytes?
• Strong because they will completely ionize
or dissociate creating many ions…….
• Weak acids/bases do not ionize
completely thus there are fewer electrons,
thus they are not very strong electrolytes
How many moles of Nitric acid are
in 500 ml of a 10 M HNO3 solution?
• 5 moles
What does pH measure?
pH – related to the concentration of H3O +
ions in solutions. The more H3O+ ions,
the lower the pH.
Given the H3O+ concentration find
the pH / pOH…A/N/B
• [H3O+]=7.3x10-13
– pH=12.13
– pOH=1.86
– Basic
• [H3O+]=5x10-2
– pH=1.3
– pOH=12.2
– Acidic
Given the pH find the Hydronium or
hydroxide ion concentration
• pH= 3.1
• [H3O+]= 7.9x10-4
• pH= 10.5
• [H3O+]=3.2x10-11
Draw a strong acid/strong base
titration curve
Draw a weak base strong acid
titration curve
Summary of titration curves
During a titration curve why do we
have to titrate so slowly when we
get close to the equivalence
point/end point?
• When the hydronium ions and hydroxide
ions are nearly equal (the equivalence
point) the curve of graph is very steep and
thus happens very quickly.
Explain the End Point
• When the indicator changes color which
should be close to the equivalence point if
chosen correctly.
– Ex. Strong acid/strong base should be litmus
– Ex. Strong base/weak acid should be
phenolphthalein
What is the pH of a .036M LiOH
solution
• First find the pOH by finding the normality
– Remember normality = molarity x equivalence
– Then you take the
–log (normality concentration)
-log (.036)=1.44 but that equals the pOH
Then you take 14-1.44=12.56 which gives you
the pH
pH=12.56
To neutralize 20 ml of aqueous sulfuric
acid, you use 32.5 ml of a 0.2 M NaOH
solution.
Calculate the Molarity
• Molarity of H2SO4 =0.16
What volume of 0.5 M sulfuric acid is
needed to react completely with 10 ml of
2.0 M LiOH
H2SO4 + 2LiOH → Li2SO4 + 2H2O
.02L
A 20 ml sample of 0.55 M KOH solution required
30 ml of aqueous acetic acid solution in a titration
experiment. Calculate M & N &pH of the acid.
• Molarity = HCH3COO=0.367
• Normality = M x eq = 0.367 x 1 = 0.367
• pH= -log [N]= -log(0.367) = .435
If you start with a pH of 1 and add water
what should you expect to have happen to
the pH?
• You should expect it to neutralize
• pH of 1 = .1M
• When you add water you dilute it so the next
step would be .01M. The pH would be 2.
• .001M = pH 3 etc.
• What would a graph look like?
You have a 4 M solution of NaOH. You need to
make up 2000 ml of a 1.5 M solution. How many
mls of the 4 M solution do you need? How much
water would you need?
• V1
• V1
x
x
• V1=750ml
M1
4M
=
=
V2
x M2
2000 x 1.5
What is the salt produced when
KOH is used to neutralize sulfuric
acid?
• K2SO4