1. Ch. 16 Notes -- Acids and Bases
What makes something an acid?
Acid Properties:
(1) tastes _______-- _______________
(2) corrosive to _________
(3) contains [ ___ ] (or [ _____ ] = “_______________” ions)
(4) proton ([ ___ ]) __________-- Brønsted-Lowry Theory
Example: HCl + H2O  ______ + ______
sour
lemons
metals H+
H3O+
hydronium H+
donor
H3O+
Cl−

2. Examples of Common Acids:
Pepsi, _________ juices, ___________, stomach acid, battery acid, _____________, ______
citrus
aspirin
vinegar
DNA

3. Acid Vocabulary
strong acid - readily ___________ to produce ______ [H+] ions in water
Examples: _________, HNO3, _______
weak acid - produces a __________ amount of [H+] ions when in water
Examples: HC2H3O2 (vinegar) , _________, _________
dissociate
many
H2SO4
HCl
small
H2CO3
lemon juice

4. Strong Acids vs. Weak Acids

5. Indicator Colors For Acids
Indicators
An indicator is a chemical that will change ___________ when placed in an acidic, basic or neutral environment.
Indicator Colors For Acids
litmus paper = _______
phenolphthalein = ___________
red cabbage juice (universal indicator) = ________
methyl orange = _______
colors
red
clear
red
red

6. pH Paper : Indicator Colors
Neutral
Acidic
Basic

7. Properties of Bases What make something a base?
Base Properties: (…the opposite of acid properties)
(1) tastes ________ -- ___________ peel , parsley, dark chocolate
(2) feels _____________ -- ________
(3) contains [ _____ ] ions
(4) proton ([H+]) ______________-- Brønsted-Lowry Theory
Example: NH H2O  ______ + _______
bitter
banana
slippery
soap
OH−
acceptor
NH4+
OH−

8. Indicator Colors for Bases
litmus paper = _______
methyl orange = ____________
red cabbage juice (universal indicator) =________
phenolphthalein = ______
blue
yellow
blue
pink
phenolphthalein
Acid
Base

9. Common Bases
Examples of Common Bases: milk of magnesia, ___________, drain cleaner, soap, blood, ____________ tablets, ___________ ________.
ammonia
antacid
baking
soda

10. Strong Bases vs. Weak Bases
strong base- readily __________ to produce ______ [OH−] ions in water
Examples: NaOH , ________
weak base- produces a __________ amount of [OH−] ions when in water
Examples: _____ (ammonia); Mg(OH)2 (milk of magnesia)
Other Vocabulary
_______________- another term for basic solutions
_______________- a substance that can act as both an acid and a base
Examples: ___________ , ____________
dissociate
many
KOH
small
NH3
Alkaline
Amphoteric
H2O
HCO3−

11. Self-Ionization of Water
Pure water is _____________. It can ionize itself to form OH− and H3O+ ions in __________ amounts.
H2O + H2O  H3O+ + OH−
(or H2O  _______ + _______ )
The universal indicator color is ___________ in neutral solutions.
neutral
small H+
OH−
green
self-ionization of water

12. Measuring the Amount of H+ and OH− Ions in a Solution
_____ Scale- measures the _____________ of [H+] ions in a solution
_____ Scale- measures the concentration of [ ____ ] ions in a solution
Formulas
pH = − (log [H+]) pOH = −(log [OH−])
[H+] = 10−pH [OH−] = 10−pOH
[H+] x [OH−] = 1 x 10− pH + pOH = 14
With the pH scale, we have another way to define acids and bases:
Acids have a pH _________7.0
Bases have a pH _________7.0
Neutral pH ___7.0 pH
concentration
pOH
OH−
below
above =

16. Practice Problems:
1) a) Calculate the pH of a M HCl solution
b) Is this an acid or a base?
2) a) What is the concentration of [H+] ions in a solution that has a pH of 8.50?
[H+] = M
So…pH = − (log M)
pH = 3
Acid!
[H+] = 10−pH
[H+] = 10−8.5 Molar or 3.16 x 10−9 M
Base!

17. pH Testing

18. Alkalinity Testing

19. Neutralization Reactions
When an acid and base are mixed, the reaction produces _______
and ___________.
If the initial concentrations and volumes of the reactants are equal, the products will be ____________... (pH= 7.0)
All neutralization reactions are ___________ replacement reactions.
salt
water
neutral
double
H2O
HX + M(OH)  ______ ______ MX
(“Salt”)

20. Titration
Mixing an acid with a base to determine a __________________ is called “titration.”
An ____________ is used to determine when neutralization has occurred.
________________ Solution - the solution of known concentration
_________________ - the point of neutralization when titrating
At the eqivalence point, the moles of [H+] ions = moles of [OH−] ions.
The “_____ Point” is when the indicator changes color.
concentration
indicator
Standard
Equivalence Point
End

21. Titration Curve

22. (1) Complete the following neutralization reactions.
Practice Problems:
(1) Complete the following neutralization reactions.
HNO3 (aq) KOH (aq)  _________ __________
HCl (aq) Ca(OH)2 (aq)  __________ + ___________
(2) How many moles of Ca(OH)2 will it take to neutralize 0.5 moles of HCl?
3) How many moles of HNO3 will it take to neutralize 3.0 moles of KOH?
KNO3
H2O +2 −1
CaCl2
H2O 2 2
1 mole Ca(OH)2
0.5 moles HCl
0.25 moles of Ca(OH)2 x =
2 moles HCl
1 mole HNO3
3.0 moles KOH
3.0 moles of HNO3 x =
1 mole KOH

23. Determining the Concentration of an Acid (or Base) by Titration
(Macid)x(Vacid) = (Mbase)x(Vbase)
Practice Problems:
A 25 mL solution of HNO3 is neutralized by 18 mL of 1.0 M NaOH standard solution using phenolphthalein as an indicator. What is the concentration of the HNO3 solution?
(2) How many mL of 2.0 M KOH will it take to neutralize 55 mL of a M HCl standard solution?
( ) x ( ) = ( ) x ( )
Macid
25 mL
1.0 M
18 mL
Macid = Molar
( ) x ( ) = ( ) x ( )
0.76 M
55 mL
2.0 M
Vbase
Vbase = mL