Unit 12 Acids and Bases
Chapter 19
Lesson 1 – Acids and Bases
Arrhenius’ Definition
Acids give _________________when dissolved in _______________________
Bases give _________________when dissolved in _______________________
Acid or Base?
The measure of the __________________ of _________ ions in a solution is called _____________
The _________________ measures how _____________ or ______________ a solution is
The scale ranges from _______ to ________.
_______ = extremely strong acid
Properties of Acids
Affects the color of ____________________
_____________ with metals to produce ________________gas.
Metal + Acid 
____________________________ of bases to form water.
Acid + Base 
Taste ____________
Strong and Weak Acids
Strong acids will _________________ _______________________.
(all of molecules become ions)
HCl(aq) + H2O(l)  H3O+(aq) + Cl-(aq)
Weak acids do not ________________________________ easily.
(only a few molecules become ions)
HC2H3O2(aq) + H2O(l) 
H3O+ (aq) +
C2H3O2 -
H3O+ = _____________________ (same as ___________)
Strong Acids (need to know!)
Hydrochloric acid
Hydrobromic acid
Hydroiodic acid
Nitric acid
Sulfuric acid
Chloric acid
Perchloric acid
______ = extremely strong base
Weak Acids
Carbonic acid
Acetic acid
Citric acid
Mono and Polyprotic Acids
Monoprotic Acids
Mono = _________________
These acids donate ________________ (per molecule) when they ______________________
HCl 
HNO3 
Polyprotic acid
Poly = ____________________
These acids donate ____________________ one H+ (per molecule) when they dissociate
Polyprotic acids ionize in ______________________.
H2S
H3PO4 
Properties of Bases
Affects the color of _____________________
Neutralization of ______________________ to form water.
Acid + Base 
Taste _____________________
Strong and Weak Bases
Strong bases:
Group 1a:
Group 2a:
yield ________________ in solution
Feel _____________________
Weak bases _________ _____________ dissociate in solution, they just __________________ a H+
Examples:
Bronsted-Lowry Definition
Acids are any substance that can ______________________ an _________
Bases are any substance that can ____________________ accept an __________
Example
Conjugate Pairs
Reversible reactions have an _______________and _________________ on both sides
Pairs that differ by only ________ ________________ (___________) are called conjugate pairs
A ____________ acid will make a weak _____________________ base
A ______________ acid will make a strong _____________________________ base.
Same for ________________and __________________ bases.
What about H2O? Acid or Base?
Water is ___________________________ which means a substance can either ______________________ a proton
(base) or _______________________ a proton (acid).
Water will act as a _________________ when in solution with ______________________
Water will act as a _________________ when in solution
with ______________________
Lesson 2 – pH and pOH
pH
Low pH = __________________
pH = _______________ of _______________________
Power is the ________________ power, as in 10 to the second power = _____________________
[H+] = _________________________of ______________ ion (molarity)
The __________________ the concentration, the stronger the acid, the _____________________ the pH
[H+] =
Solving for pH:
pH =
pH examples
What is the pH of a solution if the H+ concentration is 3.4 X 10-3 M?
What is the H+ concentration of an acid with a pH of 3.0?
pOH
Low pOH =_____________________________
pOH =measure of ____________ ion concentration
pOH is __________________________ from ____________
[OH-] = ______________________________of ____________ ion (molarity)
The higher the concentration, the stronger ___________________, the lower the _______________
[OH-] =
Solving for pOH:
pOH =
pOH Examples
What is the pOH of a solution if the OH- concentration is 3.4 X 10-6 M?
What is the OH- concentration of a base with a pOH of 2?
pH and pOH
pH is a measurement of the __________________
pOH is a measurement of the ________________
pH = __________________
pOH = ____________________
pH and pOH must equal _____________________________
pH
+
pOH
=
___________ can be found when you know ____________and vise versa
In _________________ water, pH and pOH are ____________
All aqueous solutions have a ___________and a ________________.
Example
If [H+] = 1.0 x 10-7 M, then what is the pH?
Example
If the [OH-] is 5.01 x 10-4 M, what is the pOH?
Sample Problem
In household bleach, the concentration of OH- ions is 5.0 x 10-2 M.
What is the pH?
Lesson 3 – Titration/Neutralization
Neutralization
_______________ + ___________________

__________ + ____________
Water is formed when the _____________ from the acid contacts the _________________ from the base.
__________________is an ____________________ compound formed from the other parts of the acid and base.
Terms
____________________ is a lab technique used to determine the ___________________________of an
___________ or ________________.
_____________________ is when the number of moles of ____________________ _________ equals the
number of moles of _______________________ ____________.
This does ________necessarily mean pH is ______________, as the salt may _____________ the pH of the
solution
________ ___________________is when the _____________________changes colors.
(Meaning the solution has changed from ______________________ to _________________________)
Indicators
An indicator is a chemical that _______________ _______________ at a __________________ _______.
Many indicators are a mixture of many chemicals.
Some are found naturally
Steps for Titrations
1. A measured volume of an ____________ or __________ solution of an ___________________ concentration
is placed in a flask
2. Several drops of _______________________ are added to the flask
3. Measured volumes of a ___________________ (or acid, if a base is in the flask) of ______________
concentration (_____________ solution) are placed in a ______________ and slowly added into the acid
until the indicator _____________________.
Lab Example
Phenolphthalein indicator is clear in _______________ and pink in ________________.
The endpoint is when __________extra drop of _________________ is added after equivalence is reached,
changing the indicator color.
Titration
The ________________ of an unknown solution can be determined
_______________ (unknown solution) added from a ___________
___________________are chemicals added to help determine when a reaction is complete
The __________________ of the titration occurs when the reaction is complete
This is also known as the __________________ ________________ – the point in the titration when the number of
moles of _________ added _____________ the number of moles of ___________ originally in solution
Plotting a Titration Curve
Neutralization Calculations
If the number of moles of __________ = moles of __________, you can use ___________________ to find the
______________ of the unknown
Example - A 43.0 mL volume of NaOH was titrated with 32.0 mL of 0.100 M HCl.
sodium hydroxide solution?
Step 1: how many moles of HCl were needed?
Step 2:
How many moles of H are in each mole of the acid?
Step 3:
Moles H+ = Moles OH-
What is the molarity of the
Step 4: How many moles of OH are in each mole of base?
Step 5: calculate Molarit
Example
A volume of 50.0 mL of 1.20 M H3PO4 neutralizes 45.5 mL of a Ca(OH)2 solution.
Ca(OH)2 solution?
What is the molarity of the
Neutralization Calculations (quicker)
The same formula as dilutions:
___________________ are for the ______________________solution
_____________________ are for the _________________ solution
___________________are the coefficients from the ____________________________________.
*You must have a ___________________________________________ for this to work!
Example
Solutions of sodium hydroxide (NaOH) are used to unclog drains. A 43.0 mL volume of NaOH was titrated with
32.0 mL of 0.100 M HCl. What is the molarity of the sodium hydroxide solution?
Sample Problem
A volume of 25. mL of 0.120 M H2SO4 neutralizes 40. mL of a NaOH solution.
NaOH solution?
What is the concentration of the
Lesson 3 – Salt Hydrolysis
A salt is an _________________ ___________________________ that: comes from the
____________________________ of an acid; comes from the ____________________________ of a base; is
formed from a ________________________________reaction; some neutral; others ________________ or
_____________________.
“Salt hydrolysis” - a ____________________that reacts with water to produce an ______________ or
___________________.
Salt Hydrolysis
Hydrolyzing salts usually come from:
a strong acid + a weak base =
a weak acid + a strong base =
A strong acid + a strong base =
a weak acid + a weak base =
“Strong” refers to the __________________ of ___________________________
Strong Acids
Strong Bases
Salt Hydrolysis
To see if the resulting salt is ____________ or ____________, check the ________________
formed it.
Practice on these:
HCl + NaOH
H2SO4 + NH4OH
H2S+ KOH
acid or base that