Chapter 6: Acids and Bases
6.1 Theories of Acids and Bases
A. Naming Acids and Bases
 acids always have ______ as the state and always have ________________
Classical Naming Rules
1. hydrogen _________ide becomes hydro_______ic acid
2. hydrogen _________ate becomes __________ic acid
3. hydrogen _________ite becomes __________ous acid
Examples
Change each of the following to the appropriate acid name and give the
formula:
1. hydrogen iodide =
2.
hydrogen phosphate =
3.
hydrogen nitrite =
4.
hydrogen sulphite =
 most bases are ionic compounds that are named accordingly
Examples
Name each of the following bases:
1. NaOH(aq) =
2.
NaHCO3(aq) =
3.
Mg(OH)2(aq) =
4.
NH3(aq) =
 IUPAC names for acids and bases are simply the word “aqueous” followed
by the ionic name
Examples
Write the IUPAC name for each of the following acids and bases:
1. hydroiodic acid =
2. magnesium hydroxide =
3. sulphurous acid =
4. sodium hydrogen carbonate =
Chemistry 20 Solutions, Acids, Bases Notes
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B. Properties of Acids and Bases
 ___________________________________ are _______________________
____________________________ of a substance
 acids, bases and neutral substances have some properties that distinguish
them and some that are the same
Acids
 ________ taste
Empirical Properties
Bases
 ___________ taste
 ________________
 ________________
 _____________________
 neutralize ________
 neutralize _______
_____________________
 react with ________
 react with ________
 do not affect indicators the
litmus - ___________
litmus - _____________
bromothymol blue - ___________
bromothymol blue – ___________
phenolphthalein – _____________
phenolphthalein – _____________
Neutral Substances
same way
 react with ________
to produce ______
 pH _____________
 pH _____________
_________________
_________________
eg)
eg)
 pH _____________
eg)
C. Arrhenius Definition
 ___________________________________ first proposed theory on acids
and bases
 his theory was that some compounds form __________________________
_________________________________ when in
_____________________ (he almost failed his PhD thesis on this because
electrons hadn’t been discovered yet…then won the Nobel Prize later for
the same ideas!)
Chemistry 20 Solutions, Acids, Bases Notes
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 his explanation of the properties of acids and bases is called the
____________________________________________________________
 an Arrhenius ________ is a substance that _________________ (because it
is molecular) to form ___________________________________________
 an ____________ will __________________________________________
in an aqueous solution
 an Arrhenius ___________ is a substance that _______________________
to form _______________________________________________ in water
 a ___________ will ________________________________________ in
an aqueous solution
D. Modified Arrhenius Definition
 the original definition of acids and bases proposed by Arrhenius is good but
it has _______________________________
 as you saw, some substances that might be predicted to be _____________
are actually ______________
eg)
 it has been found that not all bases contain the _______________________
as part of their ___________________________________
 an Arrhenius ________________________________ is a substance that
______________________________ to produce _____________________
in aqueous solution
eg)
 when acids ionize, they produce ____________________
eg) HCl(g) 
 it has been found using analytical technology like X-ray crystallography
that ________________________________________________________
in an aqueous solution
Chemistry 20 Solutions, Acids, Bases Notes
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 the hydrogen ion is extremely positive in charge and water molecules
themselves are very polar so…it is _____________________________ that
_____________________ would exist in water without being attracted to
the ____________________________ of ___________________________
________________________________
 this results in the formation of the ________________________________:
 an Arrhenius ____________________________ is a substance that ______
______________________ to produce ________________________ in
aqueous solution
eg)
6.2 Strong and Weak Acids and Bases
 the ____________________________________________________ of a
substance depend on two things:
1. the __________________________ of the solution
2. the _____________________ of the acid or base
A. Strong Acids and Weak Acids
 an acid that ionizes almost _________ in water is called a _____________
_____________
eg)
 100% of the __________ becomes ____________ and _____________
Chemistry 20 Solutions, Acids, Bases Notes
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 the concentration of the _________________ is the _____________ as the
concentration of the _________ it came from
 strong acids are ________________________________ and ___________
_________________________________________________
 there are 6 strong acids:
perchloric acid
hydrobromic acid
hydroiodic acid
hydrochloric acid
sulfuric acid
nitric acid
HClO4(aq)
HBr(aq)
HI(aq)
HCl(aq)
H2SO4(aq)
HNO3(aq)
 a ___________________________________________________ and only
a small percentage of the acid forms _______________________________
eg)
 we use the ______________________________________ for weak acids
 weak acids are _________________________________ and ___________
_________________________________________________
B. Strong Bases and Weak Bases
 a base that dissociates _________ into ions in water is called a __________
_______________
 _________________________________ and _______________________
are strong bases
eg)
 a ____________________________________________________ and
only a small percentage of the base forms __________________________
eg)
 we use the ______________________________________ for weak bases
Chemistry 20 Solutions, Acids, Bases Notes
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Your Assignment: pg 1
C. Monoprotic and Polyprotic Acids
 acids that have only _________________________________________ per
molecule that can ________________ are called _____________________
____________
eg)
 monoprotic acids can be _______________________________
 acids that contain _______________________________________ that can
________________ are called ___________________________________
eg)
 acids with _________________________ are ___________________, with
____________________________ are _____________________
 when polyprotic acids ionize, only __________ hydrogen is removed at a
time, with each acid becoming ___________________________________
eg)
Chemistry 20 Solutions, Acids, Bases Notes
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D. Monoprotic and Polyprotic Bases
 bases that _____________________________________________________
__________________________ are called _________________________
eg)
 bases that react with water in ___________________________ are called
_____________________________________________
eg)
 as with polyprotic acids, only ________ OH(aq) is formed at a time, and
each new base formed is _____________________ than the last
eg)
E. Neutralization
 the reaction between an acid and a base produces an __________________
_______________________ and ________________
eg)
 the products of ___________________________ are both ______________
 in a neutralization reaction or _____________________________________
between a _________________________ and a _____________________,
the product is always __________________
Chemistry 20 Solutions, Acids, Bases Notes
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F. Acid and Base Spills
 there are many uses for both acids and bases in our households and in
industry
 due to their __________________________________________________,
special care must be used when they are being _______________________
__________________________________________
 the two ways to deal with acid or base spills are:
1. ______________________: reduce the ______________________
by adding ____________________
2. _________________________________: you always use a
_______________________________________ for the
neutralization so you aren’t left with another hazardous situation
6.3 Acids, Bases and pH
A. Ion Concentration in Water
 the “self-ionization” of water is very ___________ (only 2 in 1 billion)
 the concentration of ___________________________________ and
_______________________________________ are _____________ and
_____________________ in _____________________________
[H3O+(aq)] =
[OH(aq)] =
B. The pH Scale
 in 1909, Soren Sorenson devised the concept of ___________________
 it is used because the [H3O+(aq)] is __________________________
Chemistry 20 Solutions, Acids, Bases Notes
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 at 25C (standard conditions), most solutions have a pH that falls between
___________ and __________
 it is possible to have a _____________ pH and a pH ________________
 it is a _______________________________ based on whole numbers that
are powers of 10
 there is a ________________________________________________ for
every change in ______ on the _______________________
eg) a solution with a pH of 11 is ______________________ times more basic
than a solution with a pH of 9
pH Scale
C. Calculating pH and pOH
***New sig dig rule: when reporting pH or pOH values, only the numbers to
the ____________________________________________ count as
significant
Try These:
Calculate the pH and use the correct number of significant digits.
1. [H3O+(aq)] = 1. x 1010 mol/L pH =
Chemistry 20 Solutions, Acids, Bases Notes
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2.
[H3O+(aq)] = 1.0 x 102 mol/L pH =
3.
[H3O+(aq)] = 6.88 x 103 mol/L pH =
4.
[H3O+(aq)] = 9.6 x 106 mol/L pH =
Example (a tough one!)
6.30 g of HNO3 is dissolved in 750 mL of water. What is the pH ?
Your Assignment: pgs 2-3
 just as ______ deals with _____________, _________ deals with
___________
***p just means log
 at SATP…__________________________
pH
pOH
 to calculate the _________, use the same formula as pH but substitute in
the _____________ :
pOH =  log[OH(aq)]
Chemistry 20 Solutions, Acids, Bases Notes
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Try These:
1.
[OH(aq)] = 1.0  1011 mol/L
pOH =
2.
[OH(aq)] = 6.22  102 mol/L
pOH =
3.
[OH(aq)] = 9.411  106 mol/L
pOH =
4.
[OH(aq)] = 2  106 mol/L
pOH =
Your Assignment: pgs 4-5
 you could also be given the pH or pOH and asked to calculate the
_______________________________________________________
 same new significant digit rule applies!
Try These:
Find the [H3O+(aq)] in the following solutions:
1. pH 4.0
[H3O+(aq)] =
2. pH 6.21
[H3O+(aq)] =
3. pH 13.400 [H3O+(aq)] =
4. pH 7
[H3O+(aq)] =
5. pOH 1.0
[OH(aq)] =
6. pOH 13.2
[OH(aq)] =
7. pOH 6.90
[OH(aq)] =
8. pOH 0.786 [OH(aq)] =
Chemistry 20 Solutions, Acids, Bases Notes
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9.
[H3O+(aq)]
4.0  106 mol/L
[OH(aq)]
pH
pOH
Acid/Base/Neutral
9.500
2.0  10
11
mol/L
10 mol/L
15.00
1.36
Your Assignment: pg 6-7
D. Measuring pH
 pH can be measured using :
1. ________________________________
2. ________________________________
Indicators
 an _______________________________________ is any chemical that
____________________________________ in an acidic or basic solution
 they can be ___________________________________________________
eg) ___________________________________________
 they can be _________________________
eg) _________________________________________________________
 they can be made from _____________________________________
eg) _________________________________________________________
 each indicator has a __________________________________ where it will
_____________________________
Chemistry 20 Solutions, Acids, Bases Notes
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 you can use _______________________________________ to approximate
the _______________________________________
Your Assignment: pg 8
pH Meters
 using a pH meter is the most ______________ way of measuring ________
 it has an ___________________ that compares the [H3O+(aq)] in the
solution to a _________________ and it will give a __________________
______________________ of the pH
E. Diluting an Acid or Base
 when you _______________________ to an ________________________,
you change the ________________________________________________
 diluting an acid will _________________________ the ________________
until a pH of _________ is reached
 diluting a base will ____________________ the _______________ until a
pH of _________ is reached
Your Assignment: pgs 9-10
Chemistry 20 Solutions, Acids, Bases Notes
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