Name ________________________________________________
Topic
10
ESSENTIAL QUESTION:
How do the properties and interactions of acids, bases, and salts affect
our physiology and our environment?
Properties of Acids and Bases
Acids and Bases can be identified by observable characteristic _____________________________.
Characteristic Properties of Acids:
1. Dilute acids taste ____________________.
Examples: _______________________________________________________________________
2. Aqueous solutions of acids _____________________________ electric current.
a. Electrolyte: ______________________________________________________________________
b. depends on ________________________________
c. strong acid: ______________________________________________________________________
d. weak acid: _______________________________________________________________________
3. Acids react with ______________ to form _________________ and _____________ .
a. neutralization: ____________________________________________________________________
b. Neutralization is a __________________ _______________________________ reaction!
4. Acids react with certain ___________________ to produce ____________________ ____________ .
a. All metals ___________ H2 on Table J will react with acids to form ___________________ ___________
5. Acids cause acid-base _______________________ to change _______________ .
Reference
Table M
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Characteristic Properties of Bases
1. Bases taste _____________________________ .
2. Bases feel _____________________________________ .
3. Bases _________________________ an _________________________ current.
a. Strong base: _____________________________________________________________________
b. weak base: ______________________________________________________________________
4. Bases react with ____________________ to form _____________________ and __________________.
5. Bases cause ___________________________________________ to change color.
Reference
Table M
Arrhenius Theory
Arrhenius acid: ___________________________________________________________________________
example:
Are all substances that contain hydrogen an acid? ___________
example: ________________________________________________________________________
The Nature of the Hydrogen Ion
Draw a Bohr model for hydrogen:
2
Describe a hydrogen ion using one word: __________________
Draw a hydronium ion and write its formula:
How does a hydronium ion form?
According to the Arrhenius theory, what causes the characteristic properties of acids?
monoprotic acid: ________________________________________________________________________________
ex.) _________________________________________
diprotic acid: ___________________________________________________________________________________
ex.) _________________________________________
triprotic acid: _____________________________________________________________________________________
ex.) _________________________________________
The Nature of the Hydroxide Ion
According to Arrhenius’ theory, what is responsible for the characteristic properties of bases?
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Write the formula for ammonia: ____________
Is ammonia a base? ____________
Explain where ammonia’s hydroxide ion comes from:
What are amines? _______________________________________________________________________
Are amines bases? _____________
Explain how amines form hydroxide ions:
What is a hydroxyl group? __________________________________________________________________
What does a hydroxyl group look like? __________________________________________
What is the name of compounds that contain a hydroxyl group? ___________________________________
They are _______electrolytes and do NOT ionize to produce _____________________ when dissolved in water.
Strength of Acids and Bases
Name a strong, harmful acid: ____________________
Name a harmless acid: _______________________
Explain why some acids are stronger than others:
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Naming Acid and Bases
Binary acids: _____________________ and _______________________________________
names begin with _______________ and end with _________________________________________
Ternary acids: contain a _________________ __________ containing ___________________
If the polyatomic ion ends in –ate, then the acid ends in ____________
If the polyatomic ion ends in –ite, then the acid ends in ____________
Practice: (Use Reference Table E)
HCl
____________________________________
HNO2
____________________________________
HNO3
____________________________________
H2SO3
____________________________________
H2SO4
____________________________________
H3PO4
____________________________________
H2CO3
____________________________________
HC2H3O2
____________________________________
CH3COOH
____________________________________
Now look at Reference Table K.
Bases are quite simple to name . . . . . .
Keep the name of the positive ion, and end with “hydroxide”.
Practice:
NaOH
_____________________________________
Ca(OH)2
_____________________________________
KOH
______________________________________
NH4OH
______________________________________
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Name ________________________________________________
Topic
10
Reactions Involving Acids and Bases
Reactions of Acids with Metals
Which metals will react with acids?
Which metals will not react with acids?
Which type of reaction occurs when acids react with metals? __________________________________
What gas is released when acids react with metals? _____________________________
Neutralization Reactions
In a neutralization reaction,
a __________________________ reacts with a __________________________
to produce a ____________________ and ____________________ .
What are spectator ions?
Omitting the spectator ions yields the net ionic equation:
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Neutralization reactions are __________________ ________________________________ reactions!

Remember the general formula for double replacement reactions:
AB + CD  AD + CB

Then remember to balance the equation!
Write the neutralization reaction for nitric acid and potassium hydroxide:
Write the neutralization reaction for hydrochloric acid and sodium hydroxide:
Write the neutralization reaction for hydrochloric acid and sodium hydroxide:
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Name ________________________________________________
Topic
10
Acid – Base Titrations
Titration: ________________________________________________________________________________________

 When you know the ___________________ of either the acid or the base,
and you know the ___________________________ of both solutions used for neutralization,
 then you can calculate the unknown _________________________ .
molarity of acid x volume of acid = molarity of base x volume of base
MA x VA = MB x VB
Volumes do NOT need to be converted to L. Leave as mL.
When you calculate the molarity of a diprotic acid (ex. H2SO4), divide your answer by 2.
When you calculate the molarity of a triprotic acid (ex. H3PO4), divide your answer by _______.
When you calculate the molarity of a dihydroxy base (ex. Ba(OH)2), divide your answer by ______ .
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Practice:
For the titration:
KOH + HCl  H2O + HOH
How many milliliters of 2.0M KOH are necessary to neutralize 50.0 mL of 1.0M HCl?
Write the equation AND show your work:
:
10.0 mL of hydrochloric acid neutralizes 15.0 mL of a 0.40M solution of NaOH.
What is the molarity of the hydrochloric acid?
Write the equation AND show your work:
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Name ________________________________________________
Topic
10
Acidity and Alkalinity of Solutions
Although water is covalently bonded, it does slightly separate into ions:
HOH  H+ + OHNotice that this is an ____________________________ reaction.
According to LeChatelier’s principle,


adding H+ will ____________________ the concentration of OH-.
adding OH- will ____________________ the concentration of H+.
A solution is acidic when ____________________________________________________________________________
A solution is basic (alkaline) when _____________________________________________________________________
pH Scale
The pH scale expresses the concentration of __________ .
pH is a logarithmic. Each increment is a _________________ increase or decrease in concentration.
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Acid-Base Indicators
Indicator: _________________________________________________________________________________________
Copy Reference Table M:
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Why is phenolphthalein used for titrations?
What do you see at the exact endpoint of a titration using phenolphthalein?
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Name ________________________________________________
Topic
10
Bronsted-Lowry Acids and Bases
According to this definition, an acid is ___________________________________________________________________
According to this definition, a base is ____________________________________________________________________
How does the Bronsted-Lowry theory differ from the Arrhenius theory?
Conjugate Acid-Base Pairs
When a substance donates a proton, another substance must _________________________________.
Examples of a conjugate pair:

HNO3 is an acid. When it donates a proton, ___________ is left. That makes _______ a base because now it can
accept a proton.

HCl is an ____________. When it donates a proton, _______ is left. _______ counts as a base because now it
can accept a proton.
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