Acid & Base Notesheet
Name ___________________________________
15-1 Defining Acids and Bases
Period________Date_______________________
1. Properties of Acids and Bases:
Taste
Touch
Reactions with Metals
Electrical Conductivity
Acid
Base
2. Indicators: Turn 1 ___________________ in an acid and another color in a __________________.
A. Litmus Paper:
An aciD turns blue litmus paper _______
A Base turns red litmus paper ________.
B. Phenolphthalein:
C. pH paper:
D. pH meter:
3. Neutralization: A reaction between an ___________ and ___________. When an acid and base
neutralize, _________________ form. “Salts” are any _______________ compound
formed from the metal ______________ of the base and ____________ from the acid.
_______+ ______ → _______+ ______
Ex)
HCl
+ NaOH →
4. Arrhenius Definition:
A. An acid dissociates in water to produce ______________________, __________.
B. A base dissociates in water to produce _______________________, __________.
C. Problems with Definition:
•Restricts acids and bases to _______________ solutions.
•Oversimplifies what happens when ____________ dissolve in water.
•Does not include certain compounds that have characteristic properties of acids &
bases. Ex)
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5. BrØnsted-Lowry Definition:
A. An acid is a substance that can ____________ hydrogen ions. Ex)
B. A base is a substance that can _____________ hydrogen ions. Ex)
C. Advantages of BrØnsted-Lowry Definition
•Acids and bases are defined independently of how they behave in ____________.
•Focuses solely on __________________ ions.
D. Hydrogen ion is the equivalent of a ______________. Therefore, acids are often called
proton _________________ and bases are called proton _______________.
6. Hydronium Ion:
A. Hydronium Ion – H3O+ This is a complex that forms in water.
B. To more accurately portray the BrØnsted-Lowry, the _________________ ion is used
instead of the ________________ ion.
C. Amphoteric: A substance that can act as either an ___________ or a ____________.
Ex.)
7. Conjugate Acid-Base Pairs: A pair of compounds that differ by only one ____________________
A. When an acid loses a hydrogen ion, it becomes its ________________________________.
B. When an base gains a hydrogen ion, it becomes its ________________________________.
Ex.
NH3
____
+
H2O
____
↔
NH4+
____
+
OH____
HCl
____
+
H2O
____
↔
Cl____
+
H3O+
____
A strong acid will have a _____________ conjugate base.
A strong base will have a _____________ conjugate acid.
C. A strong acid or base will ______________________ _____________________(break
apart) in water. This is represented by a ___________________________ arrow.
Ex)
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D. A weak acid or base will _____________________ _____________________in water.
This is represented by a _____________________________________ arrow.
Ex)
8. Naming Acids Review Ch 7:
A. Binary – H + one anion
Prefix “hydro” + anion name + “ic” acid
Ex) HCl _________________________________
Ex)
_________
hydrophosphoric acid
B. Tertiary – H + polyatomic anion
no Prefix “hydro”
end “ate” = “ic” acid
end “ite” = “ous” acid
Ex) H2SO4 _______________________________
Ex)
_________
sulfurous acid
15-2 The Self-ionization of Water and pH
1. Water is amphoteric, it acts as both an acid and a base in the same reaction.
Ex)
H2O(l)
+
H2O(l)
↔
H3O+(aq) +
OH-(aq)
2. In pure water at 25C, both hydronium ions and hydroxide ions are found at concentrations of
_____________________. Because they are at ______________________ and you do not include
liquid water in the equilibrium expression, Keq or Kw (water) can be expressed as follows:
A. Formula for
Kw
=
[H3O+]
[OH-]
1.0 x 10-14M = [1.0 x 10-7M] [1.0x10-7M]
1.0 x 10-14M = [H3O+] [OH-]
B. Using Kw in calculations: If the concentration of H3O+ in the blood is 4.0 x 10-8 M, what is
the concentration of OH- ions in the blood? Is blood acidic, basic
or neutral?
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3. The pH scale:
A. Used to determine if something is an ___________ or a ____________. A way to express
_________ concentration based on logarithms. pH changes by a factor of ______.
Ex)
10,000 = ________
therefore
log 10,000 = ______
0.001 = ________
therefore
log 0.001 = ______
B. pH 1- 6.9:
pH 7.1-14:
pH of 7.0:
_________
_________
_________
C. Copy the pH scale:
pH
[H3O+]
sci. not.
decimal
[OH-]
OH-
D. pH = -log [H3O+]
E. [H3O+] [OH-] = 1.0 x 10-14M
F. pH + pOH
= ______
H3 O+
H. Significant Digits Rule: The number of digits after the decimal point in your answer should
be equal to the number of significant digits in your original number.
Ex) –log[8.7 x 10-4 M] Calculator Answer = 3.060480747 Sig. Fig. pH = 3.06
Ex #1) [H3O+] = 7.3 x 10-5 M What is the pH value? Is it an acid, base or neutral?
Ex #2) [OH-] = 5.0 x 10-2 M
What is the pH value? Is it an acid, base or neutral?
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Ionization of Acids & Bases:
•
H2SO4  2 H+ + SO4-2
•
H3PO3 
•
Ca(OH)2 
~Sulfuric acid donates 2 H+ ions per mole. _____________ acid
15-3 Acid-Base Titration
1. An acid-base titration is a carefully controlled ____________________________ reaction which
can determine the ________________________________ [ ] of an unknown solution.
2. To determine the concentration of an unknown substance, a ________________________________
is needed. This solution has a ____________________ concentration.
3. An indicator, usually ___________________________________, is used in a titration.
4. The point at which enough standard solution is added to neutralize the unknown solution is called
________________________________ ________________________.
5. The point at which the indicator changes color is called the ________________________________.
6. Therefore: [H3O+] = [OH-] at the equivalence point (which is usually the endpoint)
Volume (acid) Conc.(acid) = Volume (base) Conc.(base)
VaMa = VbMb
Ex #1) Solutions of sodium hydroxide are used to unclog drains. A 43.0 mL volume of sodium
hydroxide was titrated with 32.0 mL of 0.100 M hydrochloric acid. What is the
molarity of the sodium hydroxide solution? Write the equation first:
______________ + ______________ → ______________ + ______________
ACID
BASE
SALT
WATER
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Ex #2) A volume of 25.0 mL of 0.120 M sulfuric acid neutralizes 40.0 mL of a sodium hydroxide
solution. What is the concentration of the sodium hydroxide solution? Write the equation first.
Ex #3) 24.9 mL of 2.88 M calcium hydroxide completely neutralizes 38.9 mL of a hydrobromic acid
solution. What is the molarity of the hyrdobromic acid? Write the equation first.
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