Chapter 16
ACID/BASE CHEMISTRY
Types of Acids and Bases
1. Arrhenius
2. Brønsted-Lowry
3. Lewis
Arrhenius Acid and Base
-Acid
-increase H+ concentration
-Base
-increase OH- concentration
-Brønsted-Lowry
more developed
Acid
-proton donor
Base
-Proton acceptor
-Lewis Acid/Base
-Acid
-electron pair acceptor
-base
-electron pair donor
Strong acid/base completely ionizes
Weak acid/base only partially ionizes
Ionization of water:
involves the transfer of a proton from one water molecule to another to produce a OH- and H3O+
In pure water only a small amount of OH- and H3O+ at 25 ºC
[H3O+]=[OH-]=1.0x10-7M
Formula:
-Kw=(H)(OH)
-Kw=1.0x10^-14The Kw of water will always be 1.0x10-14
if you add more [H3O+] or [OH] the solution will balance out to 1.0x10-14
Buffers
buffered Solution is one that resists a change in its pH even when a strong acid or a base is added to it
presence of a weak acid and its conjugate base
-Multiplication-short cut for addition
-exponential-short cut for multiplication
-logarithmic-short cut for exponential
pH scale
-measures how acidic or basic
-basic is 7 and above
-7 is neutral
-acidic is 7 and below
pH=-log (OH or H)
Neutralization-adding acid and base together
What is the pH if the pOH was 6?
pH + POH = 14
pH +6 = 14
pH = 8 and would be basic
Practice with kw
-What will happen to the [H3O+] when you add HCl?
Answer= the [H3O+] will increase.
remember acids will always increase [H3O+]
What will happen to the [OH] when you add HCl?
Answer= the [OH-] will go down to balance out to 1.0x10-14
logs
When an equation is in the form x = b^y, it is in exponential form. If an equation is in the form y = logbx, it is in logarithmic form.
-the pH of a human blood sample was measured to be 7.41. What is the H+ in this blood?
pH=7.41
-pH=-7.41
H+= inverse log of -7.41 = 3.9 x 10^-8
H+= 3.9 x 10^-8 M
Types of Acids and Bases
1. Arrhenius
2. Brønsted-Lowry
3. Lewis
Arrhenius Acid and Base
-Acid
-increase H+ concentration
-Base
-increase OH- concentration
-Brønsted-Lowry
more developed
Acid
-proton donor
Base
-Proton acceptor
-Lewis Acid/Base
-Acid
-electron pair acceptor
-base
-electron pair donor
Strong acid/base completely ionizes
Weak acid/base only partially ionizes
Ionization of water:
involves the transfer of a proton from one water molecule to another to produce a OH- and H3O+
In pure water only a small amount of OH- and H3O+ at 25 ºC
[H3O+]=[OH-]=1.0x10-7M
Formula:
-Kw=(H)(OH)
-Kw=1.0x10^-14The Kw of water will always be 1.0x10-14
if you add more [H3O+] or [OH] the solution will balance out to 1.0x10-14
Buffers
buffered Solution is one that resists a change in its pH even when a strong acid or a base is added to it
presence of a weak acid and its conjugate base
-Multiplication-short cut for addition
-exponential-short cut for multiplication
-logarithmic-short cut for exponential
pH scale
-measures how acidic or basic
-basic is 7 and above
-7 is neutral
-acidic is 7 and below
pH=-log (OH or H)
Neutralization-adding acid and base together
What is the pH if the pOH was 6?
pH + POH = 14
pH +6 = 14
pH = 8 and would be basic
Practice with kw
-What will happen to the [H3O+] when you add HCl?
Answer= the [H3O+] will increase.
remember acids will always increase [H3O+]
What will happen to the [OH] when you add HCl?
Answer= the [OH-] will go down to balance out to 1.0x10-14
logs
When an equation is in the form x = b^y, it is in exponential form. If an equation is in the form y = logbx, it is in logarithmic form.
-the pH of a human blood sample was measured to be 7.41. What is the H+ in this blood?
pH=7.41
-pH=-7.41
H+= inverse log of -7.41 = 3.9 x 10^-8
H+= 3.9 x 10^-8 M
websites
This website classifies the difference between acids and bases.
This website helps students understand weak and strong acids.
This website explaining Arrhenius, Brønsted, and Lewis Acids and Bases.
This website further explains the ionization of water.
This website explains neutralization of water.
This website calculates and converts pH and pOH (calculating and converting)
This website explains and shows how to convert between H+ and OH-.
This website explains how logs function.
activities
This activity helps students apply their knowledge about pH and pOH.
This activity helps you apply your knowledge about converting between H+ and OH-.
This activity helps students practice examples with logs.
videos
This video classifies the difference between acids and bases.
This video shows and explains weak and strong acids.
This video explains Arrhenius, Brønsted, and Lewis Acid and Bases.
This video explains pH/pOH and OH-/H+.
This video explains and shows how logs work.