A. Major Points and Concepts
Types of Acids and Bases
1. Arrhenius
2. Bronsted-Lowry
3. Lewis
Arrhenius Acid and Base
Acid- Any compound that increase H+ (H3O+) concentration
Base- Any compound that increase (OH-) concentration
Bronsted-Lowry Acid and Base
A more developed idea of Arrhenius Acid and Base concept
Acid-Proton Donor (H+)
Base- Proton Acceptor
Lewis Acid/base
Acid
Electron pair acceptor
Base
Electron pair donor
Strong vs. Weak acid/base
Strong Acid and Base
will completely ionized
meaning will completely break into ions
Weak Acid and Base
will partially ionized
meaning will sometime break into ions
Strong Acids
HCl
HBr
HI
H2SO4
HNO3
HClO4
Strong Base
Any elements from IA or IIA that forms a compound with hydroxide (OH-)
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 degree C
Ion-product Constant
Kw is called ion product constant of water
units are customarily omitted
Kw=(1.0x10^-7)(1.0x10^-7)
Kw=1.0 x 10^-14
Kw
The Kw of water will always be 1.0 x 10^-14
If you add more H+ or OH- the solution will balance out to 1.0x10^-14
Understanding Logarithmic function
Multiplication=short cut for addition
exponential=short cut for multiplication
Logarithmic=short cut for exponential
Logs
y=logb^x
Log Rules
1. Inverse properties: loga a^x=x and a^(loga x)=x
2. Product: loga (xy)=loga x + loga y
3. Quotient: loga x/y)=loga x -loga y
4. Power: loga (xp)=p loga x
Application
One application of logarithms is in measuring the magnitude of an earthquake.
If an earthquake has a shock wave T times greater than the smallest shock wave that can be measured on a seismograph, then the magnitude M of the earthquake, as measured on the Richter scale, is given by the formula
M = log10 T
(When we talk about the size of a shock wave, we are talking about its amplitude. The amplitude of a wave is half the difference between its highest point and its lowest point.)
Chemistry Application
pH scale
this scale measures how acidic or basic is a solution
Calculating pH
pH=-log (?) ? represents of H or OH
Converting pH and pOH
pH+pOH=14
1. Arrhenius
2. Bronsted-Lowry
3. Lewis
Arrhenius Acid and Base
Acid- Any compound that increase H+ (H3O+) concentration
Base- Any compound that increase (OH-) concentration
Bronsted-Lowry Acid and Base
A more developed idea of Arrhenius Acid and Base concept
Acid-Proton Donor (H+)
Base- Proton Acceptor
Lewis Acid/base
Acid
Electron pair acceptor
Base
Electron pair donor
Strong vs. Weak acid/base
Strong Acid and Base
will completely ionized
meaning will completely break into ions
Weak Acid and Base
will partially ionized
meaning will sometime break into ions
Strong Acids
HCl
HBr
HI
H2SO4
HNO3
HClO4
Strong Base
Any elements from IA or IIA that forms a compound with hydroxide (OH-)
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 degree C
Ion-product Constant
Kw is called ion product constant of water
units are customarily omitted
Kw=(1.0x10^-7)(1.0x10^-7)
Kw=1.0 x 10^-14
Kw
The Kw of water will always be 1.0 x 10^-14
If you add more H+ or OH- the solution will balance out to 1.0x10^-14
Understanding Logarithmic function
Multiplication=short cut for addition
exponential=short cut for multiplication
Logarithmic=short cut for exponential
Logs
y=logb^x
Log Rules
1. Inverse properties: loga a^x=x and a^(loga x)=x
2. Product: loga (xy)=loga x + loga y
3. Quotient: loga x/y)=loga x -loga y
4. Power: loga (xp)=p loga x
Application
One application of logarithms is in measuring the magnitude of an earthquake.
If an earthquake has a shock wave T times greater than the smallest shock wave that can be measured on a seismograph, then the magnitude M of the earthquake, as measured on the Richter scale, is given by the formula
M = log10 T
(When we talk about the size of a shock wave, we are talking about its amplitude. The amplitude of a wave is half the difference between its highest point and its lowest point.)
Chemistry Application
pH scale
this scale measures how acidic or basic is a solution
Calculating pH
pH=-log (?) ? represents of H or OH
Converting pH and pOH
pH+pOH=14