Chapter 16
Types of Acids and Bases:
1. Arrhenius
2.Bronsted-Lowry
3.Lewis
1. Arrhenius Acids and Bases
2. Bronsted-Lowry Acids and Bases
3. Lewis Acids and Bases
Strong Acid and Base - will completely ionize (it will completely break into ions)
Weak Acid and Base - will partially ionize
Ionization of Water
Ion - Product Constant
What will happen to the [H3O+] when you add HCl? The [H3O+] will increase
Acids will always increase [H3O+]
What will happen to the [OH-] when you add HCl? The [OH-] will go down to balanace out to 1.0*10^-14
Understanding Logarithmic Function
http://www.youtube.com/watch?v=Z4iWJ39EC1g - Video on Logs
http://www.purplemath.com/modules/logrules.htm - website on logs
http://www.youtube.com/watch?v=sB1JTTOCtJc - video on kw
http://ebookily.org/pdf/ph-scale-worksheet - pH activity
To cancel a log, you have to raise everything by the base value
pH = -log[H3O+]
pH + pOH = 14
Neutralization reaction - when you add an acid and a base together
Buffered solution - one that resists a change in its pH even when a strong acid or a base is added to it; in the presence of a weak acid and its conjugate base
Characteristics of a Buffer
Weak Acids
1. Arrhenius
2.Bronsted-Lowry
3.Lewis
1. Arrhenius Acids and Bases
- Acid - any compound that increases H+ (H3O+) concentrations
- Base - Any compound that increases [OH-} concentrations
2. Bronsted-Lowry Acids and Bases
- A more developed idea of Arrhenius Acids and Bases concept
- Acid - Proton donor (H+)
- Base - Proton Acceptor
- An acid always forms a conjugate base
3. Lewis Acids and Bases
- Acid - electron pair acceptor
- Base - electron pair donor
Strong Acid and Base - will completely ionize (it will completely break into ions)
Weak Acid and Base - will partially ionize
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 25C
- [H3O+] = [OH-] = 1.0*10^-7
Ion - Product Constant
- Kw is called the ion product constant of water
- Kw = [H3O+][OH-] = 1.0 * 10^-14
What will happen to the [H3O+] when you add HCl? The [H3O+] will increase
Acids will always increase [H3O+]
What will happen to the [OH-] when you add HCl? The [OH-] will go down to balanace out to 1.0*10^-14
Understanding Logarithmic Function
- Multiplication - short cut for addition
- Exponential - short cut for multiplication
- Logarithmic - short cut for exponential
http://www.youtube.com/watch?v=Z4iWJ39EC1g - Video on Logs
http://www.purplemath.com/modules/logrules.htm - website on logs
http://www.youtube.com/watch?v=sB1JTTOCtJc - video on kw
http://ebookily.org/pdf/ph-scale-worksheet - pH activity
To cancel a log, you have to raise everything by the base value
pH = -log[H3O+]
pH + pOH = 14
Neutralization reaction - when you add an acid and a base together
Buffered solution - one that resists a change in its pH even when a strong acid or a base is added to it; in the presence of a weak acid and its conjugate base
Characteristics of a Buffer
- The solution contains a weak acid and its conjugate base
- Resists change in pH by reacting with any added hydrogen ion or hydroxide ion so that these ions do not accumulate
Weak Acids
- Acetic Acid
- Hydrofluoric Acid
- Hydrocyanic Acid
- Formic Acid