(Ch.14) Acids & Bases Flashcards
(25 cards)
What are the two primary definitions of Acids & Bases?
- The Arrhenius Definition
- The Bronsted-Lowry Definition
How does Arrhenius define acids and bases?
- An acid produces H+ ions in an aqueous solution.
- A base produces OH- ions in an aqueous solution.
How does Brownsted-Lowry define acids and bases?
- An acid is a proton donor.
(H+ ion donor) - A base is a proton acceptor.
(H+ ion acceptor)
What does it mean to be Amphoteric?
An amphoteric substance is a substance that can act as both an acid and a base. All conjugate acid-base pairs are amphoteric.
What are Conjugate Acid-Base pairs?
These are acid-base pairs that are, firstly, amphoteric, and secondly, they differ by one proton.
What is a Neutralization Reaction?
A reaction between an acid and a base.
What forms when:
1. Metal + Acid
2. Metal Oxide + Acid
- Gas + Salt
- Water + Salt
- What is a Strong Acid?
- What is a Weak Acid?
- An acid that completely ionizes in a solution.
- An acid that does not completely ionize in a solution.
How can you tell the difference between a Strong and Weak acid?
A weak acid is usually found in a reversible equation.
Strong Acids: HCl, HBr, HI, HNO3, NClO4, H2SO4
What is a Dissociation Reaction?
What is an Ionization Reaction?
How are they different?
- The separating of charged particles that already exist.
- Producing newly charged particles.
- What is a Strong Base?
- What is a Weak Base?
- A base that completely dissociates in a solution.
- A base that does not completely ionize in a solution.
How can you determine the difference between a Weak or Strong Base?
If the base starts with any element from the first two columns of the periodic chart- it is STRONG.
EX.
Determine the concentration of OH- in the following base solutions.
1. 0.25 M NaOH
2. 0.25 M NH3
3. 0.25 M Sr(OH)2
4. 1.25 M KOH
- [OH-]= 0.25 M (strong base)
- [OH-]< 0.25 M (weak base)
- [OH-]= 0.50 M (strong base & 2 OH-)
- [OH-]= 1.25 M (strong base)
EX.
Determine the concentration of H3O+ in each of the following acid solutions.
1. 0.50 M HCHO2
2. 1.25 M HI
3. 0.75 M HF
- [H30+]< 0.50 M (weak acid)
- [H30+]= 1.25 M (strong acid)
- [H30+]< 0.75 M (weak acid)
What do we mean when we say water is capable of Self-Ionization?
Water can be both a base and an acid and can react with itself to form low concentrations of the ions OH—and H3O+.
What is the ion product constant for water?
Kw= 1.0 (10^-14) at 25 degrees Celsius
What is a:
1. Neutral Solution
2. Acidic Solution
3. Basic Solution
- The ion product for both OH- and H3O+ is equal to 1.0 (10^-7)
- There is more H3O+ product than OH-.
- There is more OH- product than H3O+.
How do you calculate H3O+ concentration from pH?
How do you calculate pH from H30+ concentration?
- H30+ = 10^(-pH)
- pH= -log(H30+)
How do you determine the concentration of [H30+] given [OH-] or [OH-] given [H30+]?
- Use the solution:
[OH-][H30+]= 1.0 (10^-14)
Describe the pH scale.
Describe the pOH scale.
- (pH):
1-6.9 is acidic, 7 is neutral, 7.1-14 is basic - (pOH):
1-6.9 is basic, 7 is neutral, 7.1-14 is acidic
How would you calculate the [OH-] or [H30+] concentration given a solution’s pOH?
[OH-]= 10^-pOH
How would you calculate pOH given the [OH-] or [H3O+] concentration?
- pOH= -log[OH-]
- Determine [OH-] concentration from [H30+], then run it through the above equation to find pOH.
How would you determine the pH of a solution given the pOH? The pOH given the pH?
- The same, using the equation:
pH+pOH=14.00
What is:
1. pH =
2. pOH =
3. [H30+] =
4. [OH-] =
- -log[H30+]
- -log[OH-]
- 10(^-pH)
- 10(^-pOH)