5.1.3 - Acids, Bases & pH. Flashcards
What is a Brønsted-Lowry Acid?
A proton donor.
What is a Brønsted-Lowry Base?
A proton acceptor.
How are conjugate acid-base pairs related?
The conjugate acid donates a proton (H+) to make the conjugate base; the base accepts the proton (H+) to make the acid.
What is the Conjugate Base of these below?
* HNO3.
* H20.
* H2SO4.
* HCl.
- NO3-.
- OH-.
- HSO4-.
- Cl-.
What is the Conjugate Acid of these below?
* OH-.
* H20.
* SO42-.
* Br-.
- H20.
- H3O+.
- HSO4-.
- HBr.
Explain what each of the below are and give 1 example of each.
1. Monobasic Acid.
2. Dibasic Acid.
3. Tribasic Acid.
- An acid which only has 1 H+ ion to donate to its conjugate base (HCl).
- An acid which only has 2 H+ ions to donate to its conjugate base (H2SO4).
- An acid which only has 3 H+ ions to donate to its conjugate base (H3PO4).
What is the DEFINITION of a Weak Acid? Give a general equation for this?
- A weak acid only partially dissociates it’s H+ ions in aqueous solution.
- [HA] ⇌ [H+] + [A-] which leads to [H+] ∼ [A-].
What is the DEFINITION of a Strong Acid?
- A strong acid fully dissociates all of it’s H+ ions in aqueous solution.
- [HA] ∼ [H+].
Write the Ka expression for a general weak acid HA.
Ka = [H+][A-]/ [HA].
Which equation gives pH from [H+]?
pH = -log[H+].
Which equation gives pKa from Ka?
pKa = -log(Ka).
Which equation gives [H+] from pH?
[H+] = 10-pH.
What simplified Ka expression can we use for weak acids?
Ka = [H+]2/ [HA].
How does the simplified Ka expression Ka = [H+]2/ [HA] rearrange to solve for [H+]?
[H+] = √(Ka x [HA]).
What is the expression for the ionic product of water?
Kw = [H+][OH-].