Chemical Equillibria Part 2

Question 1

What are the 4 common acids?

Answer 1

HCl
H2SO4
HNO3
CH3COOH

Question 2

What are the 3 common alkalis?

Answer 2

NaOH
KOH
NH3

Question 3

What is the Brønsted-Lowry definitions of acids and bases?

Answer 3

Acid - proton donor
Base - proton acceptor (using a pair of electrons)
Strong acid/base - Fully dissociates in an aqueous solution
Weak acid/base - Partially dissociates in an aqueous solution

Question 4

Define monoprotic and diprotic acids.

Answer 4

Monoprotic Acid - donates one H+
Diprotic Acid - donates two H+

Question 5

Describe how to test acidity.

Answer 5

pH is related to [H+]
pH = 7 neutral
pH < 7 acidic
pH > 7 alkaline

Practical methods:
Conductivity
Reactions with Metals
pH meter
Universal indicator:
- Red = strong acid
- Orange = weak acid
- Green = neutral
- Blue = basic

Question 6

Describe the reactions with acids.

Answer 6

Mg + 4HNO3 -> Mg(NO3)2 + 2NO2 + 2H2O
Na2O + 2HCl -> H2O + 2NaCl
Na2CO3 + 2HCl -> 2NaCl + CO2 + H2O
2NaOH + H2SO4 -> Na2SO4 + 2H2O

Question 7

Define conjugate acid and base.

Answer 7

Conjugate base - forms when an acid loses an H+
Conjugate acid - forms when a base gains an H+

Example:
HCl + H2O -> H3O+ + Cl-
H3O+ is a Conjugate Acid
Cl- is a Conjugate Base