(1) Acids and Bases Flashcards
Write the products of the following reactions:
Acid + Metal –>
Acid + Metal Oxide –>
Acid + Metal Hydroxide –>
Acid + Metal Carbonate –>
Acid + Metal –> Salt + Hydrogen
Acid + Metal Oxide –> Salt + Water
Acid + Metal Hydroxide –> Salt + Water
Acid + Metal Carbonate –> Salt + CO2 + Water
Write the formula, ions and charges of the following acids:
Hydrochloric
Sulfuric
Nitric
Phosphoric
Ethanoic
Hydrochloric - HCl (Cl-)
Sulfuric - H2SO4 (SO4 2-)
Nitric - HNO3 (NO3 -)
Phosphoric - H3PO4 (PO4 3-)
What is a Bronsted-Lowry Acid?
An ACID is a proton donor (H+).
What are Monoprotic and Diprotic Acids?
Monoprotic acid - releases ONE H+ ion
Diprotic acid - releases TWO H+ ions
What is a Bronsted-Lowry Base?
A BASE is a proton acceptor
OH-, NO3-, NH3-
HNO3 + H2SO4 –> H2NO3+ + HSO4-
Which is base and which is acid?
H2SO4 is an acid as it loses an H+
HNO3 is a base as it gains an H+
Define Amphoteric.
A substance that can act as both an acid and a base.
e.g. water
What are the formulas to find pH and [H+]?
pH = -Log10[H+]
[H+] = 10-pH
Key points about pH scale?
- smaller pH = greater [H+]
- A difference of 1 on the pH scale means a 10x difference in [H+]
Define a Strong Acid and give examples.
A STRONG acid FULLY DISSOCIATES
- HCl, H2SO4, HNO3, H3PO4
What do you have to make sure to do when the acid in the question is diatomic?
- make sure you times the concentration of [H+] by 2
Define a Weak Acid.
A WEAK acid only PARTIALLY DISSOCIATES
How can you find the pH of a Weak Acid?
Ka = [H+][A-]
[HA]
Which can be written as …
Ka = ___[H+]2 __
[HA]
Rearrange to find [H+] ….
SQUARE ROOT of Ka x [Weak Acid]
What is the formula for pKa?
pKa = -Log10Ka
Ka = 10-pKa
The stronger the acid = lower the pKa value.
Define a Buffer.
A BUFFER = weak acid and salt.
Define an Acidic Buffer.
An ACIDIC BUFFER is made of a weak acid and a soluble salt of that acid. It maintains a pH below 7.