O 2 Flashcards
What does the bronsted Lowry theory state?
Acids are proton donors eg. NH4+
Bases are proton acceptors eg. OH-
When is a conjugate acid formed?
When a base accepts a proton
When is a conjugate base formed?
When an acid donate a proton
A - acids
B - conjugate base
C - base
D - conjugate acid
What is a strong acid?
An acid that completely dissociates into its ions when in solution
What is a strong base?
A base that completely dissociates into its ions when in solution
What is the pH of a strong acid?
Between 0 - 1
What is the pH of a strong acid?
Between 0 - 1
What is the pH of a weak acid?
3-7
What is the pH of a strong base?
12-14
What is the pH of a weak base?
7-11
What is the reacting ion (the ion in the ionic equation) in reactions of acids with carbonates, metal oxides and alkalis?
H+
What does the reaction of weak acids and bases have?
An acid dissociation constant (Ka)
What is the equation for Ka?
How can you find Ka?
What does a high Pa and low Kpa mean?
Strong acid
What does pH give?
The concentration of H+ ions in a solution
what does a pH of 0 mean?
Solution is acidic
High concentration of H+ ions
Equations which link pH and [H+]
What is [H+] equivalent to?
The concentration fo a strong acid
How do you calculate the pH of a strong base?
What is [OH-] in Kw = [OH-][H+]?
The same as the concentration of the base
What is Kw?
10 to the minus 14
When do you use Kw to find [H+], then pH?
When A- is in excess
When do you use [HA] and [A-] along with Ka to find [H+], then pH?
When HA is in excess
When is pKa equal to pH?
When HA = A-
What is Kw equation and when is it used?
Kw = [OH-] [H+]
When calculating the pH of a strong base
