Acid-base equilibria Flashcards
(20 cards)
What is the Bronsted-Lowry acid
give an example
A proton donor
HCl because it donates a proton to H2O
Give an example of a Bronsted-Lowry acid:
a) monobasic
b) Dibasic
c) Tribasic
a) HCl
b) H2SO4
c) H3PO4
Why are acids put in categories such as monobasic
depends on how many protons they can donate
What is a Bronsted-Lowry base
Give an example
Proton acceptor
NH3 because it accepts a proton from H20
Give an example of a Bronsted-Lowry base:
a) Monobasic
b) Dibasic
c) Tribasic
a) NH3
b) CO3 2-
c) PO4 3-
When is a conjugate base of acid formed
When an acid donates a proton
When is conjugate acid of a base formed
When a base accepts a proton
What is an Amphoteric substance
Give an example
Can act both as an acid and as a base
Water
What is a strong acid
give an example
Fully dissociates in solution
HCl
What do you assume when you calculate the pH of a strong acid
.For a monobasic acid [H+] = acid
What is a weak acid
Give an example
Only partially dissociated in solution
Ethanoic acid
What do you need to take into account when calculating the pH of a weak acid
The acid dissociation constant, Ka
What is an acid dissociation constant
Ka
What happens the lower the Ka value
The weaker the acid
What is the ionic product of water
Kw
What is a buffer solution
It minimises the changes in pH when small amounts of acid or base are added to it
What is the pH of an acid buffer solution
pH < 7
How are acid buffers made
By mixing a weak acid with a salt of its conjugate base
What is the pH of a basic buffer solution
pH > 7
How are basic buffers made
By mixing a weak base with a salt of its conjugate acid
