How far? Flashcards
What factor is Kc and Kp affected by?
Change in reaction temperature.
Not affected by concentration or pressure change or by the use of a catalyst.
What is a Bronsted-Lowry acid?
A species that donates a proton
E.g. ammonium ions
What is bronsted-Lowry base?
A species that accepts a proton
E.g. hydroxide ions
What is a conjugate acid?
The species formed when a base accepts a proton
E.g. ammonia becomes ammonium ion
what is a conjugate base?
Species formed when an acid donates a proton
E.g. HCl forms Cl- ion.
What is a strong acid?
An acid that completely dissociates into its ions when in solution
What is a weak acid?
An acid that partially dissociates into its ions when in solution.
The definaitions are the same for weak and strong bases
What is a monobasic acid?
An acid which only has one proton that they can release into solution.
Such as HCl and HNO3
An acid which only has one proton that they can release into solution.
What is a dibasic acid and give an example?
can release 2 protons into solution
H2SO4
What is a Tribasic acid and give an example?
can release three protons into solution
H3PO4
What is the relationship between PKa and Ka?
PKa is a logarithmic acid dissociation constant, representing how acid something is.
PKa = -log10 (ka).
Ka = 10^-pka
How sis the acid dissociation constant worked out from
HA ⇌ H+ + A-
Ka = (H+)(A-) / (HA)
These are square brackets
How do i workout pH from H+?
pH = -log(H+)
Square brackets
How do i wok out H+ from pH?
(H+) = 10^-pH
What is a buffer solution?
A solution which is able to resist changes in pH when small volumes of acid or base are added.
how is a buffer solution formed?
From a weak acid and its salt.
Or
An excess of a weak acid and a strong alkali.
How to do a buffer calculation when it’s an acid + base?
Find number of moles of each species
Calculate their concentration when at equilibrium using the total volume.
Use Ka to find (H+) and therefore pH
How to do a buffer calculation with an acid + salt?
Find the moles of the salt
Use Ka to fine pH
Explain how blood Ph is controlled by the carnbonic acid-hydrogencarbonate buffer system.
The pH of human blood is maintained in a buffer between carbonic acid and hydrogencarbonate ions. These ions neutralise any acidic substances that enter the bloodstream, converting them to carbonic acid and water. This buffer is present in blood plasma maintains a pH between 7.35 and 7.45.
