Equilibria
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17 Terms
What is Brownsted-Lawry acid?
A proton donor
What is a Brownsted-Lawry base?
A proton acceptor
What is strength in terms of acids and bases?
The extent or degree of ionisation
What does ‘concentration’ mean when dealing with acids and bases?
The number of moles of a solute in one dm3 of the solution
What is Kw and give the equation?
The ionic product of water
Kw = [H+][OH-]
What is pH?
The negative log to the base ten (-log10) of H+ ions
What is Ka? Give the equation
The equilibrium constant for an acid
Ka = [H+][A-]/[HA]
How do you find pKa, give the equation?
pKa= -log10(Ka)
What are the assumption for when calculating the pH of strong acid?
The acid is fully dissociated
The concentration of HA at equilibrium is the same as the concentration of H+
List examples of diprotic acids
H2SO4
H2S
H2CO3
What are the assumptions when calculating the pH of strong bases?
Fully dissociates
The concentration of the strong acid is the same as the OH- ions
Use Kw
How do you know how strong an acid is when using Ka?
The larger the Ka the stronger the acid, the lower the Ka the weaker the acid.
The opposite for pKa
What are the are the assumptions when calculating the pH of a weak acid?
Partially dissociates
Equilibrium concentration of the acid at the end is the same as the acid at the start
At all times given times the concentration of the ions is always equal
Use Ka
What is a buffer?
A solution that resists changes in pH when small amounts of acids or bases are added
What is the definition of Ksp?
It is the equilibrium constant that related to the product of the concentration of ions of a sparingly soluble salt is raised to their stoichiometric coefficients
What is the common ion effect?
The reduction in solubility of a sparingly soluble salt when a compound with an ion in common with sparingly soluble salt is added
What is Kpc?
The equilibrium constant that related to the concentration of solute partition (splitting) between two immiscible liquids at a particular temperature