Kc/Acids stuff Definitons Flashcards
The equilibrium law states that?
The equilibrium law states that for the equilibrium
aA + bB cC + dD
Kc = [C]^c[D]^d/[A]^a[B]^b
What is a dynamic equilibrium?
A dynamic equilibrium exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction.
What is a homogeneous equilibrium?
A homogeneous equilibrium is an equilibrium in which all the species making up the reactants and products are in the same physical state.
What is a heterogeneous equilibrium?
An equilibrium in which species making up the reactants and products are in different physical states.
What is a Bronsted-Lowry acid?
A Bronsted-Lowry acid is a proton, H+, donor.
What is a Bronsted-Lowry base?
A Bronsted-Lowry base is a proton, H+, acceptor.
What is an alkali?
An alkali is a base that dissolves in water forming OH-(aq) ions.
Neutralisation
Neutralisation is a chemical reaction in which an acid and a base react together to produce a salt and water.
An acid-base pair
An acid-base pair is a pair of two species that transform into each other by gain or loss of a proton.
pH?
pH = -log[H*(aq)]
A strong acid
A strong acid is an acid that completely dissociates in solution.
A weak acid
A weak acid is an acid that partially dissociates in solution.
The acid dissociation constant, Ka.
The acid dissociation constant, Ka, of an acid HA is defined as…
Ka = [H*(aq)][A-(aq)]/[HA(aq)
pKa?
pKa = -log Ka
The ionic product of water, Kw, is defined as?
Kw = [H*(aq)][OH-(aq)]
At 25*C, Kw = 1.00 x 10^-14 mol^2 dm^-6
A buffer solution
A buffer solution is a mixture that minimises pH changes
on addition of small amounts of acid or base.
The equivalence point
The equivalence point is the point in a titration at which the volume of one solution has reacted exactly with the volume of a second solution.
The end point
The end point is the point in a titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator.
The colour at the end point is midway between the colours of the acid and conjugate base forms.
The standard enthalpy change of neutralisation
The standard enthalpy change of neutralisation is the energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of H2O(l) under standard conditions.
