TOPIC 12 - Acid-base equilibria
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What is a Bronsted-Lowry acid?
A proton donor
Do actual H+ ions really exist in solution?
No. They tend to form hydroxonium ions. (H3O+)
What is a Bronsted-Lowry base.
Proton acceptor
What is the general equation for the reaction between an acid and water?
What is the general equation for the reaction between an alkali and water?
What is the difference between strong bases/acids and weak bases/acids?
Weak base/acid dissociate partly while strong bases/acids dissociate completely.
What is the conjugate acid of a base?
The species of a base with an added proton.
What is the conjugate base of an acid?
The species of that acid without the proton.
What is the conjugate base of HA?
A-
What is the conjugate acid of B?
BH+
What is the conjugate acid of H2O?
H3O+
What is the conjugate base of H2O?
OH-
What do acids and bases give when they react together?
Salt + Water.
What is the equation for the reaction between NH3 with H2O?
What is the equation for the reaction between ammonia and sulfuric acid?
What isthe standard enthalpy change of neutralisation?
Is the standard enthalpy of neutralisation normally endothermic or exothermic?
exothermic
Why does enthalpy of neutralisation vary with different weak acids/bases?
• Energy released by OH- and H+ is the same. • However weak acids and bases are constantly dissociating during neutralisation due to equilibrium) and energy needed to dissociate different weak bases/acids varies.
Why does the enthalpy of neutralisation of strong acids/bases
• Strong acids and bases are already fully dissociated in solution so no energy is needed. • The OH- + H+ enthalpy is the same.
What is the equation for pH?
What is a polyprotic / polibasic acid?
Acids that have more than one proton (diprotic, triprotic etc.)
What assumption is made when calculating the pH of strong acids/bases?
They dissociate fully. (i.e. [HA] = [H+] )
What is Kw?
Ionic product of water. (1.0x10^-14 under standard conditions)
