Chapter 20 (Acids, Bases + pH)
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Equation for dissociation in strong acids
HA(aq) –> H+(aq) + A-(aq) Acid fully dissociates in aqueous solution
Assumptions that can be made in the dissociation of a strong acid
Since a strong acid fully dissolves in a solution, [H+]= [HA]
Equation of the dissociation of a weak acid
HA(aq) <=> H+(aq) + A-(aq)
What is Ka and how do you calculate it
Dissociation constant (only in equilibria) Ka= ([H+]+ [A-]) / [HA]
Assumption in dissosiation of weak acid
[H+] = [A- ] [HA]eql =[HA]start -> very weak acid dissociation negligible (eql lies on left) So Ka= [H ]² / [HA]start P
% dissosiation of weak acids
%= 100* ([H+]eql / [HA]start) Or nH+ and nHA as long as they are both in the same units
Equation of ionisation of water
H2O + H2O <=> H3O+ OH- A1 B2 A2 B1