A2 OCR Chemistry: Acid and Bases

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Emily Summers
Acids and Bases
Acid Proton donor
Base Proton acceptor
Acids with Metals
Mg(s) + 2H+(aq) H2(g) + Mg2+(aq)
Acids with Carbonates
CO32-(aq) = 2H+(aq) H2O(l) + CO2(g)
Acids with Alkalis
H+ + OH- H2O
Acids with Bases
2H+(aq) + O2- H2O(l)
An acid base pair is a pair of two species that transform into each other by gain or
loss of a proton
A strong acid will dissociate fully in solution, whereas a weak acid only partially
dissociates in solution- setting up a reversible reaction, the same goes for bases.
Ka shows the extent of acid dissociation.
Ka = [H+][A-]/[HA]
pH = ­log[H+] for pH of strong acids
[H+] = 10­pH
Converting between pKa and Ka
pKa = -logKa the larger the value the weaker the acid
Ka= 10-pKa the larger the value the stronger the acid
The Ionic Product of Water
Kw = [H+][OH-] 1.0 x 10-14

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Emily Summers
Buffer Solutions
A buffer solution is a mixture that minimises change to pH on addition of small
volumes of acid or base.
A buffer solution can be made from a weak acid and a salt of the weak acid, e.g.
CH3COOH/CH3COONa.…read more

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Emily Summers
Phenolphthalei Colourless 8.…read more


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