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A more rigorous theory of pH

Electroneutrality condition

Exercise 1

While taking into account the result of the water autoprotonation, write the electroneutrality condition of an aqueous solution of

a) Potassium chloride

$[K^+]$ $+$ $[H_3O^+]$ $=$ $[Cl^-]$ $+$ $[OH^-]$

b) Magnesium bromide

$2\;[Mg^{2+}]$ $+$ $[H_3O^+]$ $=$ $[Br^-]$ $+$ $[OH^-]$

c) Lithium sulfate

$[Li^+]$ $+$ $[H_3O^+]$ $=$ $2\; [SO_4^{2-}]$ $+$ $[OH^-]$

d) Ammonia

$[NH_4^+]$ $+$ $[H_3O^+]$ $=$ $[OH^-]$

e) Ammonium chloride

$[NH_4^+]$ $+$ $[H_3O^+]$ $=$ $[Cl^-]$ $+$ $[OH^-]$

f) Potassium oxide

$[K^+]$ $+$ $[H_3O^+]$ $=$ $[OH^-]$

g) Diluted sulfuric acid (successive dissociations!)

$[H_3O^+]$ $=$ $2\; [SO_4^{2-}]$ $+$ $[HSO_4^-]$ $+$ $[OH^-]$

g) Calcium hydroxide

$2\; [Ca^{2+}]$ $+$ $[H_3O^+]$ $=$ $[OH^-]$