A more rigorous theory of pH

Electroneutrality condition

Exercise 2

    

While taking into account the result of the water autoprotonation, write the electroneutrality condition of following mixtures of aqueous solutions:

a) Sodium chloride and calcium chloride

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

b) Sodium bromide and bromhydric acid

$[Na^+]$ $+$ $[H_3O^+]$ $=$ $[Br^-]$ $+$ $[OH^-]$

c) Ammonia and ammonium iodide

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

d) Phosphoric acid and iodhydric acid

$[H_3O^+]$ $=$ $[I^-]$ $+$ $[H_2PO_4^-]$ $+$ $2\;[HPO_4^{2-}]$ $+$ $3\; [PO_4^{3-}]$ + $[OH^-]$

e) Sulfuric acid and ammonium sulfate

$[NH_4^+]$ $+$ $[H_3O^+]$ $=$ $2\;[SO_4^{2-}]$ + $[OH^-]$ + $[HSO_4^-]$