“…However, the special, isohydricity property is attributed here to solutions of two different acids, A 1 and A 2 , or two different bases, B 1 and B 2 , having equal pH values, i.e., the term "isohydric" refers to solutions of the same hydrogen-ion concentration, [H +1 ]. After Arrhenius, such a pair of solutions is termed as isohydric solutions [3,4].However, the Arrhenius' statement [5], expressed in more contemporary terms, as "if two solutions of the same pH are mixed, pH of the mixture is unchanged, regardless the composition of the solutions" [6], is not true, when referred to any pair of electrolytic systems.As an example [7], let us take the pair of solutions: C 1 = 10 -2.5 ≈ 0.003 mol/L HCN and C 2 = 1 mol/L AgNO 3 .From the approximate formulae: [H +1 ] = (C 1 ⋅ K 1 ) 1/2 for HCN (C 1 ) and [H +1 ] = (C 1 ⋅ K 1 oH ⋅KW) 1/2 for AgNO 3 (C 2 ) we get pH=5.85, for both solutions; [AgOH] = K 1 OH [Ag +1 ][OH -1 ]), logK 1 OH = 2.3; [H +1 ][CN -1 ] = K 1 [HCN], pK 1 = 9.2; K W =[H +1 ][OH -1 ], pK W = 14. However, as were stated in [8], Ag +1 ions when added into HCN solution act as a strong acid generating protons, mainly in the complexation reaction Ag +1 + 2HCN = Ag(CN) 2 -1 + 2H +1 , and pH of the mixture drops abruptly.…”