Titanium dissolves rapidly in hydrofluoric acid according to the reaction:
2normalTi+6HF→2TiF3+3H2
. The formation of the trifluoride was confirmed by titration with potassium permanganate solution and by measurement of the volume of hydrogen evolved. The rate of dissolution,
V
, of titanium in hydrofluoric acid of concentrations between 0.02N and 0.2N conforms with the empirical equation:
V=459N2/3 mm3/cm2min
. For the acid between 0.2N and 10N the equation becomes
V=88+473N mm3/cm2min
. Metal salts added to the acid during the dissolution of titanium increased the rate in the following order : Fe2+, Ni2+, Ag+, Cu2+, Au3+, Pt4+, that is, nearly the order of decreasing overvoltage of the corresponding metals. Mg2+ proved to be inactive while Pb2+ hampered the dissolution reaction. The open‐circuit potential of titanium became more anodic as the concentration of hydrofluoric acid varied from 0.0125N to 0.2N. The potential remained practically constant with concentrations higher than 0.2N (−0.768 volt, hydrogen scale). A visible grayish blue film was formed on titanium in concentrations below 0.5N. The dissolution of titanium in hydrofluoric acid is probably an electrochemical process, based on the activity of local elements.