The dissolution of nickel ferrite in oxalic acid and in ferrous oxalate-oxalic acid aqueous solution was studied. Nickel ferrite was synthesized by thermal decomposition of a mixed tartrate; the particles were shown to be coated with a thin ferric oxide layer. Dissolution takes place in two stages, the first one corresponding to the dissolution of the ferric oxide outer layer and the second one being the dissolution of Ni1.06Fe1.96O4. The kinetics of dissolution during this first stage is typical of ferric oxides: in oxalic acid, both a ligand-assisted and a redox mechanism operates, whereas in the presence of ferrous ions, redox catalysis leads to a faster dissolution, The rate dependence on both oxalic acid and on ferrous ion is described by the Langmuir-Hinshelwood equation; the best fitting corresponds to K-1(ads) = 25.6 mol(-1) dm(-3) and k(1)(max) = 9.17 x 10(-7) mol m(-2) s(-1) and K-2(ads) = 37.1 x 10(3) mol(-1) dm(-3) and k(2)(max) = 62.3 x 10(-7) mol m(-2) s(-1) respectively, In the second stage, Langmuir-Hinshelwood kinetics also describes the dissolution of iron and nickel from nickel ferrite, with K-1(ads) = 20.8 mol(-1) dm(3) and K-2(ads) = 1.16 x 10(5) mol(-1) dm(3). For iron, k(1)(max) = 1.02 x 10(-7) mol of Fe m(-2) s(-1) and k(2)(max) = 2.38 x 10(-7) mol of Fe m(-2) s(-1); for nickel, the rate constants k(1)(max) and k(2)(max) are 2.4 and 1.79 times smaller respectively, The factor 1.79 agrees nicely with the stoichiometric ratio, whereas the factor 2.4 implies the accumulation of some nickel in the residual particles. The rate of nickel dissolution in oxalic acid is higher than that in bunsenite by a factor of 8, whereas hematite is more reactive by a factor of 9 (in the absence of Fe(II)) and 27 (in the presence of Fe(II)), It may be concluded that oxalic acid operates to dissolve iron, and the ensuing disruption of the solid framework accelerates the release of nickel.