Ionization and Hydration Equilibria of Periodic Acid¹

The oxidation of 2-(2-methoxyethoxy)-ethanol and 2-(2-ethoxyethoxy)-ethanol by dihydroxydiperiodato nickelate(IV): A kinetic and mechanistic study

“…The amount of dimer H2I2O10 4-and IO4 -species can be neglected, the main species of periodate are H3IO6 2-and H2IO6 3-, which was consistent with the result calculated from Crouthamel's date by Murthy [18,19]. Based on such distribution, the formula of Ni(IV) periodate complex is represented by the less protonated ionic species [Ni(OH)2(H2IO6)2] 4-.…”

Enthalpies of solution of Kbr, Ki, Kio3, and Kio4 in H2o

“…15K) = (63 .49± O.lJ)kj-mol -1 (6) From the ir solubility data, Crouthamel e t a1. [33] calculated 63.2 kJ'mol-1 which is in good agreeme nt with eq (6).…”

“…KI04 in H20 given in section 3 include a partial hydrolysi reaction for which a correction must be made in order t' obtain only the periodate as the anion product. Crouthamel ~' ayes, and Martin [33] have re po rted tlH ,5.6 kJ) from 0 °C to 70°C fo r th e reacti.on 10.9 kcal (or (4) lfrom their work, Parker [34] de ri ved the followi ng equation ime nts given in tabl e 6 was multiplied by 45600 l mol-1 we obtained the cO ITections, Q '" whi c h we re added to tlH(T). Walden , 1907 [20] W ust and Lange, 1925 [21] Popov, Bunde1, a nd Cho11er, 1930 [22] Chipman, Johnson a nd Maass, 1929 [23] Fedorov and Si1 ' chenko, 1937 [24 ] Lange and Martin, 1937 [25] Popov, Skuratov, and Stre1'tsova, 1940 [26] Hi eta la, 1960, [27] Parker's "Best " valu e , 1965 [1] Krestov and Abrosimov, 1967 [2] Tsvetkov and Rabi novich, 1969 [3] Jo1y, Thourey, and P~rachon, 1973 [5] 01ofsson, 1977 [6] This work (USSR) Tsvetkov and Rabinovich, 1969 [2] Jo1y , Thourney and Perachon, 1973 [5] Thi s work (USSR)…”

A calorimetric study of periodate species in aqueous solution

“…While our estimated uncertainty of this heat is Ifi0.7 kcal/mole, this seems to be quite a large heat of ionization. The plot of log K2 vs. 1/T given by Crouthamel et al (4) did exhibit considerable curvature at low temperatures so that this heat of ionization would not be inconsistent with their data. It is also possible that the heat of dehydration is somewhat more positive than that reported by previous investigators (4,12).…”

“…In order to determine the heats of formation of the many aqueous periodate species from the heat of formation of NaIO,(c), the heat of solution of sodium periodate was measured in 0.100 M NaC10, solution and 0.100 M HClO, solution. These heats are summarized in Tables IV and V They found for reaction [2], K, = 5.1 x lo-", AH, -0 kcal/mole; for reaction [3], K, = 40, AH, = 10.9 kcal/mole; for reaction [4], K, = 2.0 x lo-', AH, -0 kcal/mole. All of these equilibrium constants were measured in solutions which were very dilute.…”