THE HEAT OF FORMATION OF THE HYPOCHLORITE ION¹

Excess Thermodynamic Properties of Aqueous Alcohol Solutions.

“…The change of resistance of the thermistor with time was recorded. By operating the Wheatstone Bridge near the balancing point at all times, errors resulting from unbalancing were considerably minimized (10). Sensitivity of the system could be varied from run to run and during the run if necessary from about 2 to 40 mv.…”

“…Unquestionably, reasons for the complex phase behavior among crystalline solids in the LiF-NaF-ZrF4 system will be obtainable only through studies of the crystal chemistry of these nine fluorides. The structures of only two of these crystalline phases, 3NaF-ZrF4 (10) and 2LiF• ZrF4 (12), have been elucidated. Single-crystal studies of the compound 7NaF-6ZrF4 have been in progress for some VOL.…”

Heat and Entropies of Formation of Metal Chelates of Polyamine and Polyaminocarboxylate Ligands.

“…For all of the determinations except those for the polyamine chelates and part of the EDTA chelates, the heat capacity of the system was determined after thermal equilibrium was reached at the end of the reaction. For this purpose, a known quantity of energy was introduced into the system by passing a constant current (Sargent Coulometric Current Source, Model IV) through a known resistance (19). For the other determinations, the heat capacity of the solution was estimated from a knowledge of the ionic strength of the solutions and established values given by Randall and Rossini (22).…”

Thermochemistry of hypochlorite oxidations

“…Many reductants such as iodide, sulfide, thiosulfate, cyanide, and thiocyanate are rapidly oxidized in basic solution. In some cases excess base must be added; 0.5 M sodium thiosulfate must be dissolved in 1.1 M sodium hydroxide, for example 4 CIO" + SUL2-+ 20H -= 2SOP-+ 4C1-+ HaO AH = -330 koal/mole…”