Thallium and Tin Electrode Potentials in Fused LiCl–KCl Eutectic

1973 ◽  
Vol 51 (11) ◽  
pp. 1693-1696 ◽  
Author(s):  
Joseph M. Shafir ◽  
James A. Plambeck
Keyword(s):  
Reference Electrode ◽  
Ionic Species ◽  
Dilute Solutions ◽  
Electrode Potentials

Electrode potentials of thallium and tin couples were measured in dilute solutions of the ionic species in fused LiCl–KCl eutectic, at 450 °C. Standard molar electrode potentials of the Tl(III)/Tl(I) and Sn(IV)/Sn(II) couples are +0.155 and −0.310 V against a standard molar platinum reference electrode (s.m.p.e.). The standard potentials of the Tl(III)/Tl(0) and Sn(IV)/Sn(0) couples were calculated to be −0.385 and −0.964 V, respectively, vs. the s.m.p.e.

Ruthenium and Arsenic Electrode Potentials in Fused LiCl–KCl Eutectic

1972 ◽  
Vol 50 (23) ◽  
pp. 3911-3912 ◽  
Author(s):  
T. Folkman ◽  
James A. Plambeck
Keyword(s):  
Platinum Electrode ◽  
Ionic Species ◽  
Potential Range ◽  
Dilute Solutions ◽  
Electrode Potentials

Electrode potentials of the Ru(III)/Ru(0) and As(III)/As(0) systems were measured in dilute solutions of the ionic species in fused LiCl–KCl eutectic at 450 °C. Standard molar electrode potentials of these couples of −0.107 ± 0.007 V and −0.460 ± 0.017 V against a standard molar platinum electrode were calculated. The As(V)/As(III) potential was found to be beyond the potential range of the melt.

Gallium and indium electrode potentials in fused LiCl–KCl eutectic

1970 ◽  
Vol 48 (13) ◽  
pp. 2131-2132 ◽  
Author(s):  
Joseph M. Shafir ◽  
James A. Plambeck
Keyword(s):  
Ionic Species ◽  
Oxidation States ◽  
Dilute Solutions ◽  
Electrode Potentials ◽  
Salt Systems ◽  
Indium Electrode ◽  
Fused Salt

Electrode potentials of indium and gallium couples have been measured in dilute solutions of the ionic species in fused LiCl–KCl eutectic at 450 °C. Standard molar electrode potentials of the observed couples are −1.210, −0.944, and −1.136 V against a standard molar platinum reference for the In(I)–In(0), In(III)–In(I), and Ga(III)–Ga(0) couples, respectively. These oxidation states and potentials are compared with previous work in this and other fused salt systems.

Beryllium and scandium electrode potentials in fused LiCl–KCl eutectic

1968 ◽  
Vol 46 (6) ◽  
pp. 929-931 ◽  
Author(s):  
James A. Plambeck
Keyword(s):  
Ionic Species ◽  
Dilute Solutions ◽  
Electrode Potentials

Electrode potentials of the Be(II)–Be(0) and Sc(III)–Sc(0) systems were measured in dilute solutions of the ionic species in fused LiCl–KCl eutectic at 450 °C. Standard molar electrode potentials of these couples of −2.039 ± 0.013 V and −2.553 ± 0.015 V against a standard molar platinum reference were calculated. It was shown by voltammetric and chronopotentiometric methods that the equilibrium [Formula: see text] suggested by previous authors was not significant in this medium.

Reversible electrode potentials for formation of solid and liquid chlorozirconate and chlorohafnate compounds

1993 ◽  
Vol 71 (9) ◽  
pp. 1283-1289 ◽  
Author(s):  
G.J. Kipouros ◽  
S.N. Flengas
Keyword(s):  
Thermal Decomposition ◽  
Alkali Metal ◽  
Electrochemical Behaviour ◽  
Thermochemical Data ◽  
Dilute Solutions ◽  
Alkali Metal Chlorides ◽  
Metal Chlorides ◽  
Electrode Potentials ◽  
Standard Electrode Potentials

The standard electrode potentials for the formation of the pure solid and molten compounds Li2ZrCl6, Li2HfCl6, Na2ZrCl6, Na2HfCl6, K2ZrCl6, K2HfCl6, Cs2ZrCl6, and Cs2HfCl6 have been calculated from measured vapour pressures corresponding to their thermal decomposition at equilibrium and from available thermochemical data. Reversible potentials for the formation of Na2ZrCl6 and of K2ZrCl6 in solution according to the reaction[Formula: see text]where A is Na or K, have been calculated from available equilibrium vapour pressures as functions of the mole fractions of the alkali hexachlorocompounds. Standard potentials for the above reaction and "formal" potentials are also given. The latter are useful in predicting the electrochemical behaviour of dilute solutions of the hexachlorozirconates in alkali metal chlorides.

ELECTRODE POTENTIALS OF THORIUM TETRACHLORIDE IN ALKALI CHLORIDE MELTS

1964 ◽  
Vol 42 (6) ◽  
pp. 1315-1322 ◽  
Author(s):  
R. Srinivasan ◽  
S. N. Flengas
Keyword(s):  
Silver Chloride ◽  
Gravimetric Method ◽  
Reference Electrode ◽  
The Other ◽  
Alkali Chloride ◽  
Electrode Potentials ◽  
Silver Chloride Reference Electrode ◽  
Chloride Melts ◽  
Silver Silver ◽  
Silver Silver Chloride

The electrode potentials of the system Th, ThCl4 (KCl, NaCl) were measured at various concentrations of thorium chloride, and at temperatures between 670 °C and 850 °C, using a silver – silver chloride reference electrode. It was shown by a direct gravimetric method that the reaction,Th(metal) + ThCl4(melt) = 2ThCl2(in melt),postulated by previous investigators, did not take place.The activity coefficients, and the other partial molal properties of the solutions of ThCl4, in the equimolar mixture of potassium and sodium chlorides, were calculated as a function of temperature from the e.m.f. measurements.

ELECTROCHEMICAL STUDIES ON TITANIUM IN MOLTEN LiCl–KCl EUTECTIC

1965 ◽  
Vol 43 (1) ◽  
pp. 197-205 ◽  
Author(s):  
R. Baboian ◽  
D. L. Hill ◽  
R. A. Bailey
Keyword(s):  
Anodic Dissolution ◽  
Mole Fraction ◽  
Coulometric Titration ◽  
Reference Electrode ◽  
Electrochemical Studies ◽  
Reference Electrodes ◽  
Electrode Potentials ◽  
Standard Electrode Potentials

The methods of potentiometry and polarography have been used to study the Ti(II) and Ti(III) ions in solution in the LiCl–KCl eutectic at 450 °C and 550 °C. Solutions of Ti(II) were prepared by anodic dissolution of Ti metal, and Ti(III) solutions by coulometric titration of Ti(II) by Pt(II). Apparent standard electrode potentials were measured for the Ti(II)/Ti and Ti(III)/Ti(II) couples against the Pt(II)/Pt and Ag(I)/Ag reference electrodes. Values obtained on the mole fraction scale with a Pt(II)/Pt reference electrode were[Formula: see text]Polarographic waves for oxidation and reduction of Ti(II), and for reduction of Ti(III), were observed.

Studies of Galvanic Corrosion Couples in Liquid Fluorine

CORROSION ◽  
1968 ◽  
Vol 24 (12) ◽  
pp. 418-421 ◽  
Author(s):  
S. M. TOY ◽  
W. D. ENGLISH ◽  
W. E. CRANE
Keyword(s):  
Galvanic Corrosion ◽  
Reference Electrode ◽  
Metals And Alloys ◽  
Corrosion Rates ◽  
Long Term Storage ◽  
Electrode Potentials ◽  
General Arrangement ◽  
Term Storage

Abstract Galvanic corrosion couples of several metals and alloys were tested in liquid fluorine at −320 F (−196 C), and the corrosion rates of the alloys were determined. A relative galvanic corrosion series, based on the rates, was developed as a guide for selecting materials for missile components exposed to fluorine containing propellants for long term storage. Electrode potentials of Al 1100 and copper versus a platinum reference electrode in liquid fluorine verify the general arrangement of the galvanic series. Evidence of pitting was found on Al 2014-T6 and silver coupons exposed to liquid fluorine.

VOLTAIC CELLS IN FUSED SALTS: PART II. THE SYSTEMS: (a) SILVER – SILVER CHLORIDE, LEAD – LEAD CHLORIDE; (b) SILVER – SILVER CHLORIDE, ZINC – ZINC CHLORIDE; AND (c) SILVER – SILVER CHLORIDE, NICKEL – NICKELOUS CHLORIDE

1957 ◽  
Vol 35 (11) ◽  
pp. 1254-1259 ◽  
Author(s):  
S. N. Flengas ◽  
T. R. Ingraham
Keyword(s):  
Zinc Chloride ◽  
Dissociation Constants ◽  
Silver Chloride ◽  
Reference Electrode ◽  
Lead Chloride ◽  
Effect Of Temperature ◽  
Fused Salts ◽  
Electrode Potentials ◽  
Silver Silver ◽  
Silver Silver Chloride

Using a reversible silver – silver chloride reference electrode, described in the first paper of this series, standard electrode potentials have been established for the systems lead – lead chloride, zinc – zinc chloride, and nickel – nickelous chloride, in melts containing equimolar quantities of KCl and NaCl. Deviations from ideality were observed, and these were attributed to the formation of complexes. Dissociation constants for the complexes were calculated. The effect of temperature on the electromotive forces of the voltaic cells was also measured, and the heats of the cell reactions were calculated from the data.

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