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.

VOLTAIC CELLS IN FUSED SALTS: PART V. THE SYSTEMS Sn/SnCl2 (KCl–NaCl), Fe/FeCl2 (KCl–NaCI), and Mn/MnCl2 (KCl–NaCl)

1958 ◽  
Vol 36 (12) ◽  
pp. 1662-1667 ◽  
Author(s):  
S. N. Flengas ◽  
T. R. Ingraham
Keyword(s):  
Reference Electrode ◽  
Effect Of Temperature ◽  
Nernst Equation ◽  
Fused Salts ◽  
Electrode Potentials ◽  
Standard Electrode Potentials

Using a Ag/AgCl (KCl–NaCl) reference electrode, the standard electrode potentials of the systems Sn/SnCl2 (KCl–NaCl), Fe/FeCl2 (KCl–NaCl), and Mn/MnCl2 (KCl–NaCl) were determined at 700 °C and found to be 0.370 v, 0.520 v, and 1.205 v respectively. In each of the systems the Nernst equation was found to be applicable over the range of concentrations investigated.The effect of temperature on the electromotive forces of the above cells was measured and the heats of the cell reactions were calculated from the data.

VOLTAIC CELLS IN FUSED SALTS: PART IV. ELECTRODE POTENTIALS OF THE SYSTEMS: Tl/TlCl (KCl–NaCl), Cu/CuCl (KCl–NaCl), Cu/CuCl2 (KCl–NaCl), Cr/CrCl2 (KCl–NaCl), AND Cr/CrCl3 (KCl–NaCl). REDOX POTENTIALS OF THE SYSTEMS: Pt/CuCl, CuCl2 (KCl–NaCl), AND Pt/CrCl2, CrCl3 (KCl–NaCl)

1958 ◽  
Vol 36 (7) ◽  
pp. 1103-1115 ◽  
Author(s):  
S. N. Flengas ◽  
T. R. Ingraham
Keyword(s):  
Reference Electrode ◽  
Effect Of Temperature ◽  
Redox Potentials ◽  
Fused Salts ◽  
Electrode Potentials ◽  
Standard Electrode Potentials

Using a Ag/AgCl (KCl–NaCl) reference electrode, the standard electrode potentials of the systems Tl/TlCl (KCl–NaCl), Cu/CuCl (KCl–NaCl), Cu/CuCl2 (KCl–NaCl), Cr/CrCl2 (KCl–NaCl), and Cr/CrCl3 (KCl–NaCl) were measured and found to be: 0.650 volt at 680 °C, and 0.250, −0.175, 0.755, and 0.423 at 700 °C. respectively. The standard redox potentials of the systems Pt/CuCl2, CuCl (KCl–NaCl), and Pt/CrCl3, CrCl2 (KCl–NaCl) were also measured at 700 °C. and found to be 0.600 and 0.240 volt respectively. The effect of temperature on the electromotive forces of the above cells was measured and the heats of the cell reactions were calculated from the data.

Sulfate-sensing electrodes. The lead- amalgam/lead-sulfate electrode (IUPAC Technical Report)

2002 ◽  
Vol 74 (4) ◽  
pp. 593-600 ◽  
Author(s):  
Patrizia R. Mussini ◽  
Torquato Mussini
Keyword(s):  
Reference Electrode ◽  
Salt Bridge ◽  
Lead Sulfate ◽  
Preparation Procedure ◽  
Reference Electrodes ◽  
Electrode Potentials ◽  
Sulfate Solutions ◽  
Technical Report ◽  
Convenient Preparation ◽  
Lead Amalgam

A new, simplified design and a convenient preparation procedure for the Pb(Hg)|PbSO4|SO42- electrode are proposed. This procedure ensures preparation of stable amalgams and reproducible electrode potentials, which make this electrode useful and attractive for both thermodynamic investigations and electroanalytical applications. For these purposes, the electrode prepared according to the proposed procedure has been exhaustively characterized both thermodynamically and as a sulfate-sensing electrode, in different sulfate solutions, including H2SO4. Also, a practical standardization procedure has been proposed. The Pb(Hg)|PbSO4|SO42- electrode can be structured with a built-in concentrated Li2SO4 salt bridge for use as a sulfate-based reference electrode. This electrode can be operated as a reference electrode alternative to the conventional calomel or Ag|AgCl reference electrodes in electroanalytical practice.

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.

The Standard Electrode Potentials of Zinc and Copper

1968 ◽  
pp. 106-109
Author(s):  
J.M. WILSON ◽  
R.J. NEWCOMBE ◽  
A.R. DENARO ◽  
R.M.W. RICKETT
Keyword(s):  
Electrode Potentials ◽  
Standard Electrode Potentials
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