Mead electrolytes

The formation of 2D Meads phases on a foreign substrate, S, in the underpotential range can be well described considering the substrate-electrolyte interface as an ideally polarizable electrode as shown in Section 8.2. In this case, only sorption processes of electrolyte constituents, but no Faradaic redox reactions or Me-S alloy formation processes are allowed to occur, The electrochemical double layer at the interface can be thermodynamically considered as a separate interphase [3.54, 3.212, 3.213]. This interphase comprises regions of the substrate and of the electrolyte with gradients of intensive system parameters such as chemical potentials of ions and electrons, electric potentials, etc., and contains all adsorbates and all surface energy. Furthermore, it is assumed that the chemical potential //Meads is a definite function of the Meads surface concentration, F, and the electrode potential, E, at constant temperature and pressure Meads (7", ). Such a model system can only be... 

The formation of Meads on S corresponds to a transfer of solvated Me j ions from the electrolyte phase (El) to the interphase 0P) forming specifically adsorbed metal adions, Me d, which are partially desolvated and located in the inner part of the electrochemical double layer ... 

Figure 3.1 Phase scheme of an electrochemical system containing substrate (S) in contact with metal (Mei), electrolyte (El) with Meg, and metal (Me2) to derive the electrochemical equilibrium conditions for 2D Meads phases and the 3D Me bulk phase on S. Mei and Me2 are chemically identical metals Me.

The thermodynamics of 2D Meads overlayers on ideally polarizable foreign substrates can be relatively simply described following the interphase concept proposed by Guggenheim [3.212, 3.213] and later applied on Me UPD systems by Schmidt [3.54] as shown in Section 8.2. A phase scheme of the electrode-electrolyte interface is given in Fig. 8.1. Thermodynamically, the chemical potential of Meads is given by eq. (8.14) as a result of a formal equilibrium between Meads and its ionized form Me in the interphase (IP). The interphase equilibrium is quantitatively described by the Gibbs adsorption isotherm, eq. (8.18). In the presence of an excess of supporting electrolyte KX, i.e., c , the chemical potential is constant and... 

CCRIS 3510 EINECS 206-059-0 EPA Pesticide Chemical Code 073508 K-Lyte K-Lyte/CI K-Lyte DS Monopotassium carbonate Potassium acid cadronate Potassium bicarbonate Potassium hydrogen carbonate. Electrolyte replenisher. Used in pharmaceutical formulation. White crystals soluble in H2O (35.7 g/100 ml at 20°, 50 g/100 ml at 50°), insoluble in EtOH. Bristol Latioratories Mead Johnson Labs. 

Towards 1990, a group at the Engineering Research Laboratories in Denmark, with a group at the Mead Paper Company in the US (in what came to be known as the MHB venture) developed a solvent-diluted electrolyte which was polymerised in situ (Lee et al, 1989). This electrolyte is characterised by the incorporation of a liquid matter, such as propylene carbonate in a polymer matrix that is formed by crosslinking a monomer after mixing in the liquid phase. 

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