Electrolyte solutions strong

Fig. 11-1. A strong electrolyte solution conducts better than a weak electrolyte solution.

Calculation of the Thermodynamic Properties of Strong Electrolyte Solutes The Debye-Hiickel Theory... 

Solutions containing strong electrolyte solutes differ from those containing nonelectrolyte solutes in that deviations from Henry s law become important at much lower concentrations for the electrolyte solute than for the nonelectrolyte... 

Figure 7.7 In a strong electrolyte solution, negative ions are preferentially surrounded by positive ions while the positive ions are surrounded by negative ions.

The solute in an aqueous strong electrolyte solution is present as ions that can conduct electricity through the solvent. The solutes in nonelectrolyte solutions are present as molecules. Only a small fraction of the solute molecules in weak electrolyte solutions are present as ions. 

Hence, the theory of electrolyte solutions subsequently developed in two directions (1) studies of weak electrolyte solutions in which a dissociation equilibrium exists and where because of the low degree of dissociation the concentration of ions and the electrostatic interaction between the ions are minor and (2) studies of strong electrolyte solutions, in which electrostatic interaction between the ions is observed. 

The beginning of the twentieth century also marked a continuation of studies of the structure and properties of electrolyte solution and of the electrode-electrolyte interface. In 1907, Gilbert Newton Lewis (1875-1946) introduced the notion of thermodynamic activity, which proved to be extremally valuable for the description of properties of solutions of strong electrolytes. In 1923, Peter Debye (1884-1966 Nobel prize, 1936) and Erich Hiickel (1896-1981) developed their theory of strong electrolyte solutions, which for the first time allowed calculation of a hitherto purely empiric parameter—the mean activity coefficients of ions in solutions. 

As noted earlier, cobalt(II) in strong electrolyte solutions will readily form tetrahedral anionic complexes that can be extracted into an immiscible... 

Here we consider the conductivity of strong electrolyte solutions at moderate to high concentrations in polar non-aqueous solvents. The conductivity of such solutions has been studied extensively, because of their importance in applied fields. 

The rest of this section considers only strong electrolytes. If we could see the individual ions in a strong electrolyte solution, we would see each... 

In a precipitation reaction, an insoluble solid product forms when two strong electrolyte solutions are mixed. When an insoluble substance is formed in water, it immediately precipitates. In the chemical equation for a precipitation reaction, we use (aq) to indicate substances that are dissolved in water and (s) to indicate the solid that has precipitated ... 

Activity coefficient relationships for the different types of strong electrolyte solutions are summarized in Table 11.3. 

C) which he derived from the ionic product of water (Kw = 10 14 mol x dm 3). Some years later, Lewis introduced the concept of activity, and in 1923 Debye and Hiickel published their theory for strong electrolyte solutions. On the basis of this knowledge, Soerensen and Linderstroem-Lang [2] suggested a new pH definition in terms of the relative activity of hydrogen ions in solution ... 

Strong Electrolytes. Solutes of this type, such as HCl, are completely dissociated in ordinary dilute solutions. However, their colligative properties when interpreted in terms of ideal solutions appear to indicate that the dissociation is a little less than complete. This fact led Arrhenius to postulate that the dissociation of strong electrolytes is indeed incomplete. Subsequently this deviation in colligative behavior has been demonstrated to be an expected consequence of interionic attractions. 

As far as mixed strong electrolyte solutions are concerned, Harned s rule [38] holds. At constant ionic strength, the activity coefficient of one electrolyte (A) in the mixture is a function of the fractional ionic strength (y I) of the other electrolyte (B) ... 

Behaviour (c) is in fact only observed in strong electrolyte solutions as we shall see in chap. XXVII A ==1 5, and this behaviour is to be attributed to the long range of electrostatic forces between ions. Cases (a) and (6) arise in other solutions so that, apart from electrolytes, the lowest power of X2 appearing in (21.40) is the second. 

The behaviour of strong electrolyte solutions is of particular interest in this connection. The expansion on fusion is opposed by the contraction on mixing and under certain circumstances these may cancel exactly so that... 

We have already indicated (chap. XXI, 5) that the activity coefficients in a strong electrolyte solution exhibit characteristics quite different from those of non-electrolytes. In a sufficiently dilute nonelectrolyte solution (cf. 21.42),... 

Strong electrolytes Solutes that are completely dissociated into... 

Define the mean ion activity coefficient of a salt and comment on its significance in a weak versus a strong electrolyte solution. 

The potential distribution of Fig. 1 is typical of the compact-diffuse layer models (42-44). The potential varies almost linearly within the compact double layer, decaying exponentially within the diffuse layer. The thickness of the latter depends on the electrolyte ionic strength and becomes negligible in strong electrolytic solutions (42). This feature becomes important in electrocatalytic studies, since it is the potential difference (0 — < e) that can be measured or fixed experimentally versus a reference electrode, while reacting ions and molecules experience a potential difference ((j) —... 

When electrolyte solutions are involved, however, the osmotic effects such as freezing point lowering, osmotic pressure increase, and rise in boiling point are much greater than corresponds to the total electrolyte concentration. Accordingly, van t Hoff introduced the irrationality factor i (van t Hoff factor) by which the particular osmotic effect could be divided to yield a number which satisfied the equation of state (i is always greater than 1). The van t Hoff factor is purely empirical and does not account for the anomalous behavior of strong electrolyte solutions. 

Ac Choice of Standard States for Strong Electrolyte Solutes... 

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