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in which the constant A for 25 and water has a value close to 0.5 dm3/2 mol~1/2. Quantity /, called the ionic strength, describes the electrostatic effect of individual ionic species by the equation

Figure 6.6 All of the home network devices have their own private IP addresses in the 192.168.10.0/24 range. The router will use a PAT table to keep track of each address and port translation that occurs.

(1.1.22)

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(In fact, the symbol Ic should be used, as the molality ionic strength lm can be defined analogously; in dilute aqueous solutions, however, values of c and m, and thus also Ic and / m , become identical.) Equation (1.1.21) was later derived theoretically and is called the Debye-Hiickel limiting law. It will be discussed in greater detail in Section 1.3.1. 1.1.4 The A rrhenius theory of electrolytes





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At the end of the last century S. Arrhenius formulated the first quantitative theory describing the behaviour of weak electrolytes. The

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10 existence of ions in solution had already been demonstrated at that time, but very little was known of the structure of solutions and the solvent was regarded as an inert medium. Similarly, the concepts of the activity and activity coefficient were not employed. Electrochemistry was limited to aqueous solutions. However, the basis of classical thermodynamics was already formulated (by J. W. Gibbs, W. Thomson and H. v. Helmholtz) and electrolyte solutions had also been investigated thermodynamically especially by means of cryoscopic, osmometric and vapour pressure measurements. Van't Hoff introduced the correction factor i for electrolyte solutions; the measured quantity (e.g. the osmotic pressure, Jt) must be divided by this factor to obtain agreement with the theory of dilute solutions of nonelectrolytes (jz/i = RTc). For the dilute solutions of some electrolytes (now called strong), this factor approaches small integers. Thus, for a dilute sodium chloride solution with concentration c, an osmotic pressure of 2RTc was always measured, which could readily be explained by the fact that the solution, in fact, actually contains twice the number of species corresponding to concentration c calculated in the usual manner from the weighed amount of substance dissolved in the solution. Small deviations from integral numbers were attributed to experimental errors (they are now attributed to the effect of the activity coefficient). For other electrolytes, now termed weak, factor / has non-integral values depending on the overall electrolyte concentration. This fact was explained by Arrhenius in terms of a reversible dissociation reaction, whose equilibrium state is described by the law of mass action. A weak electrolyte Bv+Av_ dissociates in solution to yield v ions consisting of v+ cations B z + and v_ anions Az~, Bv+Av _<=* v + B z + + v_Az~ (1.1.23)

How does the router in Figure 6.7 obtain the necessary public IP address that will be shared by the home network devices

Thus the magnitude of the constant called the thermodynamic or real dissociation constant, ^ (1.1.24)

Figure 6.7 The router needs a way to determine what public IP address it needs to use. DHCP is the protocol that allows the router to get a dynamically assigned IP address.

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is a measure of the 'strength of the electrolyte'. The smaller its value, the weaker the electrolyte. The activity can be replaced by the concentrations according to Eq. (1.1.10), yielding

every home router/PC that needs to connect to the Internet requires a public IP address. These IP addresses have to be requested from the Internet Assigned numbers Authority (IAnA) and its regional subsidiaries. A home user does not request an IP address from IAnA, but from the service provider. The service providers are

rp>z+iv+r A Z - I V v+ v_ v+ v_

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