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that the solution is to certain degree ordered, results in lower values of the ionic entropies In special cases, the ionic entropy can be measured (eg from the dependence of the standard potential on the temperature for electrodes of the second kind) Otherwise, the heat of solution is the measurable quantity Knowledge of the lattice energy then permits calculation of the heat of hydration For a saturated solution, the heat of solution is equal to the product of the temperature and the entropy of solution, from which the entropy of the salt in the solution can be found However, the absolute value of the entropy of the crystal must be obtained from the dependence of its thermal capacity on the temperature down to very low temperatures The value of the entropy of the salt can then yield the overall hydration number.

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It is, however, difficult to separate the contributions of the cation and of the anion Various methods have yielded the following average values of the primary hydration numbers of the alkali metal cations (the number of methods used is given in brackets and the results are rounded off to the nearest integers): Li+ 5 (5), Na+ 5 (5), K+ 4 (4), Rb + 3 (4), and for the halide ions: F" 4 (3), Cl~ 1 (3), Br" 1 (3), I" 1 (2) The error is 1 water molecule (except for K + , where the error is 2) For divalent ions the values vary between 10 and 14 (according to G Kortiim) For illustration of the variability of the results obtained by various methods, the values obtained for the Na+ ion.

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1a. Can you use a CLI Help function to find out how many log files can be configured 2. Configure which events will generate debug/execution trace information, for any listening log files.

from mobility measurements were 2-4, from the entropy 4, from the compressibility 6-7, from molar volumes 5, from diffusion 1 and from activity coefficients also 1 For the Cl~ ion, these methods yielded the values (in the same order): 4, 3, 0, 1, 0, 0, 1 Of the divalent ions, for example, solution of Mg2+ was measured by the mobility method, yielding a value of 10 to 13, entropy of 13, compressibility of 16 and activity coefficients of 5 (according to B E Conway and J O'M Bockris) Remarkable data on primary hydration shells are obtained in nonaqueous solvents containing a definite amount of water Thus, nitrobenzene saturated with water contains about 02 M H2O Because of much higher dipole moment of water than of nitrobenzene, the ions will be preferentially solvated by water Under these conditions the following values of hydration numbers were obtained: Li+ 6.

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2a. Use a CLI Help function to find out what other categories of events can be specified as a source of debug information. How many are there in the router ip context 3. From CE1 and PE2, attempt to ping the IP address of PE1 s interfaces. Observe the debug ICMP messages on the core routers.

5, H + 55, Ag+ 44, Na+ 39, K+ 15, Tl + 10, Rb + 08, Cs + 05, tetraethylammonium ion 00, CIO4-O4, NO^ 14 and tetraphenylborate anion 00 (assumption) 124 Ion association As already mentioned, the criterion of complete ionization is the fulfilment of the Kohlrausch and Onsager equations (2415) and (2426) stating that the molar conductivity of the solution has to decrease linearly with the square root of its concentration However, these relationships are valid at moderate concentrations only At high concentrations, distinct deviations are observed which can partly be ascribed to non-bonding electrostatic and other interaction of more complicated nature (cf p 38) and partly to ionic bond formation between ions of opposite charge, ie to ion association (ion-pair formation).

*A:CE1>config>router# ping 140.10.0.101 PING 140.10.0.101 56 data bytes 64 bytes from 140.10.0.101: icmp_seq=1 ttl=64 time=10ms. 64 bytes from 140.10.0.101: icmp_seq=2 ttl=64 time<10ms. [... Additional output omitted ...] [ Output captured from PE1 terminal session ] 1 2000/01/01 13:53:45.62 UTC MINOR: DEBUG #2001 Base PIP PIP: ICMP instance 1 (Base), interface index 4 (toCE1), ICMP ingressing on toCE1: 140.10.0.102 -> 140.10.0.101 type: Echo (8) code: No Code (0)

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The separation of these two effects is indeed rather difficult The species appearing as strong electrolytes in aqueous solutions lose this property in low-permittivity solvents The ion-pair formation converts them to a sort of weak electrolyte In solvents of very low-permittivity (dioxan, benzene) even ion triplets and quadruplets are formed The formation of an ion pair A + + B"^ A + B(1213).

2 2000/01/01 13:53:45.62 UTC MINOR: DEBUG #2001 Base PIP PIP: ICMP instance 1 (Base), interface index 4 (toCE1), ICMP egressing on toCE1: 140.10.0.101 -> 140.10.0.102 type: Echo Reply (0) code: No Code (0)

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