Mercury water

Assume that an aqueous solute adsorbs at the mercury-water interface according to the Langmuir equation x/xm = bc/( + be), where Xm is the maximum possible amount and x/x = 0.5 at C = 0.3Af. Neglecting activity coefficient effects, estimate the value of the mercury-solution interfacial tension when C is Q.IM. The limiting molecular area of the solute is 20 A per molecule. The temperature is 25°C. 

Incidentally, a quantity called the rational potential is defined as E for the mercury-water interface (no added electrolyte) so, in general, = E + 0.480 V if a normal calomel reference electrode is used. 

Equation V-64 is that of a parabola, and electrocapillary curves are indeed approximately parabolic in shape. Because E ax tmd 7 max very nearly the same for certain electrolytes, such as sodium sulfate and sodium carbonate, it is generally assumed that specific adsorption effects are absent, and Emax is taken as a constant (-0.480 V) characteristic of the mercury-water interface. For most other electrolytes there is a shift in the maximum voltage, and is then taken to be Emax 0.480. Some values for the quantities are given in Table V-5 [113]. Much information of this type is due to Gouy [125], although additional results are to be found in most of the other references cited in this section. 

Assume that a salt, MX (1 1 type), adsorbs at the mercury-water interface according to the Langmuir equation ... 

Many organic electrode processes require the adsorption of the electroactive species at the electrode surface before the electron transfer can occur. This adsorption may take the form of physical or reversible chemical adsorption, as has been commonly observed at a mercury/water interface, or it may take the form of irreversible, dissociative chemical adsorption where bond fracture occurs during the adsorption process and often leads to the complete destruction of the molecule. This latter t q)e of adsorption is particularly prevalent at metals in the platinum group and accounts for their activity as heterogeneous catalysts and as... 

C14-0055. Mercury, water, and bromine are liquids at J — 298 K, P = 1 bar. Their molar entropies are in the sequence H2 O < Hg < BT2. Using molecular properties, explain why bromine has more entropy than mercuiy but water has the least entropy of these three. 

Only this equation has been used in practice. For a mercury/water interface, the (Ajj Pjo is equal to -0.25 V2,23 or-0.22 V. Its components [Eq. (7)] have been estimated to be -0.30 V and -0.05 V, respectively They show that in the presence of water, the electrons cannot expand freely as in a gas, but are pushed into mercury, and that the interaction of water... 

Mattigod, S., Mercury remediation A tiny solution to a big problem—using nanotechnology for adsorbing mercury, Water and Wastewater Products, 9, 20-24. 

Gaudet, C., S. Lingard, P. Cureton, K. Keenleyside, S. Smith, and G. Raju. 1995. Canadian environmental guidelines for mercury. Water Air Soil Pollut. 80 1149-1159. 

Nishimura, H. and M. Kumagai. 1983. Mercury pollution of fishes in Minamata Bay and surrounding water analysis of pathway of mercury. Water Air Soil Pollut. 20 401-411. 

Table II. Assignments of the Major Infrared Bands for Isoquinoline at the Mercury/water Interface...

Ideal polarizable interfaces are critical for the interpretation of electrochemical kinetic data. Ideality has been approached for certain metal electrode-solution interfaces, such as mercury-water, allowing for the collection of data that can be subjected to rigorous theoretical analysis. 

Buffle, J. and Cominoli, A. (1981). Voltammetric study of humic and fulvic substances. Part IV. Behaviour of fulvic substances at the mercury-water interface, J. Electroanal. Chem., 121, 273-299. 

Researches carried out in electrochemistry on solid electrodes and especially on the mercury-water interface have made a significant contribution to an understanding of interfacial phenomena. Although the electrode-water interfaces are typically... 

Systematic variation of the reaction conditions has increased the enantiomeric excess to 47.4 % in the presence of yohimbine [138]. Lowering both the cathode working potential and the pH improved the degree of asymmetric induction, and no further improvement in induction is achieved by raising the concentration of alkaloid above 0.4 mM. Enantioselectivity is due to an adsorbed layer of alkaloid and adsorption phenomena at the mercury water interface are dependent on the surface... 

Some compounds fomi a surface excess concentration at the mercury - water interface and optically active compounds in this class can generate a chiral surface... 

This [Reine] is the Mercurial Water of the Philosophers they have so named it because they called their Sulphur a King, he who must be married to this Water [Mercury], which is his natural Bride and his Mother [son epouse naturelle, et sa mere]. Basil Valentine and Trevisan are the two alchemical writers who have most specifically discussed the allegorical terminology of the Queen. ... 

Firmly in the iatrochemical tradition, Homberg believed that the analysis by fire revealed the familiar five principles, salt, sulphur, mercury, WATER, and EARTH. SuLPHUR was the active and earth the passive principle, the others having an intermediate nature. Earth never acts, but serves only as a receptacle or matrix for the other principles.These, of course, were the philosophical principles, and he spent some time describ-... 

A synthetic study has revealed that the combination of anhydrous hydrogen chloride and zinc(II) chloride in the presence of a nucleophile, e.g. benzenethiol, promotes the ring cleavage of cyclobutanones such as bicyclo[3.2.0]heptan-6-one (28) to provide / -sulfanyl ketones such as 3-phenylsulfanylcycloheptanone (27).63 Alternatively, iodotrimethylsilane in the presence of either mercury/water or zinc(II) iodide also converts cyclobutanones to /i-iodo ketones 29.64 The synthetic applications of these transformations are summarized in Table 5. 

Using 379.5 and 34.0 erg cm-2, respectively, as the values of y for the mercury-water and benzene-water interfaces, compare the observed contact angles with the predictions of Young s equation. Comment on the fact that constant values are used for yHg w and ybeniene.w... 

Values of the parameter 0 may be experimentally evaluated for the mercury-water surface from electrocapillary studies. The displacement of the coordinates of the electrocapillary maxima in Figure 7.23 reflects differences in the intrinsic adsorbability of various ions. Electrocapillary studies reveal that the strength of specific adsorption at the mercury-water interface for some monovalent anions follows the order... 

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