Aqueous Solution Chemistry

Many aspects of the aqueous solution chemistry of the group 15 elements have already been covered  

In this section we focus on the formation of aqueous solution species by Sb(III) and Bi(III). Solutions of Sb(III) contain either hydrolysis products or complex ions. The former are commonly written as [SbO]+, but by analogy with Bi(III) 

The following terms were introduced in this chapter. Do you know what they mean  

Corbridge (1995) Phosphorus, 5th edn, Elsevier, Amsterdam - A review of all aspects of phosphorus chemistry. J. Emsley (2000) The Shocking Story of Phosphorus, Macmillan, London - A readable book described as a biography of the devil s element . 

Greenwood and A. Earnshaw (1997) Chemistry of the Elements, 2nd edn, Butterworth-Heinemann, Oxford -Chapters 11-13 give a detailed account of the chemistries of the group 15 elements. 

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The aqueous solution chemistry of Al and the other group 13 metals is rather complicated. The aquo ions are acidic with... 

In addition to simple dissolution, ionic dissociation and solvolysis, two further classes of reaction are of pre-eminent importance in aqueous solution chemistry, namely acid-base reactions (p. 48) and oxidation-reduction reactions. In water, the oxygen atom is in its lowest oxidation state (—2). Standard reduction potentials (p. 435) of oxygen in acid and alkaline solution are listed in Table 14.10- and shown diagramatically in the scheme opposite. It is important to remember that if or OH appear in the electrode half-reaction, then the electrode potential will change markedly with the pH. Thus for the first reaction in Table 14.10 O2 -I-4H+ -I- 4e 2H2O, although E° = 1.229 V,... 

G. Gordon, R. G. Kieffer and D. H. Rosenblatt, Progr. Inorg. Chem. 15, 201-86 (1972). The first half of this review deals with the aqueous solution chemistry of chlorous acid and chlorites. 

The I——12 half-reaction has many applications in aqueous solution chemistry. The use of I- as a reducing agent and I2 as an oxidizing agent, particularly for quantitative purposes, is called iodimetry. 

Advances in Thallium Aqueous Solution Chemistry Julius Glaser... 

In our world, most chemical processes occur in contact with the Earth s atmosphere at a virtually constant pressure. For example, plants convert carbon dioxide and water into complex molecules animals digest food water heaters and stoves bum fiiel and mnning water dissolves minerals from the soil. All these processes involve energy changes at constant pressure. Nearly all aqueous-solution chemistry also occurs at constant pressure. Thus, the heat flow measured using constant-pressure calorimetry, gp, closely approximates heat flows in many real-world processes. As we saw in the previous section, we cannot equate this heat flow to A because work may be involved. We can, however, identify a new thermod mamic function that we can use without having to calculate work. Before doing this, we need to describe one type of work involved in constant-pressure processes. 

The aqueous solution chemistry of Ir in its higher oxidation states III, IV, and V has been explored by Sykes et al.41,48 Chemical and electrochemical oxidation of Ir(H20)6]3+ gives a brown-green Irv product, which undergoes chemical and electrochemical reduction to a blue and a purple IrIV complex. 170 NMR studies are consistent with double- and single-bridged dimeric structures, with likely formulas [(H20)4Ir(/i-0H)2Ir(H20)4]6+ for the blue complex and [(H20)5Ir(/r-0)Ir(H20)5]6+ for the purple one. 

The aqueous solution chemistry of Tc(VII) is dominated by the stability of the TeO anion [4], Nitrido complexes are few and are limited to peroxides and one dimeric nitrido-hydrazido example. The peroxo complexes based on the [TcVIIN(02 )2] core are analogous to the well-known isoelectronic [MoviO(02)2] complexes [117] and are the only examples of nitridoperoxo complexes and rare examples of peroxo complexes of a metal in the +7 oxidation state. 

Popovych, O., and Tompkins, R. P. T. (1981). Non-aqueous Solution Chemistry. Wiley, New York. 

The hydrated cation Ca2+aq is of prime importance to the aqueous solution chemistry of calcium, and to most of its various roles in biological systems. The relation between lattice energy and hydration energies of the constituent ions determine solubilities, the size of the hydrated cation controls selectivity and the passage of ions through channels, and the work required to remove some or all of the water of hydration is relevant both to... 

Aqueous Solution Chemistry of Beryllium Lucia Alderighi, Peter Gans, Stefano Midollini, and Alberto Vacca... 

The literature relating to the aqueous solution chemistry of beryllium has been covered to the end of 1998. Previous reviews and relevant compilations of data are listed in Table I. The scope of this review will be to consider all the published data, with a particular emphasis on quantitative aspects, with the aim of facilitating a general discussion. A brief section relating to health and safety issues will be found at the end. 

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