Bromides, solubility product

Silver-bromide (solubility product still coarsens rather rapidly at slightly... 

Subsequent kinetic work has amply confirmed the mechanistic picture described above. For example, the reaction of diphenylmercury with Ph(COOEt).CH.HgBr gives an almost instantaneous reaction with precipitation of phenylmercuric bromide, whereas reaction of the soluble product with a second molar equivalent of mercuric bromide gave a very slow (ca. 2 weeks) precipitation of phenylmercuric bromide722, i.e. reaction involves (287) and (288)... 

For the preparation of MBM, the starting phenol was alkylated to 2-(n)-butoxy-1,4-dimethoxybenzene in methanolic KOH with n-butyl bromide. The benzaldehyde melted at 79.5-81 °C from methanol, and formed a malononitrile derivative that had a melting point of 134.5-135 C. The nitrostyrene from the aldehyde and nitroethane in acetic acid crystallized from methanol with a mp of 71 -72 °C. Lithium aluminum hydride reduction in ether gave the ether-insoluble chloroform-soluble product 4-(n)-butoxy-2,5-dimethoxyamphetamine hydro-... 

A (T1+ T1) couple was prepared by saturating 0.1 M KBr with TIBr and allowing the T1+ from the relative insoluble bromide to come to equilibrium. This couple was observed to have a potential of —0.443 V with respect to a (Pb2+ Pb) couple in which the Pb2+ was 0.1 molar. What is the solubility product of TIBr ... 

The hydrolysis of the ammonium carbonate in aqueous solution gives rise to free dilute ammonia solution in which silver chloride, but not silver bromide or silver iodide, is appreciably soluble. The addition of bromide ions to the solution of silver chloride in ammonia results in the solubility product of silver bromide being exceeded, and precipitation occurs. 

Colloidal dispersions owe their stability to a surface charge and the resultant electrical repulsion of charged particles. This charge is acquired by adsorption of cations or anions on the surface. For example, an ionic precipitate placed in pure water will reach solubility equilibrium as determined by its solubility product, but the solid may not have the same attraction for both its ions. Solid silver iodide has greater attraction for iodide than for silver ions, so that the zero point of charge (the isoelectric point) corresponds to a silver ion concentration much greater than iodide, rather than to equal concentrations of the two ions. The isoelectric points of the three silver halides are ° silver chloride, pAg = 4, pCl = 5.7 silver bromide, pAg = 5.4, pBr = 6.9 silver iodide, pAg = 5.5, pi = 10.6. For barium sulfate the isoelectric point seems to be dependent on the source of the product and its de ee of perfection. ... 

To express theoretically the relations involved, we follow the treatment given by Flood and by Flood and Bruun. TheworkofVaslowand Boyd may be consulted for a more complete thermodynamic consideration of silver chloride-silver bromide equilibria. An equation for the distribution ratio D corresponding to Equilibrium (9-6) can be obtained in terms of solubility products. First, consider the solid to be an impure silver bromide, with chloride as a foreign ion. Thus,... 

In measurements with ion-selective electrodes, interference by other ions is expressed by selectivity coefficients as in Eq. (17). If the nature of the ion-selective membrane is known, these interferences may easily be estimated. For example, in the determination of chloride with a Cl -selective electrode containing AgCl as the electroactive component in its membrane, concentrations of bromides or iodides (generally X ) must be controlled because they form less soluble silver salts than AgCl the solubility products of corresponding silver halides are used in Eq. (20) to estimate the selectivity coefficient ... 

Triphenylethylsilicane is formed by the action of zinc ethyl on triphenylsilieon bromide. Two products are formed, triphenylethyh silicane and triphenylsilicane the first is soluble in cold acetone, and the second soluble only with difficulty. Triphenylethylsilicane forms plates, M.pt. 72° to 74° C. It may also be prepared from triphenyl-silicon chloride, using excess of ethyl magnesium bromide. ... 

Lead diphenyl di-a-naphthyl, Pb(C6ll5)2(CioH7)2. This is obtained as a snow-white, granular, crystalline powder by the interaction of lead diphenyl dibromide and magnesium a-naphth d bromide. The product melts at 197° C., lead separating at a higher temperature, and it is soluble in ether, benzene, or hot alcohol. It reacts with thallic chloride according to the equation ... 

Other Alkylation Experiments. In other experiments lithium and sodium were used in place of potassium. Biphenyl and anthracene were used in place of naphthalene. 1,2-Dimethoxyethane was used in place of tetrahydrofuran. Butyl chloride, butyl bromide, butyl mesylate, butyl triflate, methyl iodide, and octyl iodide were used in place of butyl iodide. The conditions used in these experiments were very similar to the conditions used in the procedures described in the previous paragraphs. The isolation procedure was modified in those cases where the ionic salt, e.g., sodium iodide, was soluble in tetrahydrofuran. In these instances the tetrahydrofuran-soluble product was washed with water to remove the salt prior to further study. 

Water-soluble polyether tin hydride and the bis(2-cardoxyethyl)tin hydroxide allowed reductions and cyclizations to be carried out in water with easy separation from organic soluble products. The latter tin reagent is generated in situ and has not been characterized, but may be a multiplicity of tin oxides and hydroxides. It is soluble in dilute alkali and catalyzes the reduction of alkyl and aryl bromides in the presence of NaBH4 and the water-soluble initiator 4,4 -azobis(4-cyanovaleric acid) (AVCA). 

Silver(I) forms a dithiosulfato complex for which /32 = 2 x 10 in dilute aqueous solution at 25 °C. Given that the solubility product of AgBr is 5.3 x 10 (and assuming that ionic strength effects are negligible), show that the minimal total concentration of Na2S203 needed to dissolve 1.00 g silver bromide in 1.00 L of water at 25 °C is 0.0123 mol L . Note that Na+ is introduced simply as the counterion of 8203 and does not enter into the calculations. 

According to Fig. 1.3.4, in order to determine the oxobasicity index of NaBr with respect to the CsCl-KCl-NaCl eutectic it is necessary to know, at least, two experimental magnitudes. The first set is the oxobasicity index of NaCl, and the difference of pK of CO dissociation in molten NaBr and NaCl. The second set is the difference of pKof CO > dissociation in molten CsBr-KBr-NaBr and CsCl-KCl-NaCl and the difference of pPMeo in molten CsBr-KBr-NaBr and NaBr. The former case is obviously more convenient since the investigation of the oxide solubility products in molten bromides and iodides is more complicated than the determination of the pK of CO in the said melts. 

We have also investigated the solubilities of MgO and CaO in molten potassium halides at 800 °C [197] to elucidate the effect of anion composition of the halide melt on metal-oxide solubility. The MgO was found to be practically insoluble in chloride and bromide melts, and the iodide-melt could not be investigated owing to intense iodine evolution from strongly acidic solutions. In contrast, CaO solubility products were determined successfully in all the potassium halide melts at 800 °C, by the potentiometric titration method. The corresponding potentiometric titration curves are shown in Fig. 3.7.16. 

The solubilities of metal-oxides (on the molar-fraction scale) in chloride melts possessing practically the same oxobasicity-index values are close. This shows the negligibly small effect of low-acidic constituent cations of the melt on its acidity and the solubility product values owing to the levelling of their acidity by that of the most acidic cation of the melt. The solubilities of the oxides in bromide and iodide-melts are considerably lower than those in chloride melts. This may be explained by the stronger association of bromide and iodide ionic melts, and by weakening of the stability of the complexes formed by the hard bases which most cations belong to, with the intermediate (Br ) and soft (I-) bases. 

After correcting for the conductivity of the solvent, the conductivity of a saturated solution of silver bromide in water is 6.99 x 10 S cm at 18°C. If the molar ionic conductivities of Ag" (aq) and Br (aq) are 53.5 and 68.0 S cm mol respectively, find the solubility of silver bromide in water. From this calculate the solubility product for silver bromide. 

The standard potential of the silver/silver bromide electrode is 0.073 V. Calculate the solubility product of silver bromide. 

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