INORGANIC PERBROMIDE COMPOSITIONS AND METHODS OF USE THEREOF

Abstract: A process for leaching platinum and palladium wherein an aqueous leaching solution containing bromine and bromide ion contacts a precious metal source to produce an aqueous leachate. A precursor composition for producing an aqueous leaching solution for leaching platinum and palladium. A process for electrogenerating bromine and a process for leaching platinum and palladium wherein bromine is electrogenerated and contacts a precious metal source to produce an aqueous leachate. A process for leaching gold, silver, platinum and palladium wherein bromine is electrogenerated from a solution containing chloride ions and bromide ions.

Description: INORGANIC PERBROHIDE COMPOSITIONS AND METHODS OF USE THEREOF FIELD OF THE INVENTION This invention relates to compositions containing inorganic perbromides and having desirable physical characteristics such as high bromine levels and low bromine vapor pressures. The invention further relates to the use of such compositions for the recovery of precious metals, including platinum and palladium, from a variety of sources thereof. The invention further relates to a method for the electrolytic production of bromine solutions, and to the use of electrolytically produced from mixed halide bromine solutions in applications including precious metal recovery and water treatment. DESCRIPTION OF THE PRIOR ART It is desirable in a number of applications to have a source of bromine in high concentration, but without requiring the handling of liquid bromine or solutions having a substantial bromine vapor pressure. While various bromine compositions have been proposed in the prior art, many of these have had disadvantageous physical properties such as high bromine vapor pressures, high thermodynamic crystallization temperatures or poor freeze/thaw stability. Bromine solutions have been used for the recovery of certain precious metals. Prior art recovery processes using molecular bromine have been effective, but pure bromine is a corrosive, fuming liquid which generates a suffocating vapor and must be subjected to special handling. Bromine can be dissolved in water to a certain extent, but the resulting solutions exhibit a substantial bromine vapor pressure. Molecular bromine can be generated from the acidification of alkali metal bromates, but by themselves bromates provide only a limited source of molecular bromine, and bromate salt solutions have a high crystallization temperature which makes them inconvenient to use as leaching agents for precious metals. BRIEF DESCRIPTION OF THE DRAWINGS Fig. 1 is a schematic illustrating the electrogeneration process of the invention; Fig. 2 is an illustration of a cell assembly that is 5 especially preferred for use in the practice of the process of the invention; Fig. 3 is a general schematic showing the application of electrogeneration of bromine to the recovery of gold from a source material; 10 Fig. 4 is a more detailed schematic showing the application of the electrogeneration process of the invention to recovery of gold from ore; Fig. 5 is a schematic flow sheet of an alternative embodiment of the rocess for recovery of gold 15 in which an aqueous bromine leaching solution is circulated between a leaching tank and an electrogeneration system; Fig. 6 is a schematic flow sheet showing the application of the principles of the process of Fig. 11 to a 20 continuous cascade leaching reactor system; and Fig. 7 is an Eh/pH diagram for the system H 2 O-10 "4 M Pd-O.IM Br " . Fig. 8 is an Eh/pH diagram for the system H 2 O-10" 4 M Pt-O.IM Br " . 25 Fig. 9 illustrates an especially preferred embodiment of the invention in which an aqueous leaching solution containing bromine is produced at the anode of a divided electrolytic cell and gold is recovered from a pregnant leach solution by electrowinning at the cathode of 30 the same cell. Corresponding reference characters indicate corresponding parts in the several drawings. DESCRIPTION OF THE PREFERRED EMBODIMENTS In accordance with the invention, inorganic perbromide concentrates have been discovered which may be used advantageously in a variety of applications. In certain methods of use, such as the recovery of platinum and palladium from ores, these concentrates may be diluted with water to provide aqueous working solutions that are used in practicing the method. Although the concentrates generally contain a substantial percentage of equivalent molecular bromine, they exhibit remarkably low vapor pressures. Moreover, concentrates of high equivalent bromine content exhibit remarkably low vapor pressure not only in those embodiments in which the pH is in the range of 6.5 to 7.5 but also in those concentrates of the invention which are quite acidic (as low as zero or less) . These combined properties facilitate handling of the concentrates and avoid the hazards that are normally expected in applications where molecular bromine is used. A number of the compositions are advantageously adapted for shipping, storage and/or use in harsh climates. Various of these concentrates exhibit favorable freeze/thaw stability, and certain of them exhibit exceptionally low thermodynamic crystallization temperatures. The compositions are inorganic perbromides which have been discovered to exhibit exceptionally low vapor pressures at, alternatively, pH below 1.0 or pH in the range of 6.5 to 7.5. The inorganic perbromide concentrates with acidic pH ranges include a hydrogen halide acid component, while those stable within a pH range of 6.5 to 7.5 include a bromate salt component. The latter concentrates containing bromate may optionally be converted to acidic concentrates by addition of an acid to the concentrate. Generally, the acidic compositions of the invention are formulated from a metal bromide, a hydrogen halide acid, molecular bromine, and a protic solvent. The protic solvent may be water, alcohol or an organic acid, or a mixture thereof. Compositions of the invention may contain 10-40% by weight equivalent molecular bromine, defined in molar terms as the sum of the actual molar concentration of molecular bromine, the molar concentration of perbromide ion, the molar concentration of hypobromous acid, and the molar concentration of hypobromite ion. Hypobromous acid and hypobromite are produced in the equilibrium reaction: Br 2 + H 2 0 -H + + HOBr + Br " (1) HOBr , H + + OBr " (2) In accordance with the invention, it has been found that concentrates containing 25% or more equivalent molecular bromine exhibit remarkably low bromine vapor pressures, excellent freeze/thaw stability, and exceptionally low thermodyamic crystallization temperatures. Advantageously, the molecular bromine concentration of the acidic concentrates is between about 30% and about 36% by weight. Each of these acidic compositions is prepared by mixing a source of halide ion with molecular bromine in such proportions that the halide ion is in excess. Halide sources generally include both a metal halide salt and a hydrogen halide. Preferably, the halide ion is bromide and the molar ratio of bromide ion to molecular bromine in the formulation is between about 1.2:1 and about 2.0:1, most preferably between about 1.4:1 and about 1.8:1. In solution, the molecular bromine combines with bromide ion to form perbromide or a mixed perhalide ion in accordance with the equations: Br " + Br 2 = Br 3 " (3) or CI " + Br 2 = ClBr 2 ~ (4) By control of the ranges of proportions of bromide ion (and other halide ion), complementary countercation, and molecular bromine used in formulating the composition, it has been found that a solution of low vapor pressure can be produced at both high concentrations of equivalent Br 2 and very low pH, i.e., zero or below. Among the metal bromides which can be incorporated in the composition of the invention are alkali metal salts such as sodium bromide, potassium bromide, and lithium bromide, and alkaline earth metal salts such as calcium bromide. Hydrogen halides used in preparing the composition include HC1, HI and, preferably, HBr. Optionally, the acidic concentrates of the invention further contain an alcohol or a low molecular weight organic acid. Alcohols and organic acids have a lower dielectric constant than water. Because the equilibrium constant for the above reactions increases with the reciprocal of the dielectric constant, the inclusion of an organic solvent in the composition also conduces to maintaining a low bromine vapor pressure at a high molecular bromine concentration. Useful organic acids include acetic, propionic, succinic, adipic and the like. Useful alcohols include methanol, butanol, and the like. It is known that compositions containing alcohol and bromine can be unstable, under certain circumstances explosive, due to reaction of alcohol with bromine. Thus, it is generally preferred that organic solvents other than alcohols be used. However, as explained by Bowman, et al. "A Potential Hazard in Preparing Bromine-Methanol Solutions," J. Electrochem. Soc. Vol. 137- No. 4 (April 1990) 1309-11. Br 2 /alcohol compositions can be stable, and used safely, if the alcohol content is sufficiently low. Bowman, et al. report that methanol/Br 2 compositions are essentially nonreactive, provided that the alcohol content is less than 10% by volume on an alcohol + Br 2 basis. Compositions used in the invention which contain hydrobromic acid and an organic protic solvent are generally formulated from: Br 2 10-40% by wt. Metal bromide 4-30% by wt. HBr 5-24% by wt. Organic solvent 10-40% by wt. Water is optionally present as a co-solvent. Preferred compositions are formulated from: Br 2 20-35% by wt. Metal bromide 8-16% by wt. HBr 10-20% by wt. Organic solvent 15-30% by wt. These compositions exhibit a bromine partial vapor pressure not greater than about 40 mm Hg at 25% bromine and 20°C, and a bromine vapor pressure not greater than about 50 mm Hg at 34% bromine and 20°C Thermodynamic crystallization temperatures are in the range of between about -30°C to about -50°C at 34% Br 2 for compositions in which water is the solvent, and between about -55°C and about -68°C for compositions in which the solvent comprises an organic solvent. The— H is less than 1.0 and generally less than 0.20. Preferred compositions have a pH <0. Regardless of whether the solvent comprises 25 water, an organic acid, or a mixture thereof, it is especially preferred that the Br 2 concentration be greater than 25%. Such compositions are formulated from: Br 2 > 25% by wt. HBr 4-20% by wt. Metal bromide 4-15% by wt. [Br " ]/[Br 2 ] 1.2-2.0 (molar ratio) Protic solvent balance The pH is <0. More preferably, such compositions are formulated from: Br 2 25-35% by wt. HBr 10-20% by wt. Metal bromide 10-15% by wt. [Br"]/[Br 2 ] 1 * 4-1.8 (molar ratio) Protic solvent balance Again, the pH is <1.0. Advantageously, such formulations may contain > 30%, optimally 32-36% Br 2 , and a molar excess of bromide over bromine of > 30%. Similar compositions in which HC1 is substituted for HBr are preferably formulated from: Br 2 >25% by wt. HC1 >4% by wt. Metal bromide 10-15% by wt. [H 2 0]/[NaBr] >4.0 (wt. ratio) and have a pH <0. In the NaBr 3 compositions, it is particularly preferred that the sodium ion content of the formulation be in the range of between about 1% and about 3% by weight, and that the molar ratio of Na + to equivalent Br 2 be no greater than about 0.8. It has been found that such relatively low proportions of Na + conduce to a relatively low thermodynamic crystallization temperature, and to excellent freeze/thaw stability of the concentrate. A preferred formulation for a freeze/thaw stable NaBr 3 concentrate is: NaBr 5-15% HBr 15-30% Br 2 25-35% H 2 0 balance An especially preferred low Na + acidic composition comprises: NaBr 5-10% HBr 17-27% Br 2 30-35% H 2 0 balance Calcium bromide compositions exhibit exceptionally low vapor pressure at high equivalent molecular bromine concentrations and low pH. This is believed to be attributable to the greater ionic strength of calcium bromide as compared to alkali metal bromides. Greater ionic strength tends to increase the equilibrium constant for the reactions: Br " + Br 2 = Br 3 " (3) or CI " + Br 2 = ClBr 2 " (4) At an equivalent molecular bromine concentration of 25%, the Ca(Br 3 ) 2 acidic concentrates have a bromine partial vapor pressure of less than about 40 mm Hg at 20°C, while at 34% equivalent molecular bromine, they have a bromine partial vapor pressure of less than about 50 mm Hg at such temperature. Additionally, calcium perbromide compositions provide especially low thermodynamic crystallization temperatures (TCTs), e.g., in the range of between about -50°C and about -60°C where water only is the solvent, and below -60°C where the solvent comprises an organic solvent. Such TCTs are also believed to be attributable to the greater ionic strength of these formulations as compared to alkali metal perbromides. Calcium perbromide compositions preferably are formulated from: Br 2 >25% by wt. CaBr 2 >5% by wt. HBr >10% by wt. [Br " ]/[Br 2 ] 1.4-1.8 (molar ratio) and have a pH <1.0 The acidic concentrates described above are preferably prepared by adding the bromide or other halide salt and hydrogen halide to a protic solvent, and then adding liquid bromine to the acidic bromide salt solution. This sequence insures the presence of an excess of bromide ion for reaction with the liquid bromine to form perbromide or XBr 2 " ion (where X is halide) during bromine addition. Advantageously, saturated or nearly saturated premix solutions are prepared for both the bromide salt and hydrogen halide, and these premix solutions are added to water to produce a precursor solution to which the liquid bromine is added. Thus, for example, a solution containing an organic protic solvent may be prepared by mixing in the following sequence: 10.to 40 wt.% organic solvent 8 to 45 wt.% 46% by weight NaBr solution 10 to 50 wt.% 48% by weight HBr solution 10 to 40 wt.% liquid bromine or 10 to 40 wt.% organic solvent 8 to 40 wt.% 52% by weight CaBr 2 solution 10 to 50 wt.% 48% by weight HBr solution 10 to 40 wt.% liquid bromine or 10 to 40 wt.% organic solvent 10 to 50 wt.% 38% by weight KBr solution; 10 to 50 wt.% 48% by weight HBr solution 10 to 40 wt.% liquid bromine or 10 to 40 wt.% organic solvent 7 to 35 wt.% 54% by weight LiBr solution 10 to 50 wt.% 48% by weight HBr solution 10 to 40 wt.% liquid bromine Where water alone is the solvent, an NaBr 3 concentrate is preferably prepared by mixing: 6 to 40 wt.% water 9 to 35 wt.% 46% by weight NaBr solution 10 to 50 wt.% 48% by weight HBr solution >25% by wt. liquid bromine Further included in the compositions of the invention are hydrogen perbromide concentrates formulated from: Br 2 > 15% by wt. HBr 15-40% by wt. Organic solvent 40-60% by wt. Where water alone is the solvent, the composition preferably contains: Br 2 > 25% by wt. HBr 30-40% by wt. At a bromine concentration of 25% and a temperature of 20°C, these HBr 3 compositions exhibit a bromine partial vapor pressure of less than about 40mm Hg. It should be noted that the compositions of the acidic concentrates of the invention, as outlined above are formulations, i.e., summaries of the components " from which the concentrates are formed in the relative proportions used in forming the concentrates. As indicated, these formulations _ equilibrate to convert Br 2 and Br " to Br 3 " . Additionally, some of the Br 2 reacts with water to produce hypobromous acid, which in turn dissociates to a limited degree: Br 2 + H 2 0 > H + + HOBr + Br ' (1) HOBr _. > H + + OBr " (2) Based on known equilibrium constants, the exact equilibrium composition of each of the formulations can be computed. This invention encompasses such equilibrated compositions, however produced. However, for purposes of clarity and simplicity, certain of the concentrates are defined in terms of their formulation from water, bromide salt, hydrogen halide and liquid bromine in the manner described above. •In a further and distinct aspect of the invention, inorganic perbromide concentrates have been discovered which have a relatively high pH (about 6.5 to about 7.5), and include a bromate ion component. These compositions (hereinafter "alkaline") may be prepared by mixing a perbromide salt component solution and a bromate component solution. The concentrates of this embodiment are particularly suited for dilution with water to produce a leaching solution for recovery of platinum and palladium. The remarkably low vapor pressure of the alkaline concentrates facilitates their handling and minimizes hazards of using molecular bromine for such purposes. In particular, dilution of the alkaline concentrate to produce the leaching solution can be carried out without any serious problem of containment of bromine vapor. Use and handling of the alkaline concentrate are not hampered by bromate salts crystallizing or otherwise precipitating from the solution. The leaching solution prepared from this concentrate has been demonstrated to be highly effective. In accordance with a particularly preferred embodiment of the invention, a leaching solution precursor concentrate containing perbromide and bromate salts is initially produced. In the preparation of the leaching solution of the invention, this concentrate is diluted to provide the leaching solution. If desired, the pH may be adjusted either before or after dilution by addition of an acid such as HBr, HC1, H 2 S0 4 , or Cl 2 , or a base, such as NaOH, KOH or Ca(0H) 2 . In the preparation of the alkaline concentrates, a component solution of an alkali metal or alkaline earth metal perbromide is mixed with a component solution of alkali metal or alkaline earth metal bromate. The perbromide solution is prepared by addition of bromine to an aqueous solution of a bromide ion as discussed above regarding the preparation of the acidic perbromide concentrates. For example, sodium perbromide and calcium perbromide are prepared by saturating the Br 2 content of the respective aqueous NaBr or CaBr 2 5 solution with molecular bromine: NaBr + Br 2 ^ NaBr 3 (5) 10 CaBr 2 + 2Br 2 .. Ca(Br 3 ) 2 (6) When prepared in the course of providing this composition, the metal bromide solution initially has a concentration of at least about 25% by weight, preferably essentially saturated to its solubility limit, i.e., 45-50% by 15 weight in the case of NaBr, or 55-60% by weight in the case of CaBr 2 . Whatever the initial concentration of the metal bromide solution, liquid or vapor Br 2 is added to the solution to the extent of saturating the bromide ion therein, i.e. in full stoichiometric equivalence with the Br " content. Where 20 the Br 2 is added to a NaBr solution that is initially at its solubility limit, the amount of bromine introduced, as may be determined by iodometric titration, is equivalent to a weight concentration in the resulting perbromide solution of about 40-50% Br 2 . Because of the reversibility of the reactions of 25 equation 3 (as reflected in equations 5 and 6) , a portion of the bromine is present as Br 2 , but most is present as Br 3 " . In a solution saturated with respect to both initial NaBr solubility and bromination of Br " ion, the equilibrium is such that the solution contains about 63-64% by weight NaBr 3 , 4 to 304.5% Br 2 and 2.5 to 3% NaBr. The alkali metal or alkaline earth metal bromate component solution is prepared by addition of liquid bromine or bromine vapor to an aqueous solution of metal hydroxide, most preferably an alkali metal hydroxide. Hydroxyl ions and 35 molecular bromine react in accordance with the following equation to produce both bromate and bromide ions: 3Br 2 + 60H" > 5Br " + Br0 3 " + 3H 2 0 (7) Under alkaline conditions, this reaction proceeds essentially quantitatively to the right. Preferably, the strength of the initial caustic (or other alkaline) solution and the amount of molecular bromine added thereto are controlled so that, when the bromate solution is mixed with the solution of alkali metal or alkaline earth metal perbromide in predetermined relative proportions, the resulting mixture has a pH of between about 6.5 and about 7.5. Where the bromate solution is used in the preparation of a concentrate, the strength of the initial caustic solution and the degree of bromination are selected so that the bromate solution contains at least about 15% by weight equivalent molecular bromine, i.e., at least about 4% by weight bromate ion. Preferably, the bromate solution component of the concentrate contains between about 5% and about 8% by weight bromate ion, roughly equivalent to between about 20% and about 30% by weight molecular bromine. To provide a bromate component solution having such concentration of equivalent molecular bromine and satisfying the stoichiometric requirement set forth by equation 7 the initial concentration of the caustic solution is preferably in the range of 10-20% by weight in the case of sodium hydroxide. Equivalent molar proportions may be computed for other alkalis. Alternatively, the bromate component solution may be prepared by dissolving an alkali metal bromate or alkaline earth metal bromate salt in water. This in fact is the preferred method for preparing a component solution comprising an alkaline earth metal bromate, since difficulty may be encountered in the preparation of such solution by addition of molecular bromine to a lime or magnesia solution or slurry. In this alternative method of preparing the component solution, an alkali metal or alkaline earth metal bromide is also incorporated so as to produce an overall composition essentially equivalent to that obtained by dissolving Br 2 in a caustic solution. In the preparation of the alkaline concentrate, the perbromide solution and bromate solution are mixed in proportions of between about 4 parts by weight perbromide solution per part by weight bromate solution and about 4 parts by weight bromate solution per part by weight perbromide solution. Preferably, approximately equal portions of the two component solutions are mixed. Whatever relative proportions are used, the pH of the resultant composition should be between about 6.5 and about 7.5, and the ratio of the molar concentration of bromate ion to the sum of the molar concentrations of molecular bromine and perbromide ion in the composition is between about 0.05 and about 0.8. Where the bromide ion has been fully saturated with bromine in the preparation of the perbromide component solution, the molar concentration of bromide ion in the alkaline concentrate of the invention is equal to the sum of the molar concentration of molecular bromine and five times the molar concentration of bromate ion. ~~ In the alkaline concentrate, which includes bromate, the bromate ion concentration is at least about 2%, typically ranging from about 2% to about 6% by weight, the equivalent perbromide content is preferably at least about 10%, ranging from about 55% to about 10% by weight, and the concentration of bromide ion (as computed on the basis of no dissociation of perbromide ion) generally ranges from about 3% to about 19%, the preferred compositions thereof typically containing bromide ion weight concentrations in the range of about 6% to about 17%. The equivalent molecular bromine content of the concentrate is between about 10% and about 40%, preferably between about 20% and about 40%, by weight. More preferably, the equivalent Br 2 content is at least about 25% by weight. By using the highly concentrated component solutions as described above, a concentrate can be prepared containing 34% by weight or more equivalent molecular bromine. JLo At the desired pH of between about 6.5 and about 7.5, the molecular bromine content of the concentrate is generally not converted to bromate and bromide, i.e., equation 7 does not proceed appreciably to the right. As a 5 consequence, there is a stable equilibrium between perbromide ion and Br 2 , and the composition of the concentrate is stable within the ranges discussed above. Despite the very high proportions of equivalent molecular bromine, including significant fractions of Br 2 and 10 Br " 3 , it has been discovered that the vapor pressure of this alkaline variation of the composition of the invention is quite low. For example, a concentrate containing about 34% by weight equivalent bromine exhibits a total vapor pressure of only 23mm Hg at 0°C, and a total vapor pressure of only 15 112.5mm Hg at 35°. By comparison, the vapor pressures of liquid bromine are 75mm Hg at 0°C and 357.5mm Hg at 35°C, and the vapor pressures of sodium perbromide are 44mm Hg at 0°C and 214mm Hg at 35°C. Effective aqueous bromine leaching solutions for 20 recovery of precious metals may be prepared by dilution of the alkaline or acidic concentrate of the invention. Prior to or after dilution, the pH may be adjusted by addition of an acid such as H2S04, HBr, HC1, or C12, or a base, such as NaOH or KOH. Where the concentrate is acidified, HBr is preferred 25 over HC1 for most applications. H2S04, however, is the preferred acid for use in connection with palladium and platinum recovery. The leaching solution is effective over a wide range of pH, but operation is preferably carried out at a pH of less than about 6. For platinum and palladium, it is 0 preferred that leaching occur at a pH of less than about 4, more preferably less than about 1, most preferably less than about 0. In all cases, an acidic pH is generally preferred to promote the conversion of bromate ion to molecular bromine. Compositions used for dissolution of Pd and/or Pt preferably 5 contain between about 1 and about 8 equivalents acid per liter of solution. Sul uric acid is preferred. Where sulfuric acid is the acid used to provide the desired acidity, it is preferably present in a proportion of between about 5% and about 40% by weight, more preferably between about 5% and about 30% by weight, most preferably between about 10% and about 20% by weight. Where a bromate/bromide concentrate of alkaline or neutral pH is used, acidification is preferably carried out prior to dilution, thus producing an acidic concentrate having a pH of less than about 2.5, and an equivalent molecular bromine concentration in the range of between about 28% and about 40% by weight. In conjunction with dilution, a portion of NaBr or other halide salt may be advantageously incorporated into the solution. The rate of dissolution of certain metals in the leaching solution is in some instances accelerated if the solution contains halide ions in a concentration that is even higher than that provided by a bromine saturated concentrate, in which instance, preparation of the leaching solution preferably involves incorporation of chloride salt or bromide salt from a source other than the concentrate. It may be noted that both the actual molecular bromine and the ultimate bromide ion content are also affected by the shifts in equilibria which accompany the acidification and dilution process. Thus, equations 3, 5 and 6, supra, are driven to the left,converting perbromide ion to bromide and molecular bromine; equation 7 is also driven to the left, converting bromate ion and bromide ion to molecular bromine. Dilution tends to drive equation 1 to the right, resulting in conversion of molecular bromine to bromide ion and hypobromous acid. As a net result, the hypobromous acid concentration is a significant component of the equivalent molecular bromine content of the leaching solution. It may further be noted that Eh/pH diagrams constructed from thermodynamic data show a progressively larger solubility field at lower Eh values for the formation of the complex ions (see equations 10-13 infra) as Br- ion concentration increases from 10 "5 to 1.0M. These observations are consistent with the requirement for multiple Br " ions to form the complex anions PdBr 4 2" , PdBr 6 2" , and PtBr 6 2" . It may be noted that, where the dilution ratio is modest, for example, 15:1 or less, the acidic or alkaline concentrate of the invention typically furnishes sufficient Br " ion to fully satisfy the requirement for co-ordinating the metal. At higher ratios of dilution, addition of supplementary bromide salt may be needed. Stoichiometrically, the proportion of Br " , the Br " /metal ratio, and the Br " /Br 2 are greater for Pd and Pt than for Au, but as a practical matter, dilutions may more often be appropriate in preparing leaching solutions for sources such as low grade ores, in which instance the addition of supplementary bromide salt may be necessary. Where a precursor concentrate or leaching solution is acidified by addition of Cl 2 , not only the bromate but the bromide ion content thereof are converted to molecular bromine. This may further enhance the oxidizing and complexing power of the leaching solution for leaching of platinum and palladium from a source material. Water, and optionally the halide salt, are mixed with the concentrate in such relative amounts that the equivalent molecular bromine content of the leaching solution is between about 0.01% and about 20% by weight equivalent molecular bromine, between about 0.005% and about 20% by weight bromide ion, and between about 0.005% and about 30% by weight total halide ion. Where low grade sources, such as typical low grade ores are leached, the solution preferably contains between about 0.01% and about 1% by weight, more preferably about 0.02% to about 0.5% by weight, equivalent molecular bromine, between about 0.005% and about 10%, more preferably about 0.01% to about 1%, by weight bromide ion, and between about 0.005% and about 15%, preferably about 0.01% to about 1.5%, by weight total halide ion. However, in certain applications such as, for example, recovery of Pd from spent catalyst, or recovery of Pt/Pd from high grade concentrates, a more concentrated leaching solution may be used to advantage. Such may be prepared from the above described concentrates by modest dilution with water. For example, a 0.5% Pd on alumina catalyst, or a concentrate containing 30-50 oz. Pd per ton, may advantageously be leached with a solution prepared by diluting a Br 2 concentrate of the invention to an equivalent molecular bromine content of between about 8 and about 25 gpl, a Br " content of between about 5 and about 20 gpl, and a total halide content of between about 10 and about 40 gpl. Platinum and palladium are recovered from a source thereof, such as comminuted ore, by contacting the source material with the aqueous bromine leaching solution. In the case of platinum, oxidation and complexing of the platinum is believed to proceed in accordance with the equations: Pt + 2Br 2 + 2Br " > PtBr 6 2" (10) or Pt + 2H0Br + 4Br " > PtBr 6 2" + 2H 2 0 (11) In the case of palladium, oxidation and complexing of the palladium is believed to proceed in accordance with the equations: Pd + Br 2 + 2Br " > PdBr 4 2" (12) or Pd + HOBr + 3Br " --> PdBr 4 2" + H 2 0 (13) Depending on the nature of the ore, the relative proportions of ore (or other source material) and leaching agent may be such that the leaching slurry contains between about 1 and about 600 lbs. active agent per ton of source. Active agent in this instance is defined as the sum of the amounts of bromide, perbromide, metal hypobromite, hypobromous acid, and molecular bromine in the leaching solution. For recovery of Pd metal from a catalyst support, the Br 2 /Pd molar ratio is preferably between about 1 and about 8, and for recovery of Pt and Pd from high grade concentrates containing, for example 30-50 oz. Pd per ton, the molar ratio of Br 2 /Pd+Pt is preferably between about 2 and about 40. For dissolution of Pt from a Pt compound such as a platinum oxide, an oxidation reduction potential of about 850-1250 mV is required. The oxidation reduction potential required to dissolve Pd is about 500-750 mv. As a consequence Pd may be leached with solutions containing only HBr, sulfuric acid, and optionally another source of bromide or other halide ion. For example, a leaching solution for Pd may contain between about 10 and about 20 % by weight sulfuric acid, between about 15 and about 30% by weight HBr, between about 10 and about 25% by weight total bromide ion, and between about 20 and about 40% by weight total halide ion. However, the presence of Br 2 in the proportions outlined above is preferred for complete, rapid and efficient leaching. If the source material is a refractory ore, it may be necessary to pretreat it for removal of sulfide and carbonaceous material. Such may be accomplished by methods known to the art such as roasting or pressure oxidation. Roasting may be sufficient pretreatment if carried out at a temperature of at least about 500°C. For the recovery of palladium from certain sources, it has been discovered that recovery may be improved if the ore is roasted at a temperature of at least about 900°C, preferably at least about 1000°C. For the recovery of platinum, roasting at a temperature in the range of about 500°C to about 750°C is preferred. If pressure oxidation is performed, it is preferably in an autoclave under 150-300 psi oxygen pressure and at a temperature in the range of from about 150°C to about 220°C. The composition and method may be used for recovery of silver from various sources, including photographic film. The composition and method may also be used for recovery of platinum and/or palladium from ores, Pd catalysts and other sources. The slurry of ore in leaching solution is preferably agitated to promote transfer of the precious metals to the aqueous phase. A leachate is thus produced containing platinum or palladium complexed with bromide ions. Although stated here in the alternative, it will be understood that many sources may provide leachates containing combinations of platinum group metals. For platinum and palladium, leaching may be carried out for up to about 20 hours or longer, preferably for about 4 to about 15 hours, more preferably for about 6 to about 10 hours. For sources containing platinum, leaching is preferably carried out at a temperature in the range of from about 50°C to about 120°C, more preferably from about 60°C to about 90°C, most preferably from about 80°C to about 90°C. After treatment of the metal source with the leaching solution is completed, the leachate is separated from the leached ore, catalyst substrate or other residue, as by filtration. The filter cake is washed with an aqueous washing medium, the spent wash solution is combined with the filtrate (leachate), and the combined filtrate and wash solution is treated for recovery of the metal therefrom. Advantageously, particularly in the case of silver, the filter cake is washed with a 2-4 molar HC1. Washing the filter cake in such fashion may be effective to remove further quantities of silver in the form of AgCl 2 ~ from the cake. A washing solution of 4M HC1 is especially preferred. Platinum and palladium may be recovered from the combined filtrate and wash solution by conventional means such as solvent extraction, ion exchange and precipitative methods. Further in accordance with the present invention, it has also been discovered that bromine can be generated in aqueous solution to produce an aqueous bromine solution, and that the bromine solution generated can be used in an economically advantageous process for the leaching of platinum and palladium from sources thereof. This solution has been demonstrated to be effective for recovery of these metals from ores in high yield and at commercially acceptable leaching rates. By controlling the relationship between current and the flow of electrolytic solution through the electrogeneration system, high current efficiencies can be realized in the process of the invention. By controlling the composition of the solution entering the electrogeneration system and creating sufficient turbulence in the system to minimize overvoltages, the power consumption per unit weight of bromine produced is maintained within acceptable limits. Where the aqueous bromine solution is used for leaching of precious metals, separation of product from the leaching solution produces a depleted bromide solution which can be recycled to the electrogeneration step. Unreacted bromide ion is thus reclaimed for conversion to bromine, thereby limiting the consumption of reagents and making it possible to operate a recovery process at lower reagent cost than a conventional cyanide or other recovery process. As a result, the process can be used in the recovery of precious metals from ores and other sources at operating costs that are quite competitive with the cyanide process. Fig. 3 is a schematic flow sheet of the electrogeneration process. A bromide solution prepared in a makeup tank 101 is transferred by a pump 103 to an electrolytic cell 105. Power is applied to the cell by a direct current power source 107 via an anode 109 and a cathode 111. The cell shown in Fig. 3 is an undivided cell, i.e., it contains no diaphragm or other impediment or obstruction to flo of electrolytic solution sufficient to cause a discontinuity in the concentration gradient between the anode and the cathode. Bromine is generated at the anode by the reaction: 2Br " / Br 2 + 2e " (14) Hydrogen is generated at the cathode by the reaction: 2H + + 2e " / H 2 (15) or 2H 2 0 + 2e " > H 2 + 20H ' (15A) Although a single cell is illustrated in Fig. 3, it will be understood that the electrogeneration system may comprise a cell bank containing a plurality of cells. The cells of such a system may be arranged in a variety of ways, but are preferably connected electrically in series. Depending on production requirements, the desired equivalent bromine concentration of the product solution and electrical design considerations, several banks of cells may be used with the cells of each bank electrically in series, and the banks arranged either in series or in parallel with respect to each other. Depending on production requirements, the desired equivalent bromine concentration of the product solution, and the relationship of electrode area to flow of electrolytic solution, the cells may be hydraulically in series or hydraulically in parallel. The feed solution entering the cell (or cell bank) from tank 101 has a pH of between about 0 and about 6, preferably between about 0 and about 3, and contains between about 0.5 and about 8.8 moles/1, preferably between about 0.5 and about 5 moles/1, bromide ion. Where a relatively concentrated product solution is desired, such as that suitable, for example, in the recovery of Pd from a catalyst substrate or high grade concentrate, the feed solution preferably contains between about 0.25 and about 2.5 moles per liter bromide ion. Where a the product solution is used to treat a low grade source, filter cake losses of bromide may be minimized by operating with a somewhat weaker feed solution, for example, a solution containing between about 0.0125 and about 0.625 moles per liter bromide solution. The feed solution may be prepared by dissolving an alkali metal bromide in water and acidifying with an acid such as HBr, sulfuric acid, or HC1 to the desired pH. Thus, the solution may contain between about 0.5 and about 8.8 moles/1 of sodium ion. Turbulent flow velocity and/or mechanical agitation in the electrode region is established at a level sufficient to minimize overvoltages and maintain the individual cell voltage in the range of between about 4 and about 5 volts at a current density in the range of between about 1.0 and about 4.0, preferably between about 2.0 and about 4.0, more preferably about 2.5 and about 3.0, kA/m 2 . Preferably, feed solution is introduced into the cell at essentially ambient temperature. Temperature rise in the cell (or bank of cells) is in the range of between about 4°C and about 20°C. Preferably, conditions are controlled to avoid increase of the cell discharge solution temperature to greater than about 50°C. High current efficiency is maintained by controlling the relationship between current and the throughput of electrolytic solution through the system so that the conversion of bromide ion during passage through the cell bank is between about 4% and about 50%, preferably between about 5% and about 40%. For satisfactory productivity, the current density should be in the range of between about 2.0 and about 4.0 kA/m 2 . The product solution has a pH of less than 6, preferably less than about 4. If the product solution is to be used for the leaching of platinum or palladium, it has a pH of less than about 4, preferably less than about 1, most preferably less than about 0. The product solution contains between about 0.01 and about 3.66 moles/l of equivalent bromine, between about 0.1 and about 4.0 moles/1 unreacted bromide ion, and between about 0.1 and about 4.0 moles/1 alkali metal ion. Preferably, the product solution containing between about Q.03 and about 2.5 moles/1, more preferably between about 0.1 and about 2.0 moles/1, equivalent bromine, between about 0.4 and about 3.0 moles/1, more preferably between about 0.6 and about 2.5 moles/1, bromide ion, and between about 0.4 and about 3.0 moleε/1, more preferably between about 0.6 and about 2.5 mόles/1, alkali metal ion. A solution used for recovery of precious metal from a high grade source preferably contains between about 8 and about 15 gpl equivalent bromine, between about 6 and about 12 gpl Br " , and between about 10 and about 20 halide ion, while a solution used for recovery of precious metal from a low grade source, may suitably contain between about 0.01% and about 1%, preferably between about 0.02 and about 0.5%, by weight equivalent molecular bromine, between about 0.005% and about 10%, preferably between about 0.01% and about 1%, by weight bromide ion and between about 0.005% and about 15%, preferably between about 0.01% and about 1.5%, by weight total halide ion. Product solutions containing more than about 15 gpl equivalent Br 2 can be generated if desired but, in undivided cells, current efficiencies begin to deteriorate at product solution concentrations of around 10 gpl, and fall off sharply at product solution concentrations above about 15 gpl equivalent Br 2 . If divided cells are used, current efficiencies of 90% or more can be realized in the generation of product solutions containing as high as 400 gpl or more equivalent Br 2 . Equivalent bromine is defined as the sum of the molar concentrations of molecular bromine, perbromide ion (Br 3 ~ ), hypobromite ion, and hypobromous acid. It also includes any bromate ion present in the solution, but at the prevailing pH, no substantial bromate ion concentration would be anticipated. The molar ratio of equivalent bromine to bromide ion in the product solution is between about 0.05 and 0.6, preferably between 0.2 and 0.6. Throughout this range, the solution has substantial oxidizing power, but does not have a substantial bromine vapor pressure. Where the solution leaving cell 105 is used in such applications as leaching of ore, a depleted bromide solution is produced which may optionally be recycled to tank 101 where it is replenished by addition of fresh bromide, preferably as hydrogen bromide, alkali metal bromide or a combination thereof, and adjusted with acid or base as necessary to provide a feed solution of the proper pH for electrolysis in cell 105. To provide adequate conductivity and high current efficiency using only bromide ion as the oxidizable electrolyte, it is desirable that the electrolytic solution fed to the cell contain at least about 0.65 moles per liter bromide ion. It will be noted that this is substantially in excess of the bromide content necessary for generation of the 1-5 gpl equivalent Br 2 solutions that are optimal for precious metal sources. In these circumstances, relatively high bromide ion consumption may result from the fraction of Br " in the spent ore residue discarded from the process. In a variation of the electrogeneration process of the invention, bromide consumption and power consumption are both reduced by use of a mixed halide electrolytic solution, specifically a solution containing both chloride and bromide ion. In this embodiment of the invention, the bromide ion content of the cell feed solution is preferably between about 0.065 and about 0.25 moles per liter and the chloride content is at least about 0.56 moles per liter, preferably between about 1.25 and about 2.25 moles per liter. The molar ratio of chloride ion to bromide ion is at least about 10, preferably at least about 25. In the operation of the cell with such feed solutions, a portion of the current is utilized in the oxidation of chloride ion to Cl 2 , but the Cl 2 is quantitatively converted back to chloride by the oxidation of bromide to Br 2 . The mixed halide process is preferably operated at a bromide to bromine conversion in the upper portion of above noted range, generally between about 20% and about 50%, more preferably between about 30% and about 50%. The combination of high conversion and low bromide ion content in the feed solution results in advantageously low Br " consumption. While bromide ion conversion is relatively high, the total halide conversion is preferably in the low end of the 4 to 50% range, preferably between about 5% and about 15%. As a consequence. the mixed halide process can also be operated at high current efficiency and moderate power consumption. By operation at modest current density, for example, in the range of about 1 to about 2 kA/m 2 , the mixed halide process can be operated with very low power consumption. By operation at higher current densities, high productivity is realized with modest power consumption. In one preferred embodiment of the invention, electrolysis is conducted under the following conditions: Feed Solution Composition 5wt% CI " , 0.5wt% Br " Product Solution Composition 0.2wt%Br 2 , 0.3wt% Br " , 5wt% CI " Current Density 100 mA/cm 2 Avg Individual Cell Voltage 2.25 V Electrolysis Time 4 hr Current Efficiency 78% H 2 S0 4 0.4 g dm "3 Br 2 1.75 g dm "3 The bromine-containing product stream produced by electrolysis of the mixed halide stream may then be used in the recovery of precious metals or treatment of water as described herein. As noted above, the electrogeneration system may comprise one or more banks of cells rather than the single cell that is illustrated in Fig. 1. Moreover, the electrogeneration system may operate on a continuous basis as shown in Fig. 1 or on a batch basis in which the electrolytic solution is circulated between the cell(s) and reservoir such as the bromide solution makeup tank until the desired conversion has been realized. In either case the cell(s) preferably operate on a flow basis, but in the latter (batch) case, recirculation is required to reach the desired conversion. Whether operation is continuous or batch, the relationship between electric current and throughput is such that the conversion of bromide ion is in the desired range described herein. It will be understood that, in a fully continuous operation, the throughput is the flow rate through the electrogeneration system, while in a recirculation or other batch operation the throughput is determined from the batch volume and time of application of power to recirculating solution. In order to produce an aqueous bromine leaching solution at competitive cost, it is important that the cells of the electrogeneration system operate with high productivity and high electrical efficiency. High current efficiency is promoted in an undivided cell by operation at low bromide conversions, thereby minimizing the back reaction by which bromine is reduced to bromide ions at the cell cathode. Electrical efficiency is further promoted by the use of cells which are arranged to provide high rates of mass transfer between the bulk solution and the anode, thereby minimizing half cell overvoltage. High productivity is attained through high electrical efficiency, adequate current density, and a high ratio of electrode surface area to solution volume. Preferably, mass transport coefficient (k.,) for transfer of bromide ions from the bulk solution to the anode surface is at least about 5xl0 "4 cm/sec. typically 5xl0 "4 to about 5xl0 "3 cm/sec. for the relationship: where I L is the mass transport limited current density, F is Faraday ' s constant, and C R is the bulk concentration of the bromide ion. The ratio of anode surface to cell compartment volume is preferably at least about 80 cm "1 , more preferably 100-150 cm" 1 . By operation within these parameters, productivities of between about lxl0 "3 and about 5x10 "3 moles Br 2 per hour per cm 3 of working volume in the cell can be achieved. Fig. 2 is a schematic illustration of a type of undivided cell that can be utilized effectively to provide the desired electrical efficiency and productivity discussed above. A cell of the type illustrated is available from Electrocatalytic, Inc., of Union New Jersey under the trade designation "Chloropac". This cell, which was originally developed for generation of hypochlorite in shipboard seawater systems, is described in detail in literature available from Electrocatalytic, Inc. The apparatus depicted in Fig. 2 is a bipolar dual cell assembly which comprises an outer electrode subassembly 113 that includes two outer cylindrical electrodes 115 and 117 that are substantially axially aligned and mechanically attached to each other through an insulating spacer 119. The cell assembly further comprises an inner cylindrical electrode 121 that is of smaller diameter than either of electrodes 115 and 117, is concentric therewith, and is substantially coextensive longitudinally with subassembly 113. The annular space 123 between subassembly 113 and electrode 121 provides the path along which electrolytic solution may be caused to flow through the cell. As illustrated in the drawing, outer electrode 115 serves as an anode to which current is supplied to the bipolar dual cell assembly and outer electrode 117 serves as a cathode from which current is withdrawn. Accordingly, the portion 125 of inner electrode 121 facing anode 115 serves as a cathode and the portion 127 of the inner electrode facing cathode 117 serves as an anode. In a particularly preferred embodiment of the invention, each of electrodes 115, 117 and 121 is constructed of titanium, and both anode 115 and anodic portion 127 of electrode 121 are coated with platinum. The platinized surface catalyzes the anodic reaction and promotes generation of bromine at high current efficiency and minimum overvoltage. In operation of the cell of Fig. 2, an electrolytic feed solution containing bromide ions is caused to flow through annular path 123 between the electrodes and a direct current is applied to the flowing solution. Bromide ions are oxidized to bromine at anodes 115 and 127, while hydrogen is generated in the solution at cathodes 117 and 125. To provide the desired rate of mass transfer from the bulk solution to the anode surface, the velocity through the cell is preferably about 1.22 to 2.44 m/sec, more preferably between about 1.52 and about 2.13 m/sec. Although the cells illustrated in Fig. 2 are particularly preferred, a variety of different cell designs may provide the high rates of mass transfer, even potential and current distribution and high ratio of electrode area to working volume that characterize the Chloropac type unit. As noted, the bromine solution produced in the electrogeneration system is advantageously used for leaching of gold, silver, platinum or palladium from sources thereof. Illustrated in Fig. 3 is a process for recovery of gold which includes a barren or makeup tank 101 in which electrolytic solution is prepared for delivery by a pump 103 to an electrogeneration system 105. Electrogeneration system 105 may consist of a single electrolysis cell or comprise a plurality of banks of cells, but in any case comprises paired anode and cathode means which may be either monopolar or bipolar, and which may be arranged in a variety of electrical and hydraulic configurations as discussed above. Aqueous bromine solution produced in system 105 is transferred by discharge pump 129 to a leaching tank 131 where it contacts a solid particulate source of gold, such as crushed gold ore. This causes the gold contained in the source to react with elemental bromine, perbromide ions, hypobromite ions and bromide ions to produce an aqueous auriferous solution containing AuBr 4 " ions and a particulate residue. The resulting slurry is transferred from tank 131 by a pump 133 through a filter or other solid/liquid separation means 135 for separation of the solid residue from the pregnant leach solution, and thence to a pregnant leach solution tank 137. Gold may be recovered from the pregnant leach solution by a variety of means, including zinc precipitation, carbon adsorption, solvent extraction, electrowinning, or ion exchange. The process of Fig. 3 causes the gold to be removed by ion exchange. Pregnant leach solution is transferred by a pump 139 to a pair of ion exchange columns 141 loaded with an ion exchange resin. AuBr 4 " ions are removed from the solution and collected on the column. Residual bromine in the pregnant leach solution is reduced to bromide ion in the columns. Depleted bromide solution is returned to the barren tank 101, where it is replenished by addition of fresh bromide. A very similar process may be used for the recovery of platinum and palladium from sources thereof. In each case, the electrolytic cells are operated with a feed composition and conversion effective to provide the leaching solution compositions described hereinabove. Sulfuric acid is preferably incorporated in the leaching solution, either by incorporation in the feed solution to the cells or by addition to the product solution to provide a leaching solution. In the case of platinum and palladium, the leaching solution is preferably heated to a temperature of at least about 60°C, preferably to 80-90°C, either in the leaching vessel or immediately upstream thereof. In order to minimize environmental emissions of Br 2 , the cells and the remainder of the system are preferably operated at <50°C. The leaching tank is preferably a closed tank which contains heating coils for heating the leaching slurry to the desired temperature. A heat exchanger in the slurry discharge line from the leaching tank (or filtrate discharge line from the filter) may be provided to cool the Pt bearing leachate. In order to provide the relatively concentrated leaching solutions (8-25 gpl equivalent Br 2 ) that are preferably used in leaching of high grade Pd/Pt ore concentrates, it may be advantageous to use divided cells in order to realize high current efficiencies. An especially preferred gold leaching embodiment of the process of the invention is illustrated in Fig. 4. In this process, which operates on a continuous basis, gold ore is loaded into an ore bin 143 from which it is transferred by a conveyor 145 to a ball mill 147. Milled ore passes to a classifier 149. A fines fraction from the classifier is subjected to leaching for recovery of gold while a coarse fraction is recycled to ball mill 147. The fines fraction is delivered to the first of two cascade agitated leaching tanks 151 and 153 where it is contacted with an aqueous bromine solution. The resultant leaching slurry overflows tank 151 to tank 153 and overflows tank 153 to solids/liquid separation means comprising a thickener 155. Solids residue drawn from the bottom of thickener 155 is passed through a countercurrent washing system comprising thickeners 157, 159, and 161. An aqueous washing medium is fed to the last of the series of thickeners, thickener 161. Solids/liquid contact and separation in each thickener yields a liquid fraction that is transferred to the next thickener nearer the leaching system and a solids fraction which is transferred to the next thickener more remote from the leaching system. Thus, operation of the countercurrent washing system provides a liquid stream which moves with progressively increasing gold content from thickener 161 to thickener 155 and a solids stream which moves with progressively decreasing gold content from thickener 155 to thickener 161. Solid tailings are withdrawn from the bottom of thickener 161. In thickener 155, the wash liquor containing soluble gold recovered from the residue mixes with the pregnant leach solution from leaching tank 153 to produce an auriferous solution that is transferred to ion exchange columns 141. Removal of gold by ion exchange produces a depleted bromide solution which is recycled for use in generating additional aqueous bromine solution. To maintain the water balance of the plant, the depleted bromide solution is concentrated by passing all or part of the solution through a reverse osmosis unit 162. Water removed by the reverse osmosis unit is used in the circuit or purged from the process. The concentrated bromide solution is transferred to the electrogeneration system 163. Electrogeneration system 163 includes a makeup tank (not shown) and one or a plurality of cells in which bromide is converted to bromine as discussed above. The spent bromide solution is replenished by addition of alkali metal bromide and acid in the makeup tank, thus producing fresh feed solution for the cells of the electrogeneration system. The aqueous bromine solution leaving system 163 has the composition described hereinabove and is effective for the removal of gold from ore. This solution is recycled to leaching tank 151 for further recovery of gold from ore. Ion exchange columns 141 contain a commercial anion exchange resin such as the resin comprising secondary amine functional groups combined with a phenol-formaldehyde matrix sold under the trade designations "PAZ-4" by Sela, Inc., the resin comprising trimethylamine functional groups combined with a styrene/divinylbenzene matrix sold under the trade designation "D0WEX-21K" by Dow Chemical Company, and the polyester resin sold under the trade designation "Amberlite XAD-7" by Rohm and Haas. The gold loading capacity of PAZ-4 and D0WEX-21K is in the neighborhood of 80-120 oz./cubic foot, while that of XAD-7 is in range of about 10-20 oz./cubic foot. In batch tests, 80% loading is typically achieved in 1-2 hr. and maximum loading is reached in about 3-6 hr. These data allow specification of ion exchange column height and resin requirements in accordance with conventional design criteria. An acidic ketone solution, for example an acetone/HCl solution, is preferably used for elution of the column. Other eluents such as thiourea/HCl may also be used. Illustrated in Fig. 5 is an alternative embodiment of the invention in which a slurry of leaching solution and particulate gold-bearing material is circulated between a leaching zone (contained within leaching tank 165) and an electrogeneration system 167 by operation of a high volumetric capacity circulating pump 169. In this process, the driving force for gold leaching may be enhanced by maintaining (or restoring) a high bromine content in the leaching solution. Conditions for operation of the cell or cells of the electrogeneration system are comparable to those for the processes of Figs. 3 and 4, except that back mixing in the leaching tank causes the feed solution to the cells to have a somewhat lower bromine content than in the other processes. The latter effect can be minimized by baffling the leaching tank or using a pipe reactor to approach plug flow conditions. As illustrated in Fig. 5, this process operates on a batch basis. However, Fig. 6 shows how the principle of the process of Fig. 5 can be implemented in a continuous operation. In Fig. 6, each of a series of cascaded leaching tanks 165, 171, and 173 is associated with an electrogeneration system, and leaching slurry is circulated between each leaching tank and its associated cell(s) 167, 175, and 177 respectively by means of pumps 169, 179 and 181, while leaching slurry moves forward progressively from tank to tank. Such a scheme may be integrated into the process of Fig. 4, with or without an electrolytic system for regeneration of depleted bromide solution passing from the ion exchange column to the first leaching tank. The processes illustrated in Figs. 3-6 can also be used for the recovery of Pd and Pt from sources thereof. The feed solutions and cell operating conditions are controlled to produce product solutions that have the desired compositions of Pd/Pt leaching solutions, or which may be readily modified to produce such leaching solutions. As noted, leaching solutions for Pd/Pt preferably contain HC1, HBr or H 2 S0 4 , most preferably H 2 S0 4 in a proportion of between about 10% and _ about 20% by weight. To produce the desired leaching solution, acid may be added to either the feed solution or the product solution. Regardless of which acid predominates in the leaching solution HBr is advantageously used for makeup in a recirculating system of the type illustrated in Figs. 3 or 4. Since both H + and Br " are consumed in the process, HBr provides a suitable source of both. Sulfate ion is consumed, for example, through environmental losses, with catalyst substrate or spent ore residue, in the acidulation of a catalyst substrate or ore gangue, or in competition with the complexed metal anion for ion exchanger resin sites. Thus, makeup of sulfuric acid is required. Whatever acid or combination of acids is used, acid makeup may be either before or after electrolysis, but is preferably done before. In providing a leaching solution of the desired combination of pH, sulfate ion content, and bromide ion content, alkali metal bromide is commonly used as a source of bromide ion. Alkali metal is lost only marginally, primarily by environmental losses or with catalyst substrate or spent ore residue. Alkali metal bromide is added to compensate for these marginal losses of alkali metal ion, and is preferably added upstream of the electrolytic cells. In accordance with the invention, electro-generation of bromine to produce an aqueous bromine solution can also be conducted in divided cells. Such process may be carried out in a conventional plate and frame cell construction, using a diaphragm that preferably comprises a cation exchange membrane such as the perfluorosulfonic acid membrane sold under the trade designation "Nafion" by E.I. du Pont de Nemours & Co. The anode is preferably constructed of graphite, vitreous carbon, or the ceramic sold under the trade designation Ebonex by Ebonex Technology, Inc., or platinum, ruthenium dioxide, or iridium dioxide on a titanium substrate. The bromide ion content of the feed solution to the anode compartment of the cell is substantially the same as that of the solution described above for feed to an undivided cell. However, bromide ion can be supplied either in the form of an alkali metal bromide, in which case the pH of the feed solution is between about 0 and about 6, preferably about 0 to about 3, or hydrobromic acid, in which case the pH of the feed solution is approximately 0 or less. A proton source such as sulfuric acid or hydrochloric acid is fed to the cathode side of the cell. Operating conditions are generally the same as described above for undivided cells, except that somewhat higher conversions can be tolerated without loss of current efficiency. Using a divided cell, the conversion of bromide ion in the electrogeneration system is typically between about 4% and about 50%, preferably between 20% and 40%. Thus, the equivalent bromine content of the product solution is between about 0.01 and about 3.66 moles/1, preferably between about 0.4 and about 3.0 moles/1, more preferably between about 0.2 and about 1.0 moles/1. Where an alkali metal bromide is used as the source of bromide ion, the product solution has a pH of between about 0 and about 6, preferably between about 0 and about 3, and an alkali metal ion content of between about 0.1 and about 4.0 moles/1, preferably between about 0.4 and about 3.0 moles/1, more preferably between about 0.3 and about 1.5 moles/1. The product of a divided cell is particularly advantageous in such applications as industrial water treatment, such as cooling tower water, where the higher equivalent bromine concentration facilitates treatment of substantial volumes of water with modest volumes of aqueous bromine solution. It is also advantageous for such leaching applications as recovery of Au from jewelry scraps, Pd from catalyst substrate, and Pt/Pd from high grade ore concentrates. The following examples illustrate the invention. EXAMPLE 1 Precursor compositions were prepared by adding a 48% HBr solution and a 46% NaBr solution to water. Liquid bromine was added to the precursor solution to produce acidic concentrates containing 34% by weight equivalent molecular bromine. Satisfactory solutions were prepared from the proportions of water, HBr solution, NaBr solution and liquid bromine set forth in Table 1. Table 1 These solutions were clear and stable. No phase separation occurred on standing. EXAMPLE 2 Using the method generally described in Example 1, acidic concentrates containing 34% by weight equivalent molecular bromine were prepared from water, a 46% by weight NaBr solution, and a 37% by weight HCl solution. Satisfactory compositions were prepared from the proportions set forth in Table 2. Table 2 Using the method generally described in Example 1, acidic concentrates containing 34% by weight equivalent molecular bromine were prepared from water, a 40 48% by weight HBr solution, a 52% by weight CaBr 2 solution, and liquid bromine. Satisfactory compositions were prepared from the proportions set forth in Table 3. Table 3 Additional compositions were prepared from CaBr 2 , Br 2 , methanol, either HBr or HCl and, optionally, water. Satisfactory compositions were prepared from the proportions set forth in Table 4. Table 4 Acidic concentrates were prepared from water or organic solvent, 46% by weight NaBr solution, 48% HBr solution, and liquid bromine. NaBr and HBr solution were added to the water or organic solvent, and liquid bromine was added at a modest rate to the precursor mixture. The mixture was stirred constantly but not too vigorously during the addition of Br 2 . Four separate concentrates were prepared, each of which was a stable, clear liquid. The partial vapor pressures were measured 24 hours after the concentrates were formulated. The compositions of these concentrates, their bromine partial vapor pressures and the thermodynamic crystallization temperatures are set forth in Table 5. Table 5 Physical and Chemical Characteristics of formulations of Example 4 Comp. Comp. Comp. Comp. Parameters #28 #29 #30 #31 Wt.% H 2 0 — — 6 10 Wt.% Methanol 15 26 Wt.% 46% NaBr, or 52% CaBr 2 , or 38% KBr or 54% LiBr Wt. % 48% HBr Wt.% Br 2 % Available Br 2 by Titration Density (g/mL) Partial Vapor Pressure (mm Hg at 20°C) Crystallization Temp. (°C) pH EXAMPLE 5 The effect of organic solvent additions was evaluated; acidic bromine concentrates were prepared having the compositions set forth in Table 6. Measurements were made of Br 2 partial pressure and other parameters. These are also set forth in Table 6. The compositions of this table are effective for precious metal recovery and industrial water treatment. Table 6 Organic Solvent Acetic Propionic Acid Acid Wt.% H 2 0 (from 48% HBr) 33.8 19.3 19.3 Wt.% 48% HBr 65.0 37.0 37.0 Wt.% Organic Solvent 28.0 28.0 Wt.% Br 2 (experimental) 36.5 36.8 36.6 pH <0 <0 <0 Br 2 Partial Pressure 39.0 20.0 17.0 (mm Hg at 20°C) Density (g/mL) 1.87 1.64 1.60 Crystallization Temp (°C) -45 <-50 -42 EXAMPLE 6 A solution was prepared by dissolving sodium bromide (27.7 grams) in water (29.3 grams). A sodium perbromide solution was prepared by adding liquid bromine in an amount (43.0 grams) sufficient to saturate the bromide ion, i.e., stoichiometrically equivalent to the initial bromide ion content, in the solution. The resulting sodium perbromide component solution contained 43% equivalent molecular bromine. A sodium hydroxide solution was prepared containing 16.7% by weight sodium hydroxide. Liquid bromine (25.0 grams) was added to this solution (75.0 grams) producing a composition which contained 6.7% by weight bromate ion (7.9% by weight as sodium bromate; 25% by weight equivalent molecular bromine) . A concentrate was prepared by mixing equal parts by weight of the perbromide and bromate component solutions. The concentrate so prepared contained 31.82% by weight sodium perbromide, 2.14% by weight bromine, 14.80% by weight sodium bromide, 3.94% by weight sodium bromate and 47.30% by weight water. It had an equivalent molecular bromine concentration of 34% by weight. The bromine concentrations of both the precursor 5 concentrate and the sodium perbromide component solution were confirmed by adding to the respective solutions an excess of potassium iodide and then titrating the iodine released with sodium thiosulfate using starch as an indicator. Titration of the total equivalent molecular bromine content of the 10 concentrate was effected by the addition of a strong mineral acid to convert the bromate content to Br 2 . The concentrate was also titrated without addition of acid in order to determine the actual bromine concentration in terms of molecular bromine and perbromide ion. This titration showed 1521.5% bromine in the concentrate. Using the Isoteniscope method, the total vapor pressure was measured as a function of temperature for liquid Br 2 , the sodium perbromide component solution of this example, and the precursor concentrate of this example. From the data 20 obtained, the corresponding enthalpies of vaporization were calculated. The results of these measurements and calculations are set forth in Table 7. Table 7 Vapor Pressure Data Va or Pressure mm H »c Sodium perbromide and sodium bromate component solutions were prepared in the manner described in Example 6. A series of concentrates was prepared using varying proportions of the two component solutions. The composition of the concentrates obtained are set forth in Table 8. * not computed EXAMPLE 8 In order to compare the vapor pressure of solutions containing bromate ion prepared according to the invention with previously known aqueous bromine-based solutions, a solution was prepared by a formulation method comparable to Bahl, et al. U.S. Patent No. 4,190,489, and a composition was prepared according to the invention, each containing 34% by weight equivalent bromine. For the Bahl et al. formulation, 26 g KBr was dissolved in 40 g water and then 34 g Br 2 was added to the resulting solution. For the composition prepared according to the invention, 14.26 g NaBr, 45.49 g H 2 0, 6.25 g NaOH and 34 g Br 2 were mixed. Bromate content and vapor pressure were calculated as follows: Titration with Thiosulfate-KI using a weak acid determines actual Br 2 content (Br 2 + Br 3 " ) while titration with Thiosulfate-KI using a strong acid converts bromate to bromine and determines the sum of bromate and bromine concentration. Therefore, the bromate content of the two solutions was determined by Thiosulfate-KI titration first with acetic acid to determine the actual bromine concentration, and then by Thiosulfate-KI titration with H 2 S0 4 to determine the total equivalent molecular bromine (Br 2 + Br 3 " + Br0 3 " ) and subtracting the difference. Solution vapor pressure at 25°C was obtained by using the Isoteniscope method. The results obtained are set forth in Table 9. Table 9 pH, Br 2 Concentration, and Vapor Pressure Measurements: Composition A of the invention * vs. Bahl Formulation ** Parameter A Bahl Formulation pH Wt. % Br 2 (with Acetic acid) Wt . % Br 2 (with H 2 S0 4 ) Wt. % Br 2 (present as Br0 3 " ) Vapor Pressure at 25°C mm-Hg * 14.26 g NaBr, 45.49 g H 2 0, 6.25 g NaoH, 34 g Br 2 . ** 26 g KBr, 40 g H 2 0, 34 g Br 2 . EXAMPLE 9 A solubilizing reagent having the composition of that prepared in accordance with Example 4, composition #31 (using 46% NaBr) (hereinafter the "PGM Reagent") was used to demonstrate the ability of the present composition to solubilize palladium. Samples of a precious metal scrap, comprising a hydrocracking catalyst (estimated 0.5% Pd) were used in the following tests to evaluate the effect of pH, pH adjuster, time, bromide concentration, reagent source, temperature and mixing speed. pH/pH Adjuster The suitability of various acids was studied for adjustment of pH in order to achieve the very low pH (<0) found to be particularly advantageous for palladium recovery. These tests involved the dissolution of 2.5 g catalyst in 5 g PGM Reagent and 100 g H 2 0. The results are set forth in Table 10. The various acids tested were shown to be useful for pH adjustment. Sulfuric acid provided for the greatest palladium recovery, but also digested the largest amount of substrate. Sulfuric acid was chosen as the pH adjuster for subsequent tests. Table 10 Dissolution Time Duplicate tests were conducted to demonstrate the effect of reaction time for recovery of Pd from the catalyst. 2.5 g catalyst was dissolved in a solution containing 5 g PGM Reagent, 10 g cone. H 2 S0 4 and 100 g H 2 0 at 85°C with a shaker bath mixing speed of 280 rpm. The results of these tests are shown in Table 11. A graph with the best fitting curve of the oz/ton Pd in solution vs. time peaks at approximately 10-14 hours. Due to the time limitations of a workday, 10 hours was chosen as the optimum reaction time for further studies. Bromide Concentration The bromide concentration variable was controlled by using 46% NaBr. 2.5 g catalyst was contacted with a solution of 5 g PGM Reagent, 10 g cone. H 2 S0 4 and 100 g H 2 0 for 10 hrs at 85°C with a shaker bath mixing speed of 280 rpm. The results of this set of tests, provided in Table 12, show that NaBr in addition to that provided by the PGM reagent did not improve palladium dissolution. Table 12 A further test was performed to evaluate the dissolution of palladium using bromine only as the reagent. For each of the tests described in Table 13, 2.5 g catalyst was contacted with a solution containing 10 g cone. H 2 S0 4 and lOOg water for 10 hrs at 85°C with a shaker bath mixing speed of 280 rpm. As shown in Table 12, the PGM Reagent performed better than the equivalent amount of bromine in water. Table 13 It has been found that effective leaching of palladium and platinum can be achieved at temperatures in the range of 80-90°C. Tests were conducted to assess leaching effectiveness at lower temperatures in recovery of Pd from spent catalyst. 2.5 g catalyst was contacted with a solution containing 5 g PGM Reagent, 10 g cone. H 2 S0 4 and 100 g H 2 0 for 10 hrs at a shaker bath mixing speed of 280 rpm. The results are given in Table 14. The recovery reported in these tests was not as good as had been demonstrated at 80°C-90°C. Lower temperatures helped to preserve the substrate, but lowered the palladium recovered in solution. For the recovery of Pd from this scrap, 85°C was chosen as the optimum temperature. Table 14 Mixing Speed The effect on dissolution of the the mixing speed of the shaker bath was studied. In earlier tests mixing was carried out at the highest mixing speed (280 rpm) that would allow the reaction flasks to remain securely positioned. In these tests, at lower speeds, 2.5 g catalyst was contacted with a solution containing 5 g PGM Reagent, 10 g cone. H 2 S0 4 and 100 g H 2 0 for 10 hrs at 85°C. As shown in Table 15, the 100 rpm setting was surprisingly better for palladium dissolution than the 200 rpm setting. Also, the 100 rpm mixing speed performed just as well, if not better, than the speed (280) of the other tests. Three confirmatory tests, using the 100 rpm setting, were performed. The palladium in solution ranged from 104 to 116 oz/ton, averaging 109.9 oz/ton. The tailings of all three confirmatory tests plus the original, duplicate tests of the 100 rpm setting were placed in aqua regia refluxes. An average of 9.46 oz/ton Pd remained in the five residues. From these results, a mass balance showed that the average percent of palladium solubilized by the PGM Reagent was 92.11%. EXAMPLE 10 _ A refractory concentrate containing platinum, palladium, rhodium and gold was used (after roasting overnight at 800°C) in this example to evaluate the efficacy of the — inventive compositions for solubilizing gold, platinum, and palladium. The analysis of this concentrate by Hazen Research Laboratories was 50.6 oz/ton Pd, 15.6 oz/ton Pt, 0.83 oz/ton Au, and 0.44 oz/ton Rh. Due to the high sulfur content, roasting of the concentrate was deemed necessary, and several tests were performed on the calcine concentrate. The variables studied included PGM Reagent concentration, reaction time, preleaching, pH adjuster, method of agitation, and acid concentration. PGM Reagent Concentration Three concentrations of PGM Reagent were tested. 10 g of calcine concentrate was dissolved in a solution containing varying amounts of PGM Reagent, 10 g cone. H 2 S0 4 5 and 100 g H 2 0 for 16 hrs at 85°C and at a mixing speed of 200 rpm. The results are shown in Table 16. Based on these tests, 5 g or 5% PGM Reagent was selected as the optimum concentration for the remaining tests. Rh was not detectable by ICP analysis throughout all tests. 10 Table 16 2.5g PGM Reagent pH <0 ORP (mV) 897 15 Pd ox/ton soln. 24.6 Pt oz/ton soln. 6.71 Au oz/ton soln. * Reaction Time 10 g calcine was dissolved in a solution containing 20 10 g cone. H 2 S0 4 , 5 g PGM Reagent and 100 g H 2 0 at 85°C and at a mixing speed of 200 rpm. The results shown in Table 17 indicate a palladium peak at six hours, but also a platinum peak at sixteen hours (or overnight). Both of these reaction times were used interchangeably in subsequent testing. 25 Table 17 1 hr 2 hrs 4 hrs 6 hrs 8 hrs 16 hrs 24 hrs pH <0 ORP (mV) 910 Pd oz/t 17.4 30 Pt oz/t 6.44 Au oz/t * Preleaching Because a high concentration of base metals was thought to be inhibiting platinum and palladium dissolution, the effect of acid preleaching to remove these metals, followed by bromine leaching, was studied. The two preleaches compared were a 20% H 2 S0 4 preleach to a 10% H 2 S0 4 /24% HBr preleach. Each was followed by a 5% PGM Reagent bromine leach. 10 g ore was preleached in 20 g cone. H 2 S0 4 and 80 g H 2 0 for 3 hrs at room temperature. 10 g ore was also preleached in a solution containing 10 g cone. H 2 S0 4 , 50 g 48% HBr and 50 g H 2 0 for 16 hrs at 85°C. After preleaching, each sample was leached in a solution containing 5 g PGM Reagent, 10 g cone. H 2 S0 4 and 100 g H 2 0 at 85°C and a shaker bath mixing speed of 200rpm. As shown in Table 18, the 20% sulfuric acid preleach helped palladium dissolution, but not platinum. The bromine leach following the HBr/H 2 S0 4 preleach improved the platinum dissolution only slightly. T - aCLbl-ll- e— 18O H SS0O, pre Br 2 leach HBr/H,S0 1 pre Br, leach pH <0 <0 <0 <0 ORP (mV) N.A. 874 N.A. 989 Pd oz/ton N.D. 31.3 37.9 N.D. Pt oz/ton N.D. 6.40 4.78 1.36 Au oz/ton N.D. * * * pH Adjuster It was known from prior work that very low pH (<0) was preferred for dissolution of Pt and Pd. The effect of different acids for pH adjustment in the dissolution of this concentrate was studied. 10 g ore was slurried in a solution containing 5 g PGM Reagent and 100 g H 2 0 for 16 hrs at 85°C and a shaker bath mixing speed of 200 rpm. As shown in Table 19, although the HBr and HCl leaches produced a higher concentration of palladium in solution, the H 2 S0 4 leach produced a higher concentration of platinum in solution. A stir plate and heating mantle apparatus was compared to the shaker bath method for agitating ore slurries. The H 2 S0 4 concentration variable was tested simultaneously. 20 g ore was slurried in a solution containing 10 g PGM Reagent and 100 g H 2 0 at 85°C for 6 hrs using stir bars. The results of these tests are presented in Table 20. Fire assay results were obtained and metallurgical balances calculated for the following three tests. The conditions were: LEACH-A: 10 g ore; 10 g cone. H 2 S0 4 ; 5 g PGM Reagent; 90 g H 2 0; 85°C (shaker bath); and 16 hours. LEACH-B: 20 g ore; 40 g cone. H 2 S0 4 ; 10 g PGM Reagent; 150 g H 2 0; 85°C (stir plate); and 16 hours. LEACH-C: Same as B, except time was only 6 hours. The results are presented in Table 21. Pd Solubilized Pt Solubilized Au Solubilized Following the above tests, it was determined that roasting at 750°C may have left some of the Pd and Pt in sulfide form, meaning the roasting was incomplete. Therefore, new samples of the Pd/Pt ore were roasted at 900°C and 1000°C. Weight losses were detected of 8.7% and 9.4%, respectively. Duplicate tests were performed on both the 900°C and 1000°C roasted samples. 10 g calcine was dissolved in a solution containing 20 g cone. H 2 S0 4 , 5 g PGM Reagent and 90 g H 2 0 at 85°C for 6 hours using stir plate mixing. The-results, set forth in Table 22, are averages of the duplicate tests. An increased roasting temperatures helped to increase the Pd dissolution slightly, although the Pt and Au were compromised. Further tests were performed on these samples to optimize the PGM Reagent and bromide concentrations. Lowering the PGM Reagent and compensating the bromide loss with HBr gave very poor results. Pd Solubilized Pt Solubilized Au Solubilized EXAMPLE 11 As for the PGM Reagent used in the preceding Examples, the various other compositions of the present invention provide high levels of molecular bromine for dissolution of platinum and palladium. Repetition of the foregoing Examples 9 and 10 using each of the compositions of Examples 1-7 provides suitable platinum and palladium recoveries. For certain of these processes, the initial PGM reagent includes water, at least about 25% by weight bromine, between about 4% and about 30% by weight hydrobromic acid, and between about 4% and about 15% by weight of lithium bromide, sodium bromide, potassium bromide or calcium bromide, a molar excess of bromide ion over bromine of at least about 30%, and a pH of not greater than about 1.0. This reagent is diluted with water to prepare the leaching solution, which is thereafter contacted with the Pt/Pd source. For others of these processes, the initial PGM reagent includes a precursor composition initially having a pH of between about 6.5 and about 7.5 and comprising bromide ion, perbromide ion, molecular bromine, at least about 2% by weight bromate ion, and an alkali metal or alkaline earth metal ion, the precursor composition having an equivalent molecular bromine content of between about 10% and about 40% by weight and the ratio of the molar concentration of bromate ion to the sum of the molar concentrations of molecular bromine and perbromide ion being between about 0.05 and about 0.8. The precursor composition is acidified, producing a leaching solution having a pH of between about 0 and about 6 and containing between about 0.01% and about 20% by weight equivalent molecular bromine, between about 0.005% and about 20% by weight bromide ion, and between about 0.005% and about 30% by weight total halide ion, which leaching solution is then contacted with the PGM source. EXAMPLE 12 Referring to the Figures 7 and 8, there are shown Eh/pH diagrams for representative platinum group metals in the systems H 2 0-10 "4 M Pd-O.lMBr " (Fig. 7) and H 2 0-10 "4 M Pt-O.IM Br " (Fig. 8). These diagrams are based on thermodynamic data for these metals in Br-H 2 0 at 25°C. The diagrams show the regions of soluble and/or solid bromide complexes formed with platinum and palladium as a function of concentration of bromide and metal ion, applied potential, and pH. EXAMPLE 13 A simulated barren solution was prepared having a composition typical of that which would be obtained after recovery of gold by ion exchange from a pregnant leach solution produced by bromine leaching. To this end, sodium bromide and 48% hydrobromic acid were mixed with water to produce a solution containing 5% by weight bromide ion and having a pH of 3. In a series of runs this solution was circulated at a flow rate of 125 L/sec. between a 300 gal. pilot scale reservoir for the solution and a Chloropac cell operated at a constant amperage of 100A. At this amperage, the Chloropac cell is rated to produce 1/2 lb. Cl 2 per hour. Velocity through the annular portion of the Chloropac cell between the electrodes was about 1.83 m/sec. Measurements were made of current efficiency as a function of the conversion of bromide and the bromine content generated in the solution. The current efficiency decreased with conversion and bromine content, but the cumulative efficiency was still close to 80% at a bromine concentration of 56 mmol dm "3 and a conversion of 11.5%. EXAMPLE 14 Further electrolysis runs were conducted in the manner described in Example 13, except that the simulated barren solution was buffered with 6 mol dm "1 sulfuric acid instead of 48% HBr. The results were essentially identical to those of Example 13. These results indicate that the depletion of Br " from the system has a negligible effect on current efficiency at low conversion. Loss in current efficiency with conversion in this low range can be substantially attributed to reduction of Br 2 to Br " at the cathode. EXAMPLE 15-17 Runs were made according to the general procedure of Example 14 except that the concentration of Br " was varied. In Example 15 the concentration was 4%, in Example 16 it was 3%, and in Example 17 it was 2.5%. To maintain conductivity, the solutions of Examples 16 and 17 further contained sodium sulfate as an auxiliary electrolyte. In Example 16, the Na 2 S0 4 concentration was 0.25 mol dm "3 and in Example 17 it was 0.33 mol dm "3 . In Example 15 the electrolysis was carried out to a conversion of 15.1% and bromine content of about 58 mmol dm "3 . At this point the cumulative current efficiency was about 83-85%. In Example 16 the conversion was 18%, the bromine content about 48 mmol dm "3 , and the cumulative current efficiency about 79%, while in Example 17 the conversion was 12.3%, the bromine content about 24 mmol dm "3 , and the cumulative current efficiency about 84%. EXAMPLE 18 A black sand concentrate (100 g) containing 6 kg/tonne Au was contacted in an agitation bottle with a bromine leaching solution (8.0 g) having a composition typical of a solution that may be prepared from the electrolysis of a sodium bromide solution as described hereinabove. The leaching solution had a pH of about 2 and contained about 0.68% by weight equivalent molecular bromine, about 0.43% by weight bromide ion, and about 0.43% by weight sodium ion. The resultant leaching slurry was agitated in the capped bottle using an overhead mixer at slurry temperature of about 22°C for 24 hours. During leaching the pH and oxidation-reduction potential (ORP) of the slurry were monitored but no adjustment was made while the run was in progress. Measurements indicated that the pH of the slurry was about 1.7 and the oxidation-reduction potential of the system was initially about 900 mV, falling off to about 800 mV. To establish the kinetics of extraction, samples were withdrawn from the leaching bottle at 2, 4, 6, 12, 18, and 24 hours. Fresh water was added to the bottle to compensate for the sampling loss. At the end of the run, the leaching slurry was filtered and the cake was repulped for 10 minutes in a volume of water equal to twice the solids weight. The repulped slurry was then filtered and the cake was washed with a volume of water equal to the solids weight. The gold values in the leaching samples, filtrate, wash, and residue were determined by inductively coupled plasma spectrometry (ICP) and fire assay. The results indicated that 90% of the gold was dissolved during the first two hours, and that dissolution reached a maximum in about 4 hours. To optimize gold recovery, the residue ("tails") was releached twice with fresh leaching solution under conditions comparable to the initial leaching operation. Fresh leaching solution restores the ORP to the 800-900 mV range in which effective removal of gold from the source is realized. To maintain a recovery of 95% of the gold, a total of 14.0 g of leaching solution was consumed, 8.0 g in the initial leach and a total of 6.0 g in the two stage leaching of the residue. D0WEX-21K ion exchange resin was used for recovery of gold from the leaching solution. In the ion exchanger operation, leaching solution (100 mL) containing 300 mg/L Au and having a pH of 2-3 was mixed with particulate ion exchange resin (1.0 g). Loadings of 125-150 kg/tonne were realized after about 4 hours of contact. In certain runs, gold was eluted from the loaded resin using an acetone/HCl solution prepared from three volumes of acetone and one volume of 1M HCl. In other runs, gold was eluted using a thiourea/HCl solution prepared from equal volumes of 1M thiourea and 1M HCl. After each elution, the resin was regenerated by contacting it for two hours with 1M HCl solution. EXAMPLE 19 Electrowinning of gold was carried out in the cathode compartment of a divided electrolytic cell. A simulated pregnant gold bromide solution (146.6 ppm Au) (12 dm 3 ) containing 5% Br " ion and residual Br 2 (not determined) was the catholyte, and a 5% H 2 S0 4 solution served as the anolyte. The streams were recirculated (140 dm 3 hr _1 ) through a plate and frame-type cell equipped with a cation exchange membrane. Nickel foams (30 pores per inch) served as the cathode, and anodized lead shot (Pb0 2 ) was the anode. A cell current of 5A (Cell voltage =4.IV) was imposed for 1.5 hours. This was reduced to 2A for an additional 2.3 hours (Cell voltage =2.9V). On termination, 0.51 ppm Au was dete:r * mined in the catholyte which indicates a 99.7% recovery of the gold which plates on the nickel surface. At the cathode, three electrode reactions take place: At the anode in this example, the counter reac- tion is the oxidation of water to oxygen. However, it should be recognized that anodic oxidation of Br " to Br 2 at, for example, graphite anodes, could also have been the reaction of choice. EXAMPLE 20 Four units of a plate and frame-type cell were used to process a 5% HBr solution. Particulate graphite anodes were separated from Pb cathodes by a cation exchange membrane. A 10% sulfuric acid solution was the catholyte. Flow rates of 300 and 260 dm 3 hr~ 1 were established for the anolyte and catholyte, respectively so that there was no differential fluid pressure across the membrane. A cell voltage of 14.3V was imposed across bipolar electrical connectors to force a cell current of 10A (individual cell voltage = 3.75V). A Faradaic current efficiency of 96.5% was measured at 9.8% Br " conversion. In view of the above, it will be seen that the several objects of the invention are achieved and other advantageous results attained. As various changes could be made in the above products and methods without departing from the scope of the invention, it is intended that all matter contained in the above description shall be interpreted as illustrative and not in a limiting sense.

Claims: WHAT IS CLAIMED IS: 1. A process for producing an aqueous leachate containing platinum, palladium or mixtures thereof from a source thereof comprising contacting said source with an aqueous bromine leaching solution, said leaching solution containing between about 0.01% and about 20% by weight equivalent molecular bromine, between about 0.005% and about 20% by weight bromide ion, and between about 0.005% and about 30% by weight total halide ion, thereby producing said aqueous leachate containing platinum or palladium. 2. A process as set forth in claim 1 wherein said contacting occurs at a pH of less than about 4. 3. A process as set forth in claim 2 wherein said contacting occurs at a pH of less than about 1. 4. A process as set forth in claim 3 wherein said contacting occurs at a pH of less than about 0. 5. A process as set forth in claim 4 wherein said leaching solution contains between about 0.5 and about 5.0 equivalents per liter of acid. 6. A process as set forth in claim 1 wherein said leaching solution contains between about 5% and about 40% by weight H 2 S0 4 . 7. A process as set forth in claim 6 wherein said leaching solution between about 10% and about 20% by weight sulfuric acid. 8. A process as set forth in claim 7 wherein said leaching solution contains between about 15% and about 30% by weight HBr, between about 10% and about 25% by weight total bromide ion and between about 20% and about 40% by weight total halide ion. 9. A process as set forth in claim 2 wherein said leaching solution contains an acid selected from the group consisting of HBr, and HCl. 10. A process as set forth in claim 1 wherein said contacting occurs at a temperature of between about 50°C and about 120°C. 11. A process as set forth in claim 10 wherein said contacting occurs at a temperature of between about 60°C and about 90°C. 12. A process as set forth in claim 11 further comprising the step of recovering platinum or palladium from the leachate. 13. A process as set forth in claim 1 wherein said_ leaching solution contains between about 0.005 and about 10% by weight bromide ion, between about 0.01 and about 1% by weight equivalent molecular bromine, and between about 0.005% and about 15% by weight total halide ion, and has a pH less than about 0. 14. A process as set forth in claim 13 wherein said leaching solution contains between about 0.01 and about 1% by weight bromide ion, between about 0.02 and about 0.5% by weight equivalent molecular bromine, between about 0.01% and about 1.5% by weight total halide ion, and between about 0.5 and about 5.0 equivalents per liter sulfuric acid. 15. A process as set forth in claim 1 wherein said leaching solution contains between about 8 and about 25 gpl equivalent molecular bromine, between about 5 and about 20 gpl bromide ions, and between about 10 and about 40 gpl total halide ions. 16. A process as set forth in claim 1 wherein said aqueous bromine leaching solution is prepared by dilution of a precursor composition initially having a pH of no more than about 8.0 and having an equivalent molecular bromine content of between about 10% and about 40% by weight. 17. A process as set forth in claim 16 wherein said precursor composition has a pH of less than about 4. 18. A process as set forth in claim 17 wherein said leaching solution contains between about 0.5 and about 5.0 equivalents per liter of acid. 19. A process as set forth in claim 18 wherein said leaching solution comprises between about 5% and about 40% by weight H 2 S0 4 . 20. A process as set forth in claim 16 wherein said contacting occurs at a temperature between about 60°C and about 90°C. 21. A process as set forth in claim 16 further comprising the step of recovering platinum or palladium from the leachate. 22. A process as set forth in claim 1 wherein said aqueous leaching solution is prepared by acidification and dilution of a precursor composition initially having a pH of no more than about 8.0 and comprising bromide ion, perbromide ion, molecular bromine, at least about 2% by weight bromate ion, and a metal ion selected from the group consisting of alkali metal and alkaline earth metal, the precursor composition having an equivalent molecular bromine content of between about 10% and about 40% by weight and the ratio of the molar concentration of bromate ion to the sum of the molar concentrations of molecular bromine and perbromide ion in the precursor composition being between about 0.05% and about 0.8, the process further comprising the step of recovering platinum or palladium from the leachate. 23. A process as set forth in claim 22 wherein said contacting occurs at a pH of less than about 4. 24. A process as set forth in claim 23 wherein said leaching solution contains between about 0.5 and about 5.0 equivalents per liter of acid. 25. A process as set forth in claim 24 wherein said leaching solution additionally comprises between about 5% and about 40% by weight H 2 S0 4 . 26. A process as set forth in claim 1 wherein said aqueous leaching solution is prepared by dilution of a composition comprising water, at least about 25% by weight bromine, between about 4% and about 30% by weight hydrobromic acid, and between about 4% and about 15% by weight of a metal bromide selected from the group consisting of lithium bromide, sodium bromide, potassium bromide and calcium bromide, said composition comprising a molar excess of bromide ion over bromine of at least about 30%, said composition having a pH of not greater than about 1. 27. A leaching solution adapted for leaching a metal selected from the group consisting of platinum, palladium or mixtures thereof from a source containing metal, said solution having a pH of less than about 4 and containing between about 0.01% and about 1% by weight equivalent molecular bromine, between about 0.01% and about 1% by weight bromide ion, and between about 0.005% and about 15% by weight total halide ion. 28. A solution as set forth in claim 27 having a pH less than about 0. 29. A solution as set forth in claim 28 wherein said composition contains between about 0.01 and about 1% by weight bromide ion, between about 0.02 and about 0.5% by weight equivalent molecular bromine between about 0.01% and about 1.5% by weight total halide ion, and between about 0.5 and about 5.0 equivalents per liter sulfuric acid. 30. A solution as set forth in claim 27 wherein said composition contains between about 8 and about 25 gpl equivalent molecular bromine. 31. A process for producing an aqueous leachate containing a metal or metals selected from the group consisting of platinum and palladium from a source thereof comprising the steps of: causing an aqueous solution containing bromide ions to flow through an electrogeneration system that comprises paired anode means and cathode means, said system having an inlet and an outlet for the flow of said solution; applying a direct electric potential via said anode means and said cathode means to cause an electric current to pass through said flowing solution in said system and to generate bromine at said anode means by electrolytic oxidation of bromide ions, thereby producing a brominated leaching solution, the relationship between said electric current and the throughput of said flowing solution through said system being such that between about 4% and about 50% of the bromide in said inlet solution is converted to bromine at said anode means; contacting said source with said brominated leaching solution, thereby causing metal or metals contained in said source to react with said leaching solution producing said aqueous leachate containing metal or metals. 32. A process as set forth in claim 31 comprising the additional step of recovering metal or metals from said aqueous leachate. 33. A process as set forth in claim 32 comprising the additional step of recycling a depleted bromide solution to the inlet of said electrogeneration system, said depleted bromide solution being produced by said recovering step. 34. A process as set forth in claim 341 wherein said ' aqueous solution has a bromide ion concentration of between about 0.05 and about 8.8 moles per liter at the inlet of said system, said brominated leaching solution contains at least about 8 grams per liter equivalent molecular bromine, and said contacting occurs at a temperature between about 50°C and about 120°C and at a pH of less than about 4. 35. A process as set forth in claim 34 comprising the additional step of recovering platinum or palladium from said aqueous leachate. 36. A process as set forth in claim 35 comprising the additional step of recycling a depleted bromide solution to the inlet of said electrogeneration system, said depleted bromide solution being produced by said recovering step. 37. A process as set forth in claim 36 comprising the additional step of introducing a source of bromide ion into said depleted bromide solution. 38. The process of claim 36 comprising the additional step of adjusting the pH of said aqueous solution by adding an acid selected from the group consisting of H 2 S0 4 , HCl and HBr in the preparation of said aqueous solution. 39. A process as set forth in claim 38 wherein said acid is H 2 S0 4 . 40. A process as set forth in claim 34 wherein said contacting occurs at a temperature between about 60°C and about 90°C. 41. A process as set forth in claim 34 wherein said contacting occurs at a pH of less than about 1. 42. A process as set forth in claim 41 wherein said contacting occurs at a pH of less than about 0. 43. A process as set forth in claim 34 wherein said leaching solution contains between about 5% and about 40% by weight H 2 S0 4 . 44. A process as set forth in claim 34 wherein said electrogeneration system comprises one or more undivided cells each having an annular path for flow of said aqueous solution between substantially concentric electrodes. 45. A process as set forth in claim 44 wherein said electrogeneration system comprises one or more bipolar dual cell assemblies, said assembly comprising an outer electrode subassembly comprising two substantially axially aligned outer cylindrical electrodes mechanically attached to each other through an electrically insulating attachment means, said assembly further comprising an inner cylindrical electrode of smaller diameter than said outer electrodes, said inner electrode being substantially concentric with said outer electrodes, whereby one of said outer electrodes may serve as an anode when the other serves as a cathode, the portion of said inner electrode facing said the outer electrode serving as an anode thus functioning as a cathode and the portion of said inner electrode facing said outer electrode serving as a cathode thus functioning as an anode, all of said electrodes being constructed of titanium, said anodic outer electrode and said anodic portion of said inner electrode being coated with platinum. 46. The process of claim 34 wherein said source comprises platinum and palladium oxides. 47. A process as set forth in claim 34 wherein the relationship between said electric current and the throughput of said flowing solution through said system being such that the solution discharged from the outlet of said system contains between about 0.01 and about 3.66 moles per liter equivalent bromine and between about 0.1 and about 4.0 moles per liter unreacted bromide ion, said contacting occurs at a temperature between about 60°C and about 90°C and at a pH of less than about 0, said process comprising the additional step of recovering said platinum or palladium from said aqueous leachate. 48. A process for producing an aqueous leachate containing gold, silver, platinum, palladium or mixtures thereof from a source thereof comprising the steps of: causing an aqueous solution containing between about 0.065 and about 0.25 moles per liter bromide ions and at least about 0.56 moles per liter chloride ions to flow through an electrogeneration system that comprises paired anode means and cathode means, said system having an inlet and an outlet for the flow of said solution; applying a direct electric potential via said anode means and said cathode means to cause an electric current to pass through said flowing solution in said system and to generate bromine at said anode means by electrolytic oxidation of bromide ions, thereby producing a brominated leaching solution, the relationship between said electric current and the throughput of said flowing solution through said system being such that between about 20% and about 50% of the bromide in said inlet solution is converted to bromine at said anode me contacting said source with said brominated leaching solution, thereby causing gold, silver, platinum, palladium or mixtures thereof contained in said source to react with said leaching solution producing said aqueous leachate. 49. A process as set forth in claim 48 wherein said aqueous solution contains between about 1.25 and about 2.25 moles per liter chloride ions. 50. A process as set forth in claim 48 wherein the molar ratio of chloride ions to bromide ions in said aqueous solution is at least about 10. 51. A process as set forth in claim 50 wherein the molar ratio of chloride ions to bromide ions in said aqueous solution is at least about 25.

Inventors: BORDEN DENNIS W, DADGAR AHMAD, FAVSTRITSKY NICOLAI A, HOWARTH JONATHAN N, LIKENS L JANE, MCKEOWN JULIE A, SANDERS BRENT M, SERGENT RODNEY H, BORDEN, DENNIS, W., DADGAR, AHMAD, FAVSTRITSKY, NICOLAI, A., HOWARTH, JONATHAN, N., LIKENS, L., JANE, MCKEOWN, JULIE, A., SANDERS, BRENT, M., SERGENT, RODNEY, H.
Applicants: GREAT LAKES CHEMICAL CORP, GREAT LAKES CHEMICAL CORPORATION
Application year: 1993
Main classification: C22B11
IPC codes: C22B3, C22B11