Copper(II) interaction with carbonate species based on malachite solubility in perchlorate medium at the ionic strength of seawater

Equilibrium constants for copper(II)-carbonate and -bicarbonate species have been determined at 25°C from consideration of malachite, Cu₂(OH)₂CO_3(s), solubility in UV-photo-oxidized perchlorate solutions of 0.72 m ionic strength. The ratios of total dissolved copper, T(Cu), to free copper(II) ion, [Cu ²⁺], in 30 malachite saturated experimental solutions of 1–10 × 10^?3eq kg^?1 H₂O initial total alkalinity (TA_i in the pH range 5.0–9.3 were fitted to a copper(II)-ion speciation model. The experimental data indicate the existence of CuCO₃⁺, CuHCO₃⁺ and Cu(OH)CO₃^? in addition to the hydrolys and Cu(OH)CO₃^? in addition to the hydrolysis products in the range of conditions defined by this study. The stoichiometric equilibrium constants, applicable to seawater at 0.72 m ionic strength, 25°C and 1 atm are

A speciation model employing the equilibrium constants determined in this study and copper(II) hydrolysis constants from previous work suggests that the inorganic speciation in seawater (pH = 8.2, TA = 2.3 meq kg ^?1, 25°C) is dominated by the CuCO₃⁰ complex (82%) and that only 2.9% of the total inorganic copper exists as the free copper(II) ion. Hydrolysis products, CuOH⁺ and Cu(OH)₂⁰, account for 6.5% while CuHCO₃⁺ and Cu(OH)CO₃^? species comprise 1.0 and 6.3% of the total inorganic copper, respectively.     

Thermodynamics of the system H2ONaClMgCl2Na2SO4MgSO4 at 25°C

Osmotic coefficients and Gibbs energies of mixing for the system H₂ONaClMgCl₂MgSO₄ have been calculated from isopiestic vapor pressure measurements. These results have been combined with earlier results from the system H₂ONaClNa₂SO₄MgSO₄ to construct Jänecke diagrams giving osmotic coefficients at constant ionic strength. Osmotic coefficients calculated from the theory of Reilly and Wood are in good agreement with measured values for the four-salt system, for compositions and ionic strengths comparable to those of natural brines.     

Effects of alkaline aluminate waste dumping on seawater chemistry

The alkaline aluminate waste, of which 1000–2000 tonnes are dumped a few times a year off the Belgian coast in the Southern Bight of the North Sea, contains 5·4% NaCl, 1·8% dissolved Al and 7·4% NaOH, in addition to traces of heavy metals and some aniline- and phenol-derivatives. The pH rises locally to 8-5 and the total Al-concentration reaches 120niglitre⁻¹(corresponding to an initial waste dilution factor of only 150) in the 10-m wide track just beyond the discharging barge, but these decay quickly to pH 8·1 and 1 mg litre^-1 in the 30-m wide track, 500m behind the barge. The relation between the waste concentration and seawater pH was studied. The white precipitate that forms immediately in the sea was identified as Mg₆---Al₂---CO₃---(OH)₁₆---4H₂0 (hydrotalcite-manasseite like). No trace of it was found in the local sediments.     

Peculiarities of the disturbance in the mesosphere composition and optical emissions caused by high-altitude discharges

The suggested equation system, including 267 chemical reactions and corresponding parametrizations of disturbances of the electric field and electron temperature, describes the dynamics of the mesosphere composition under the influence of high-altitude discharges (sprites and halos). Based on this system, the ionic disturbance, neutral components, and optical emissions of the night mesosphere caused by the sprites were modeled for a height of 77–85 km. Most attention was paid to the dynamics of disturbances of concentrations of electrons and O ₂ ⁺ , NO⁺, H₃O⁺, H₅O ₂ ⁺ , and N ₂ ⁺ typical of the studied heights. The major chemical reactions leading to the disturbance of ionic contents are determined and the relaxation dynamics of the chemical components is reviewed. The account of the excited atoms and molecules of nitrogen and oxygen allowed us to model the radiation of the sprite flash, calculate the volumetric velocity of the photon emission, and study the influence of the sprite on the neutral components of the mesosphere.     

The speciation of Fe(II) and Fe(III) in natural waters

The interactions of Fe(II) and Fe(III) with the inorganic anions of natural waters have been examined using the specific interaction and ion pairing models. The specific interaction model as formulated by Pitzer is used to examine the interactions of the major components (Na⁺, Mg²⁺, Ca²⁺, K⁺, Sr²⁺, Cl⁻, SO₄⁻, HCO₃⁻, Br⁻, CO₃²⁻, B(OH)₄⁻, B(OH)₃ and CO₂) of seawater and the ion pairing model is used to account for the strong interaction of Fe(II) and Fe(III) with major and minor ligands (Cl⁻, SO₄²⁻, OH⁻, HCO₃⁻, CO₃²⁻ and HS⁻) in the waters. The model can be used to estimate the activity and speciation of iron in natural waters as a function of composition (major sea salts) and ionic strength (0 to 3 M). The measured stability constants (K_FeX^*) of Fe(II) and Fe(III) have been used to estimate the thermodynamic constants (K_FeX) and the activity coefficient of iron complexes (γ_FeX) with a number of inorganic ligands in NaClO₄ medium at various ionic strengths: In(K_FeX/γ_Feγ_X) = InK_FeX − In(γ_FeX) The activity coefficients for free ions (γ_Fe, γ_x) needed for this extrapolation have been estimated from the Pitzer equations. The activity coefficients of the ion pairs have been used to determine Pitzer parameters (B_FeX, B_FeX⁰, C_FeX^φ) for the iron complexes. These results make it possible to estimate the stability constants for the formation of Fe(II) and Fe(III) complexes over a wide range of ionic strengths and in different media. The model has been used to determine the solubility of Fe(III) in seawater as a function of pH. The results are in good agreement with the measurements of Byrne and Kester and Kuma et al. When the formation of Fe organic complexes is considered, the solubility of Fe(III) in seawater is increased by about 25%.     

Distribution of oxygen-containing functional groups and elements in humic acids from marine sediments

The elemental composition and oxygen-containing functional groups contents in the marine humic acids from the five sediment samples from Sagami Bay and Suruga Bay were determined. Kumada's method of classification of soil humic acids was applied to the marine humic acids. The carbon, nitrogen, hydrogen, oxygen and sulfur contents of the marine humic acids were, on average, 52.96, 5.12, 5.79, 34.99 and 1.13%, respectively, without wide variation. In comparison with terrestrial humic acids, the marine ones had relatively lower carbon content and higher hydrogen and nitrogen contents. It is suggested that the marine humic acids have more aliphatic and less aromatic character, as expected from their possible origins, e.g., phytoplankton. The total acidity, carboxyl, phenolic and alcoholic hydroxyl, carbonyl and methoxyl group contents in the marine humic acids were, on average, 5.80, 3.27, 2.53, 2.53, 3.09 and 0.41 milliequivalents per gram of dry ash-free humic acid (me g^–1), respectively. From quantitative data on the elemental composition and functional groups of the average marine humic acid, its empirical formula was calculated to be C₁₀₇H₁₃₈O₂₀(COOH)₉(OH)₇ ^phenolic (OH)₇ ^alcoholic (CO)₉(OCH)₃N₁₀S. The marine humic acids were similar to the so-called B type of soil humic acids with regard to the distribution of functional groups and spectroscopic properties.     

Benzo[a]pyrene-dione-stimulated oxyradical production by microsomes of digestive gland of the common mussel, Mytilus edulis L

The potential of benzo[ a]pyrene (BaP) quinones (diones) to stimulate NAD(P)H-dependent hydroxyl radical (·OH) production (2-keto-4-methiolbutyric acid (KMBA) oxidation) by digestive gland microsomes of M. edulis was studied using iron/EDTA as a promotor of the Haber-Weiss reaction (O₂⁻ + H₂O₂ = ·OH + OH⁻ + O₂). Stimulation of basal rates of KMBA oxidation was observed for all three diones. Stimulation was similar for the 1,6- and 3,6-diones, but much less for the 6,12-dione, and greater for the NADH than the NADPH-dependent reaction, viz. % increases of 78 to 333 (NADH) compared to 0 to 78 (NADPH). Maximal KMBA oxidation was obtained at dione concentrations of 12.5 to 50 μm. Inhibition of KMBA oxidation by Superoxide dismutase and catalase indicated the involvement of respectively Superoxide anion radical (O₂⁻) and hydrogen peroxide (H₂O₂) in 1,6-dione stimulated NADPH-dependent · OH formation. The apparent K_m values of xenobiotic-stimulated KMBA oxidation were lower for BaP-diones than for the model redox cycling quinone menadione (2-methyl-1,4-naphthoquinone), viz. in μm, 0.6 to 14.6 (NADH) and 4.4 to 28.5 (NADPH) compared to 315 to 457 (NADH) and 72 to 103 (NADPH). The results are consistent with metabolism of BaP to diones and resultant enhanced generation of oxyradicals being a potential mechanism of pollutant-mediated toxicity in molluscs.     

Actinide speciation in aquatic systems

Nuclear test explosions and reactor wastes have deposited an estimated 16 × 10¹⁵ Bq of plutonium into the world's aquatic systems. However, plutonium concentration in open ocean waters is on the order 10^− 5 Bq/kg, indicating that most of the plutonium is quite insoluble in marine waters and has been incorporated into sediments. Actinide ions often are not in a state of thermodynamic equilibrium and their solubility and migration behavior is related to the form in which the nuclides were introduced into the aquatic system.Actinide solubility depends on such factors as the pH (hydrolysis), Eh (oxidation state), reaction with complexants (e.g., carbonate, phosphate, humic acid, etc.), sorption to surfaces of minerals and/or colloids etc., in the water. The most significant of these variables is the oxidation state of the metal ion. The simultaneous presence of more than one oxidation state for some actinides (e.g., plutonium) in a solution complicates actinide environmental behavior. Both Np(V)O₂⁺ and Pu(V)O₂⁺, the most significant states in natural, oxic waters are relatively noncomplexing and resistant to hydrolysis and subsequent precipitation. The solubility of NpO₂⁺ can be as high as 10^− 4 M while that of PuO₂⁺ is limited by reduction to the insoluble tetravalent species, Pu(OH₄), (pK_sp = 56). The net solubility of hexavalent UO₂²⁺ in sea water is also limited by hydrolysis; however, it has a relatively high concentration due to formation carbonate complexes. The insoluble trivalent americium hydroxocarbonate, Am(CO)₃(OH), is limiting species for the solubility of Am(III) in sea water. Thorium is found exclusively as the tetravalent species and its solubility is limited by the formation of quite insoluble Th(OH)₄.The chemistry of actinide ions in the environment is reviewed to show the spectrum of reactions that can occur in natural waters which must be considered in assessing the environmental behavior of actinides. While much is understood about sorption of actinides on surfaces, the mode of migration of actinides in such waters and the potential effects of these radioactive species on marine bioto, much more is needed for a satisfactory understanding of the behavior of the actinides in the environment.     

Equilibrium and structural studies of silicon(IV) and aluminium(III) in aqueous solution. II. Formation constants for the monosilicate ions SiO(OH)3 and SiO2(OH)2. A precision study at 25°C in a simplified seawater medium

The hydrolysis of silicic acid, Si(OH)₄, was studied in a simplified seawater medium (0.6 M Na(Cl)) at 25°C. The measurements were performed as potentiometric titrations (hydrogen electrode) in which OH⁻ was generated coulometrically. The total concentration of Si(OH)₄, B, and log[H⁺] were varied within the limits 0.00075 B 0.008 M and 2.5 -log[H⁺] 11.7, respectively. Within these ranges the formation of SiO(OH)₃⁻ and SiO₂(OH)₂²⁻ with formation constants log β₋₁₁(Si(OH)₄ SiO(OH)₃⁻ + H⁺) = −9.472 ±0.002 and log β₋₂₁(Si(OH)₄ SiO₂(OH)₂²⁻ + 2H⁺) = −22.07 ± 0.01 was established. With B > 0.003 M polysilicate complexes are formed, however, with -log[H⁺] 10.7 their formation does not significantly affect the evaluated formation constants. Data were analyzed with the least squares computer program LETAGROPVRID.     

Equilibrium and structural studies of silicon(IV) and aluminium(III) in aqueous solution. II. Formation constants for the monosilicate ions SiO(OH)3− and SiO2(OH)22−. A precision study at 25°C in a simplified seawater medium

The hydrolysis of silicic acid, Si(OH)₄, was studied in a simplified seawater medium (0.6 M Na(Cl)) at 25°C. The measurements were performed as potentiometric titrations (hydrogen electrode) in which OH^? was generated coulometrically. The total concentration of Si(OH)₄, B, and log[H⁺] were varied within the limits 0.00075 ? B ? 0.008 M and 2.5 ? -log[H⁺] ? 11.7, respectively. Within these ranges the formation of SiO(OH)₃^? and SiO₂(OH)₂^2? with formation constants log β_?11(Si(OH)₄ ? SiO(OH)₃^? + H⁺) = ?9.472 ±0.002 and log β_?21(Si(OH)₄ ? SiO₂(OH)₂^2? + 2H⁺) = ?22.07 ± 0.01 was established. With B > 0.003 M polysilicate complexes are formed, however, with $\text{-}\text{log[H}{}^{\mathrm{+}}\text{] ? 10.7}$ their formation does not significantly affect the evaluated formation constants. Data were analyzed with the least squares computer program LETAGROPVRID.     

Solubility of hydrous ferric oxide and iron speciation in seawater

Iron solubility equilibria were investigated in seawater at 36.22‰ salinity and 25°C using several filtration and dialysis techniques. In simple filtration experiments with 0.05 μm filters and Millipore ultra-filters, ferric chlorides fluorides, sulfates, and FeOH²⁺ species were found to be insignificant relative to Fe(OH)₂⁺ at p[H⁺] = ?log [H⁺] greater than 6.0. Hydrous ferric oxide freshly precipitated from seawater yielded a solubility product of ${}^1\text{K}{}_{\mathrm{<mtext>so</mtext>}}\text{=}\text{[Fe}{}^{\mathrm{3+}}\text{][H}{}^{\mathrm{+}}\text{]}{}^{\mathrm{?3}}\text{= 4.7 · 10}{}^5$. Solubility studies based on the rates of dialysis of various seawater solutions and on the filtration of acidified seawater solutions indicated the existence of the Fe(OH)₃⁰ species. The formation constant for this species can be calculated as ${}^1\text{β}{}_3\text{=}\text{[Fe(OH)}{}_3{}^0\text{] [H}{}^{\mathrm{+}}\text{]}{}^3\text{/[Fe}{}^{\mathrm{3+}}\text{] = 2.4 · 10}{}^{\mathrm{?14}}$. The Fe(OH)₄^? species is present at concentrations which are negligible compared to Fe(OH)₂⁺ and Fe(OH)₃⁰ in the normal pH range of seawater. However, there is at least one other significant ferric complex in seawater above p[H⁺] = 8.0 (possibly with bicarbonate, carbonate, or borate ions) in addition to the Fe(OH)₂⁺ and Fe(OH)₃⁰ species.     

Interconversion of iron(III) hydroxy complexes in seawater

Interconversion rates of the mononuclear ferric iron species Fe(OH)₃⁰ and Fe(OH)₂⁺ are derived and their implications for the behavior of these species in seawater are examined. The previously reported formation constant for Fe(OH)₃⁰ and its claimed extreme adsorptive reactivity in seawater are shown to be mutually inconsistent. Although Fe(OH)₃⁰ is probably a stoichiometrically minor dissolved iron species, its rapid formation from Fe(OH)₂⁺ could substantially enhance the rates of heterogeneous reaction rates of the [Fe(OH)₂⁺ + Fe(OH)₃⁰] pool if the latter species is very reactive.     

Aluminum hydroxide’s solubility and the forms of dissolved aluminum’s occurrence in seawater

The solubility of aluminum hydroxide in seawater of 35‰ salinity at pH = 7.4−8.2 and 25°C was determined experimentally for three samples synthesized in different ways. The solubilities of two phases subjected to ageing and precipitated (a) from a boiling solution of aluminum sulfate and (b) immediately from seawater at room temperature were a little different and showed the minimum within pH = 8.05−8.10. The solubility of aluminum hydroxide precipitated from a solution of sulfate aluminum at room temperature and not subjected to ageing was about twofold at pH∼7.9. The analysis of the pH dependence of the concentration of dissolved aluminum allows one to suppose that an Al(OH)₂⁺ hydroxo complex is the primary form of the aluminum occurrence in seawater at pH < 8.05, whereas the Al(OH)₄⁻ anion is prevailing at pH > 8.10. Electrically neutral Al(OH)₃⁰ hydroxocomplexes may be prevailing within the narrow range of pH = 8.05−8.10 and, in general, are of secondary importance.     

Experimental evaluation of the isotopic exchange equilibrium 10B(OH)3+11B(OH)4−=11B(OH)3+10B(OH)4− in aqueous solution

The precision of spectrophotometric measurements of indicator absorbance ratios is sufficient to allow evaluation of small isotopically induced differences in the dissociation constant of boric acid (K_B). The quotient of ¹¹K_B and ¹⁰K_B, obtained using isotopically ⩾99% pure borate/boric acid buffers, provides an equilibrium constant for the reaction ¹⁰B(OH)₃+¹¹B(OH)₄⁻⇔¹¹B(OH)₃+¹⁰B(OH)₄⁻ which heretofore had not been experimentally determined. Previous theoretical and semi-empirical evaluations of this equilibrium, which is important for assessments of the paleo-pH of seawater and the paleo-pCO₂ of the atmosphere, have yielded constants, ^11–10K_B=¹⁰K_B/¹¹K_B, that have ranged between 1.0194 and approximately 1.033. The experimentally determined value ^11–10K_B=1.028₅±0.001₆ (mean±95% confidence interval) obtained at 25 °C and 0.63 molal (mol kg⁻¹ H₂O) ionic strength is in much better agreement with recent theoretical assessments of ^11–10K_B that have ranged between 1.026 and 1.033, than the much-cited original estimate (1.0194) of Kakihana et al. (1977) [Fundamental studies on the ion-exchange separation of boron isotopes. Bulletin of Chemical Society of Japan 50, 158–163]. Since the activity quotient for the fractionation reaction is almost equal to unity, it is expected that the ^11–10K_B value obtained in this study will be applicable over a wide range of solution compositions and ionic strengths.     

Ionic medium effects in sea water — A comparison of acidity constants of carbonic acid and boric acid in sodium chloride and synthetic sea water

It is shown that the values of pK_1C and pK_2C for carbonic acid, pK_B for boric acid and the ionic product of water, pK_w, in sea water may be explained on the basis of their determination in 0.7 M_w sodium chloride and the formation of the following ion-pairs: NaSO₄^?, MgSO₄, CaSO₄, MgCO₃, CaCO₃, MgHCO₃⁺, CaHCO₃⁺, MgOH⁺, HSO₄^?, MgB(OH)₄⁺ and CaB(OH)₄⁺. On the whole the calculated stability constants are lower than those given by Garrels and Thompson (1962).     

预处理方法对海洋微藻Isochrysis zhanjiangenisis脂肪酸组成及稳定碳同位素的影响

This study aims to quantify the effects of different pretreatment methods on the stable carbon isotope values of fatty acids in marine microalgae(Isochrysis zhanjiangenisis).To identify the effects of sample preparation on theδ~(13)C value and the fatty acid composition,we examined eight types of pretreatment methods including:(a) drying the sample followed by direct methyl esterification using HCl-CH_3OH;(b) drying the sample followed by direct methyl esterification using H_2SO_4-CH_3OH;(c) drying the sample by ultrasonic extraction and methylesterification using HCl-CH_3OH;(d) drying the sample by ultrasonic extraction and methyl-esterification using H_2SO_4-CH_3OH;(e) fresh sample followed by direct methyl-esterification using HCl-CH_3OH;(f) fresh sample followed by direct methyl-esterification using H_2SO_4-CH_3OH;(g) fresh sample with ultrasonic extraction followed by methyl-esterification using HCl-CH_3OH,and(h) fresh sample with ultrasonic extraction followed by methylesterification using H_2SO_4-CH_3 OH.The results show that the δ~(13)C values from Groups a–e,g and h fluctuated within 0.3‰,and the δ~(13)C values of Group f were approximately 0.7‰ lower than the other seven groups.Therefore,the different sample pretreatment methods used towards the extraction of fatty acids from marine microalgae may result in different results regarding the stable carbon isotope ratios,and if necessary a correction should be applied.     

A theoretical study of the kinetics of the boric acid–borate equilibrium in seawater

Dissolved boron in seawater occurs mainly in the form of boric acid (B(OH)₃) and borate (B(OH)₄⁻). While the equilibrium properties of the dissociation of boric acid have been studied in detail, very little work has focused on the kinetics of the boric acid–borate equilibrium in seawater. Here, we present a theoretical study of the relaxation of the seawater borate–carbonate system towards equilibrium using the experimental data of Mallo et al. [Nouv. J. Chim. 8 (1984) 373] and Waton et al. [J. Phys. Chem. 88 (1984) 3301]. The reaction rate constants are two to four orders of magnitude smaller than typical rate constants of diffusion-controlled reactions of other acid–base equilibria. This is presumably due to the substantial structural change that is involved in the conversion from planar B(OH)₃ to tetrahedral B(OH)₄. The time required to establish the boric acid–borate equilibrium in seawater is calculated to be ∼95μs at temperature T=25°C and salinity S=35. Considering stable boron isotopes ¹¹B and ¹⁰B, the isotopic equilibration time is ∼125 μs. As a result, kinetic isotope effects during coprecipitation of boron in calcium carbonate are unlikely and therefore do not affect the use of stable boron isotopes as a paleo-pH recorder.     

Simulation of upper-ocean biogeochemistry with a flexible-composition phytoplankton model: C, N and Si cycling in the western Sargasso Sea

We report the first application of a biogeochemical model in which the major elemental composition of the phytoplankton is flexible, and responds to changing light and nutrient conditions. The model includes two phytoplankton groups: diatoms and non-siliceous picoplankton. Both fix C in accordance with photosynthesis-irradiance relationships used in other models and take up NO₃⁻ and NH₄⁺ (and Si(OH)₄ for diatoms) following Michaelis-Menten kinetics. The model allows for light dependence of photosynthesis and NO₃⁻ uptake, and for the observed near-total light independence of NH₄⁺ uptake and Si(OH)₄ uptake. It tracks the resulting C/N ratios of both phytoplankton groups and Si/N ratio of diatoms, and permits uptake of C, N and Si to proceed independently of one another when those ratios are close to those of nutrient-replete phytoplankton. When the C/N or Si/N ratio of either phytoplankton group indicates that its growth is limited by N, Si or light, uptake of non-limiting elements is controlled by the content of the limiting element in accordance with the cell-quota formulation of Droop (J. Mar. Biol. Ass. U.K 54 (1974) 825).We applied this model to the Bermuda Atlantic Time-series Study (BATS) site in the western Sargasso Sea. The model was tuned to produce vertical profiles and time courses of [NO₃⁻], [NH₄⁺] and [Si(OH)₄] that are consistent with the data, by adjusting the kinetic parameters for N and Si uptake and the rate of nitrification. The model then reproduces the observed time courses of chlorophyll-a, particulate organic carbon and nitrogen, biogenic silica, primary productivity, biogenic silica production and POC export with no further tuning. Simulated C/N and Si/N ratios of the phytoplankton indicate that N is the main growth-limiting nutrient throughout the thermally stratified period and that [Si(OH)₄], although always limiting to the rate of Si uptake by diatoms, seldom limits their growth rate. The model requires significant nitrification in the upper 200 m to yield realistic time courses and vertical profiles of [NH₄⁺] and [NO₃⁻], suggesting that NO₃⁻ is not supplied to the upper water column entirely by physical processes. A nitrification-corrected f-ratio (f_NC), calculated for the upper 200 m as: (NO₃⁻ uptake—nitrification)/(NO₃⁻ uptake+NH₄⁺ uptake) has annual values ranging from only 0.05–0.09, implying that 90–95% of the N taken up annually by phytoplankton is supplied by biological regeneration (including nitrification) in the upper 200 m. Reported discrepancies between estimates of organic C export based on seasonal chemical changes and POC export measured at the BATS site can be almost completely resolved if there is significant regeneration of NO₃⁻ via organic-matter decomposition in the upper 200 m.     

Chromium(VI) reduction by sulphur(IV) in aqueous solutions

The rates of the reduction of Cr(VI) with S(IV) were measured in deaerated NaCl solution as a function of pH, temperature and ionic strength. The rates of the reaction were found to be first order with respect to Cr(VI) and second order with respect to S(IV), in agreement with previous results obtained at concentrations two order higher than the present study. The reaction also showed a first-order dependence of the rates on the concentration of the proton and a small influence of temperature with an apparent energy of activation ΔH_app of 22.8 ± 3.4 kJ/mol. The rates were independent of ionic strength from 0.01 to 1 M. The rate of Cr(VI) reduction is described by the general expression

−d[Cr(VI)]/dt=k[Cr(VI)][S(IV)]²