The use of microbial siderophores for foliar iron application studies

Experiments were conducted to assess the distribution of foliar applied Fe-containing compounds using microbial siderophores. Fe was measured in leaf fluid obtained by centrifugation according to a determination method based on Fe chelation by desferrioxamine E and HPLC separation on a reversed phase column. To avoid sample Fe contamination, treatments were only applied to a part of the leaf following a systematic and reproducible procedure and iron concentration was exclusively determined in fluid obtained from non-treated leaf surfaces. The increase in leaf fluid Fe concentration associated with the distribution of leaf applied Fe-siderophores, Fe–EDTA and FeSO₄ × 7H₂O was evaluated using Vicia faba L., Nicotiana tabacum L. and Citrus madurensis Lour. plants. The method proved useful to investigate the process of leaf Fe penetration and its distribution within the plant. Evidence of the penetration and distribution of leaf applied Fe-rhizoferrin, Fe-coprogen hydrolysis products and Fe-dimerum acid is presented in this study.     

A direct method for quantification of non-transferrin-bound iron

A direct method for quantification of non-transferrin-bound iron has been developed. This assay relies on the use of a large excess of a low affinity ligand (nitrilotriacetic acid, NTA) which removes and complexes all low molecular weight iron and iron nonspecifically bound to serum proteins. Iron bound to transferrin, ferritin, desferrioxamine, and its metabolites is unaffected. The Fe-NTA complex present in the serum ultrafiltrate is then quantified using an automated HPLC procedure where on-column derivatization with a high affinity iron chelator (3-hydroxy-1-propyl-2-methyl-pyridin-4-one) takes place. The iron complexes of desferrioxamine and its metabolites are unaffected by the above-derivatization procedure. With minor modifications, this method is equally applicable for the quantification of low molecular weight iron in other biological fluids.     

Interaction between iron(II) and hydroxamic acids: oxidation of iron(II) to iron(III) by desferrioxamine B under anaerobic conditions

Interaction between iron(II) and acetohydroxamic acid (Aha), alpha-alaninehydroxamic acid (alpha-Alaha), beta-alaninehydroxamic acid (beta-Alaha), hexanedioic acid bis(3-hydroxycarbamoyl-methyl)amide (Dha) or desferrioxamine B (DFB) under anaerobic conditions was studied by pH-metric and UV-Visible spectrophotometric methods. The stability constants of complexes formed with Aha, alpha-Alaha, beta-Alaha and Dha were calculated and turned out to be much lower than those of the corresponding iron(II) complexes. Stability constants of the iron(II)-hydroxamate complexes are compared with those of other divalent 3d-block metal ions and the Irving-Williams series of stabilities was found to be observed. Above pH 4, in the reactions between iron(II) and desferrioxamine B, the oxidation of the metal ion to iron(III) by the ligand was found. The overall reaction that resulted in the formation of the tris-hydroxamato complex [Fe(HDFB)]+ and monoamide derivative of DFB at pH 6 is: 2Fe2+ + 3H4DFB+ = 2[Fe(HDFB)]+ + H3DFB-monoamide+ + H2O + 4H+. Based on these results, the conclusion is that desferrioxamine B can uptake iron in iron(III) form under anaerobic conditions.     

Investigation of ascorbate-mediated iron release from ferric phytosiderophores in the presence of nicotianamine

Phytosiderophores (PS) are strong iron chelators, produced by graminaceous plants under iron deficiency. The ability of released PS to chelate iron(III), and subsequent uptake of this chelate into roots by YS1-type transport proteins, are well-known. The mechanism of iron release from the stable chelate inside the plant cell, however, is unclear. One possibility involves the reduction of ferric PS in the presence of an iron(II) chelator via ternary complex formation. Here, the conversion of ferric PS species by ascorbate in the presence of the intracellular ligand nicotianamine (NA) has been investigated at cytosolic pH (pH 7.3), leading to the formation of a ferrous NA chelate. This reaction takes place when supplying Fe(III) as a chelate with 2'-deoxymugineic acid (DMA), mugineic acid (MA), and 3-epi-hydroxymugineic acid (epi-HMA), with the reaction rate decreasing in this order. The progress of the conversion of ferric DMA to ferrous NA was monitored in real-time by high resolution mass spectrometry (FTICR-MS), and the results are complemented by electrochemical measurements (cyclic voltammetry), which allows detecting reactive intermediates and their change with time at high sensitivity. Hence, the combined results of electrochemistry and mass spectrometry indicate an ascorbate-mediated mechanism for the iron release from ferric PS, which highlights the role of ascorbate as a simple, but effective plant reductant.     

Characterization of a novel Spirillum-like bacterium that degrades ferrioxamine-type siderophores

A novel Gram-negative Spirillum-like bacterium (ASP-1) was isolated from lake water by enrichment culture on desferrioxamine B as sole source of carbon and energy. ASP-1 was able to degrade the siderophores desferrioxamine B and E. The property of siderophore degradation was inducible in the presence of desferrioxamine B. The ferric complexes, however, were not measurably degraded but served as an iron source. Degradation of desferrioxamines in culture was followed by measuring the residual ferrioxamines colorimetrically at 430 nm after addition of iron. Degradation in cell-free assays was followed quantitatively by HPLC on a reversed-phase column measuring the time-dependent disappearance of the desferrioxamines B and E. Cell-free assays also revealed that degradation of the cyclic desferrioxamine E was rapid and complete, whereas degradation of the linear desferrioxamine B yielded two intermediate iron-binding metabolites of shorter chain length. Preparative isolation by HPLC and mass spectrometric analysis of the metabolites revealed masses at 361 and 419 a.m.u., respectively, suggesting a splitting at the two amide bonds. ASP-1 is a nitrogen fixing Spirillum bacterium which could also use ammonium and glucose or several organic acids as a carbon source but grew poorly with amino acids. Physiological comparisons with Aquaspirillum and Azospirillum failed to assign ASP-1 to any of the presently known Spirillum species. Based on 16S rDNA sequence analysis the strain could be placed within the radiation of the Azospirillum/Rhodocista group. The closest relative was Azospirillum irakense, showing 98.8% similarity.     

Humic acid and iron uptake by plants

Summary The behaviour of ferric EDTA and ferric citrate in nutrient solution and their interaction with humic acid was investigated at various hydrogen ion concentrations using the technique of membrane ultrafiltration to separate small iron species from high molecular weight products of hydrolysis and to estimate the binding of iron by humic acid. Ferric EDTA was found to be of small molecular size at all pH values between 5.0 and 7.0 whilst ferric citrate solutions contained an increasing proportion of high molecular weight material as pH was increased from 5.0 to 7.0. Some iron present in solutions of both ferric EDTA and ferric citrate was bound by humic acid at all pH values from 5.0 to 7.0. Studies were also made of the uptake of iron by wheat roots from nutrient solutions containing either ferric EDTA or ferric citrate and of the effect of humic acid on uptake. More iron was absorbed from ferric EDTA than from ferric citrate at all pH values. Increasing pH between 5.0 and 7.0 resulted in a progressive decrease in the uptake of iron in both cases. The presence of humic acid depressed iron absorption from both solutions at all pH values.     

Microbial ferric iron reductases

Almost all organisms require iron for enzymes involved in essential cellular reactions. Aerobic microbes living at neutral or alkaline pH encounter poor iron availability due to the insolubility of ferric iron. Assimilatory ferric reductases are essential components of the iron assimilatory pathway that generate the more soluble ferrous iron, which is then incorporated into cellular proteins. Dissimilatory ferric reductases are essential terminal reductases of the iron respiratory pathway in iron-reducing bacteria. While our understanding of dissimilatory ferric reductases is still limited, it is clear that these enzymes are distinct from the assimilatory-type ferric reductases. Research over the last 10 years has revealed that most bacterial assimilatory ferric reductases are flavin reductases, which can serve several physiological roles. This article reviews the physiological function and structure of assimilatory and dissimilatory ferric reductases present in the Bacteria, Archaea and Yeast. Ferric reductases do not form a single family, but appear to be distinct enzymes suggesting that several independent strategies for iron reduction may have evolved.     

Exchange of iron by gallium in siderophores

Siderophores are iron transport compounds produced by numerous microorganisms and which strongly chelate Fe(III), but not Fe(II). Other trivalent metals, such as Al(III), Cr(III), or Ga(III), are not capable of significantly displacing iron from siderophores. However, I demonstrate here that Ga(III) can effectively displace iron under reducing conditions. With ascorbate as reductant and ferrozine as Fe(II) trapping agent, the kinetics of reductive displacement of iron by Ga(III) were followed spectroscopically by the increase of absorbance at 562 nm due to formation of the Fe(II)-ferrozine complex. No significant reduction of siderophore occurred in the absence of Ga(III). With excess Ga(III), the displacement was quantitative and very rapid. The rate of metal exchange was pseudo first order with respect to Ga(III) concentration and highly pH dependent, suggesting that siderophore ligands are displaced from the iron in a concerted mechanism by Ga(III) and protonation to expose the Fe(III) to reduction by ascorbate. Reaction rates were dependent upon the structure of the siderophore, being greatest for ferric rhodotorulic acid and slowest for ferrichrome A at pH 5.4. The pH profile for ferric rhodotorulic acid was unusual in that it showed a maximum at pH 6.5, while all other siderophores examined showed an increase in rate as pH was lowered from 7.0. The physiological significance of this reaction to the clinical use of gallium is discussed.     

Ferrous ion formation by ferrioxamine prepared from aged desferrioxamine: A potential prooxidant property

The siderophore desferrioxamine (DEFOM) binds ferric ions in a 1:1 ratio resulting in a ferrioxamine (FOM) complex. When DEFOM is stored or heat degraded, the resulting FOMD undergoes an autoreduction with the transfer of electrons to the bound ferric ions forming ferrous ions, which react with Ferrozine to yield a pink-coloured complex absorbing at 562 nm. Heat-aged DEFOM forms a FOND complex with an absorption maxima changing from 432 nm to 441 nm. When the autoreduced FOMD complex is placed in a phosphate buffer at pH 7.4, ferrous ions autoxidase transferring electrons to molecular oxygen to form superoxide and hydrogen peroxide. Fenton chemistry leading to the formation of hydroxyl radicals can then occur. Studies with a variety of reactive oxygen scavengers support a role for the hydroxyl radical in damage to the detector molecule deoxyribose. However, when EDTA is present, damage to deoxyribose is decreased and the radicals causing deoxyribose degradation no longer appear to be characteristic of the hydroxyl radical.     

Oxidation of low-density lipoprotein by iron at lysosomal pH: implications for atherosclerosis

Low-density lipoprotein (LDL) has recently been shown to be oxidized by iron within the lysosomes of macrophages, and this is a novel potential mechanism for LDL oxidation in atherosclerosis. Our aim was to characterize the chemical and physical changes induced in LDL by iron at lysosomal pH and to investigate the effects of iron chelators and α-tocopherol on this process. LDL was oxidized by iron at pH 4.5 and 37 °C and its oxidation monitored by spectrophotometry and high-performance liquid chromatography. LDL was oxidized effectively by FeSO(4) (5-50 μM) and became highly aggregated at pH 4.5, but not at pH 7.4. The level of cholesteryl esters decreased, and after a pronounced lag, the level of 7-ketocholesterol increased greatly. The total level of hydroperoxides (measured by the triiodide assay) increased up to 24 h and then decreased only slowly. The lipid composition after 12 h at pH 4.5 and 37 °C was similar to that of LDL oxidized by copper at pH 7.4 and 4 °C, i.e., rich in hydroperoxides but low in oxysterols. Previously oxidized LDL aggregated rapidly and spontaneously at pH 4.5, but not at pH 7.4. Ferrous iron was much more effective than ferric iron at oxidizing LDL when added after the oxidation was already underway. The iron chelators diethylenetriaminepentaacetic acid and, to a lesser extent, desferrioxamine inhibited LDL oxidation when added during its initial stages but were unable to prevent aggregation of LDL after it had been partially oxidized. Surprisingly, desferrioxamine increased the rate of LDL modification when added late in the oxidation process. α-Tocopherol enrichment of LDL initially increased the rate of oxidation of LDL but decreased it later. The presence of oxidized and highly aggregated lipid within lysosomes has the potential to perturb the function of these organelles and to promote atherosclerosis.     

Effects of iron and desferrioxamine on Rhizopus infection

To investigate the association among iron, desferrioxamine, and a Rhizopus infection, the influence of iron and/or desferrioxamine on experimental mucormycosis in mice was examined. All mice pretreated with iron, desferrioxamine, or a combination of iron and desferrioxamine died within 5 days after the inoculation of R. oryzae. In the mice fungal lesions were observed in the brain which resembled human cerebral mucormycosis. By contrast, the mortality in the control mice with R. oryzae was 20% through the 3-week experimental period. Therefore, it was demonstrated that iron as well as desferrioxamine administration markedly promotes the growth of R. oryzae. The increased susceptibility to R. oryzae was considered to be due to increased serum iron in the animals pretreated with iron only; however, pretreatment with desferrioxamine did not affect the amount of serum ion. Thus, the data suggest that desferrioxamine acts as a siderophore to R. oryzae and exerts an adverse effect on mucormycosis. This study has shown that the presence of iron and desferrioxamine enhances the virulence and pathogenicity of R. oryzae by serving as a growth factor.     

Physical evidence that yeast frataxin is an iron storage protein

Frataxin is a conserved mitochondrial protein required for iron homeostasis. We showed previously that in the presence of ferrous iron recombinant yeast frataxin (mYfh1p) assembles into a regular multimer of approximately 1.1 MDa storing approximately 3000 iron atoms. Here, we further demonstrate that mYfh1p and iron form a stable hydrophilic complex that can be detected by either protein or iron staining on nondenaturing polyacrylamide gels, and by either interference or absorbance measurements at sedimentation equilibrium. The molecular mass of this complex has been refined to 840 kDa corresponding to 48 protein subunits and 2400 iron atoms. Solution density measurements have determined a partial specific volume of 0.58 cm(3)/g, consistent with the amino acid composition of mYfh1p and the presence of 50 Fe-O equivalents per subunit. By dynamic light scattering, we show that the complex has a radius of approximately 11 nm and assembles within 2 min at 30 degrees C when ferrous iron, not ferric iron or other divalent cations, is added to mYfh1p monomer at pH between 6 and 8. Iron-rich granules with diameter of 2-4 nm are detected in the complex by scanning transmission electron microscopy and energy-dispersive X-ray spectroscopy. These findings support the hypothesis that frataxin is an iron storage protein, which could explain the mitochondrial iron accumulation and oxidative damage associated with frataxin defects in yeast, mouse, and humans.     

Ferrous iron dependent nitric oxide production in nitrate reducing cultures of Escherichia coli

l-Lactate-driven ferric and nitrate reduction was studied in Escherichia coli E4. Ferric iron reduction activity in E. coli E4 was found to be constitutive. Contrary to nitrate, ferric iron could not be used as electron acceptor for growth. Ferric iron reductase activity of 9 nmol Fe²⁺ mg^-1 protein min^-1 could not be inhibited by inhibitors for the respiratory chain, like Rotenone, quinacrine, Actinomycin A, or potassium cyanide. Active cells and l-lactate-driven nitrate respiration in E. coli E4 leading to the production of nitrite, was reduced to about 20% of its maximum activity with 5 mM ferric iron, or to about 50% in presence of 5 mM ferrous iron. The inhibition was caused by nitric oxide formed by a purely chemical reduction of nitrite by ferrous iron. Nitric oxide was further chemically reduced by ferrous iron to nitrous oxide. With electron paramagnetic resonance spectroscopy, the presence of a free [Fe²⁺-NO] complex was shown. In presence of ferrous or ferric iron and l-lactate, nitrate was anaerobically converted to nitric oxide and nitrous oxide by the combined action of E. coli E4 and chemical reduction reactions (chemodenitrification).     

Intra- and intercellular iron trafficking and subcellular compartmentation within roots

Iron is abundant in most soils, but ferric compounds are almost insoluble. Therefore, plant roots use as tools acidification and enzymatic reduction of iron at the outer cell surface (strategy I) or solubilization by phytosiderophores, which are specific ferric chelators (strategy II). In the first case, iron is taken up as Fe²⁺ into the root symplast, and in the latter one, iron is taken up as Fe(III) complex. The path of iron from the root surface, up to the point of the xylem vessels within the central cylinder, may be completely symplasmic. However, a part of this route also may be an apoplasmic one, through the free space of the cell walls of rhizodermis and cortex (apoplast). In the endodermis, the Casparian band forms a strict barrier for apoplasmic transport; to move past this site, all ions must enter the symplast. During symplasmic transport, the intracellular environment is protected against the reactive species of iron by handling of iron in chelated forms. A promising candidate for this purpose is the plant-endogenous chelator nicotianamine. At the apoplasmic site, iron can be oxidized followed by precipitation as hydroxide or phosphate compounds. Thus, a pool of apoplastic iron can be formed, as shown by reductive mobilization or by proton-induced X-ray emission. This pool may be remobilized when iron deficiency takes place. During radial transport to the vessels, vacuoles may compete with the transport stream forming an iron store. When there is an iron excess, as in plants growing in waterlogged soils or by experimental techniques, plants can escape the deleterious effects of free iron by depositing it in phytoferritin, a storage protein inducible under iron excess. Also, nicotianamine forms a pool of metabolically available iron. Thus, in roots cells of the nicotianamine-free tomato mutant chloronerva iron precipitations occur as evidenced by energy dispersive X-ray analysis and the electron microscopic energy loss technique of energy spectroscopic imaging. Future research concerning the plant root's iron metabolism are needed to clarify the function of nicotianamine in intra- and intercellular iron trafficking and to identify the so-called iron-sensor which mediates the regulation of iron acquisition reactions of rhizodermal cells in response to the iron nutritional status of the plant.     

Functional characterization of the FoxE iron oxidoreductase from the photoferrotroph Rhodobacter ferrooxidans SW2

Photoferrotrophy is presumed to be an ancient type of photosynthetic metabolism in which bacteria use the reducing power of ferrous iron to drive carbon fixation. In this work the putative iron oxidoreductase of the photoferrotroph Rhodobacter ferrooxidans SW2 was cloned, purified, and characterized for the first time. This protein, FoxE, was characterized using spectroscopic, thermodynamic, and kinetic techniques. It is a c-type cytochrome that forms a trimer or tetramer in solution; the two hemes of each monomer are hexacoordinated by histidine and methionine. The hemes have positive reduction potentials that allow downhill electron transfer from many geochemically relevant ferrous iron forms to the photosynthetic reaction center. The reduction potentials of the hemes are different and are cross-assigned to fast and slow kinetic phases of ferrous iron oxidation in vitro. Lower reactivity was observed at high pH and may contribute to prevent ferric iron precipitation inside or at the surface of the cell. These results help fill in the molecular details of a metabolic process that likely contributed to the deposition of precambrian banded iron formations, globally important sedimentary rocks that are found on every continent today.     

An in vitro examination of intestinal iron absorption in a freshwater teleost, rainbow trout (Oncorhynchus mykiss)

This study investigated the physiological characteristics of intestinal iron absorption in a freshwater teleost, rainbow trout (Oncorhynchus mykiss). Using an in vitro gastro-intestinal sac technique, we evaluated the spatial pattern and concentration dependent profile of iron uptake, and also the influence of luminal chemistry (pH and chelation) on iron absorption. We demonstrated that the iron uptake rate in the anterior intestine is significantly higher than that in the mid and posterior intestine. Interestingly, absorption of iron in the anterior intestine occurs likely via simple diffusion, whereas a carrier-mediated pathway is apparent in the mid and posterior intestine. The uptake of ferric and ferrous iron appeared to be linear over the entire range of iron concentration tested (0–20 μM), however the uptake of ferrous iron was significantly higher than that of ferric iron at high iron concentrations (>15 μM). An increase in mucosal pH from 7.4 to 8.2 significantly reduced iron absorption in both mid and posterior intestine, implying the involvement of a Fe²⁺/H⁺ symporter. Iron chelators (nitrilotriacetic acid and desferrioxamine mesylate) had no effects on iron absorption, which suggests that fish are able to acquire chelated iron via intestine.     

Influence of pH on the balance between methanogenesis and iron reduction

Methanogenesis and iron reduction play major roles in determining global fluxes of greenhouse gases. Despite their importance, environmental factors that influence their interactions are poorly known. Here, we present evidence that pH significantly influences the balance between each reaction in anoxic environments that contain ferric (oxyhydr)oxide minerals. In sediment bioreactors that contained goethite as a source of ferric iron, both iron reduction and methanogenesis occurred but the balance between them varied significantly with pH. Compared to bioreactors receiving acidic media (pH 6), electron donor oxidation was 85% lower for iron reduction and 61% higher for methanogenesis in bioreactors receiving alkaline media (pH 7.5). Thus, methanogenesis displaced iron reduction considerably at alkaline pH. Geochemistry data collected from U.S. aquifers demonstrate that a similar pattern also exists on a broad spatial scale in natural settings. In contrast, in bioreactors that were not augmented with goethite, clay minerals served as the source of ferric iron and the balance between each reaction did not vary significantly with pH. We therefore conclude that pH can regulate the relative contributions of microbial iron reduction and methanogenesis to carbon fluxes from terrestrial environments. We further propose that the availability of ferric (oxyhydr)oxide minerals influences the extent to which the balance between each reaction is sensitive to pH. The results of this study advance our understanding of environmental controls on microbial methane generation and provide a basis for using pH and the occurrence of ferric minerals to refine predictions of greenhouse gas fluxes.     

Effects of iron on Vitamin C/copper-induced hydroxyl radical generation in bicarbonate-rich water

The aim of this study was to evaluate whether iron, like copper, could support Vitamin C mediated hydroxyl radical formation in bicarbonate-rich water. By using the hydroxyl radical indicator coumarin-3-carboxylic acid, we found that iron, in contrast to copper, was not capable to support Vitamin C induced hydroxyl radical formation. However, when 0.2 mg/l iron and 0.1 mg/l copper were both added to bicarbonate supplemented Milli-Q water, the Vitamin C induced formation of 7-hydroxycoumarin, as measured by HPLC analysis, was inhibited by 47.5%. The inhibition of hydroxyl radical formation by iron was also evident in the experiments performed on copper contaminated bicarbonate-rich household drinking water samples. In the presence of 0.2 mg/l of ferric iron the ascorbic acid induced hydroxyl radical formation was inhibited by 36.0-44.6%. This inhibition was even more significant, 47.0-59.2%, when 0.8 mg/l of ferric iron was present. None of the other redox-active metals, e.g. manganese, nickel or cobalt, could support ascorbic acid induced hydroxyl radical formation and did not have any impact on the ascorbic acid/copper-induced hydroxyl radical generation. Our results show, that iron cannot by itself produce hydroxyl radicals in bicarbonate rich water but can significantly reduce Vitamin C/copper-induced hydroxyl radical formation. These findings might partly explain the mechanism for the iron-induced protective effect on various copper related degenerative disorders that earlier has been observed in animal model systems.     

Uptake of iron by apoferritin from a ferric dihydrolipoate complex

A study was made on the uptake of iron by horse spleen apoferritin, by using as an iron source the same ferric dihydrolipoate complex which represents the major product in the anaerobic removal of ferritin-bound iron by dihydrolipoate at neutral pH. The ferric dihydrolipoate complex was chemically synthesized and used as an iron donor to apoferritin. Iron uptake was studied, at slightly alkaline pH and in anaerobic conditions, as a function of the concentration of both the iron donor and apoferritin. Isolation of ferritin from mixtures of ferric dihydrolipoate and apoferritin, and subsequent identification of the oxidation state of ferritin-bound iron, showed that the first metal atoms were taken up in the ferrous form and that this early step was accompanied by accumulation of ferric iron. Total iron uptake increased with the molar ratio of complex to apoprotein and ranged over 25-40% of the iron being supplied. The amount of ferrous iron found inside the protein did not exceed 50-60 mol iron/mol ferritin after a 48-h incubation. At this time, ferric iron represented a significant fraction of the iron found in the isolated ferritin. Analytical and spectroscopic data indicated that fractional rates and equilibria for disassembly of the ferric complex in the presence of apoferritin were independent of the concentration of the protein and of the complex itself.     

Separation of cellular iron containing compounds by electrophoresis

High resolution separation of metalloproteins and other iron compounds based on native gel electrophoresis followed by⁵⁹Fe autoradiography is described. Lysates of mouse spleen erythroid cells metabolically labeled with⁵⁹Fe-transferrin were separated on 3–20% polyacrylamide gradient gels in the presence of Triton X100 and detected by autoradiography. In addition to ferritin and hemoglobin, several compounds characterized by their binding of iron under different conditions were described. Iron chelatable by desferrioxamine migrated in the region where several high-molecular weight compounds were detected by silver staining. The technique is nondissociative, allowing identification of iron compounds with the use of specific antibodies. Cellular iron transport and the action of iron chelators on specific cellular targets can be investigated in many small biological samples in parallel.