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Review

Soil Chemistry Factors Confounding Crop Salinity Tolerance—A Review

by
Pichu Rengasamy
School of Agriculture, Food and Wine, Prescott Building, Waite Campus, The University of Adelaide, Adelaide, 5005 SA, Australia
Agronomy 2016, 6(4), 53; https://0-doi-org.brum.beds.ac.uk/10.3390/agronomy6040053
Submission received: 26 August 2016 / Revised: 18 October 2016 / Accepted: 25 October 2016 / Published: 29 October 2016
(This article belongs to the Special Issue Crop Salinity Tolerance)
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Abstract

:
The yield response of various crops to salinity under field conditions is affected by soil processes and environmental conditions. The composition of dissolved ions depend on soil chemical processes such as cation or anion exchange, oxidation-reduction reactions, ion adsorption, chemical speciation, complex formation, mineral weathering, solubility, and precipitation. The nature of cations and anions determine soil pH, which in turn affects crop growth. While the ionic composition of soil solution determine the osmotic and ion specific effects on crops, the exchangeable ions indirectly affect the crop growth by influencing soil strength, water and air movement, waterlogging, and soil crusting. This review mainly focuses on the soil chemistry processes that frustrate crop salinity tolerance which partly explain the poor results under field conditions of salt tolerant genotypes selected in the laboratory.

1. Introduction

The aqueous components of a soil at different water contents in the field determine the abiotic stress experienced by plants during their growth, consequently affecting the crop yield [1]. In salt-affected soils, the total concentration of dissolved salts in soil solutions, generally measured as the electrical conductivity (EC) of the soil solutions, is considered as the primary criterion affecting the yield (e.g., [2]). Thus, most of the research on crop salinity tolerance has focussed on EC of soil solutions inducing osmotic pressure affecting water uptake by plants and the accumulation of specific ions in the plant over a period of time leading to ion toxicity or ion imbalance [3]. Because of the common opinion that sodium chloride (NaCl) is the predominant salt in saline soils, ionic effects of sodium (Na) and chloride (Cl) have received more attention.
However, the composition of electrolytes, in addition to the total concentration, determines the multi-phase equilibria involving: (1) the solid phase comprising clay minerals and other inorganic and organic materials, (2) the liquid phase comprising soil water, (3) the gaseous phase comprising mainly oxygen and carbon dioxide, and (4) the complex exchange phase [4,5]. During crop growth in the field soil water fluctuates from high to very low levels and the chemical equilibria become more complex. Exchange reactions are determined by the nature of cations and anions, and as a result soil physical conditions are altered leading to the limitations to crop growth caused by increased soil strength and reduced water and air movement. Plant roots need a well-hydrated and well aerated soil environment of low osmotic pressure, with adequate nutrients and low toxicity. Soil pH, which depends on the composition of cations and anions and its relation with pE (electron activity related to redox potential), is changed by soil water regime, control solubility, and precipitation reactions. These processes result in the toxicity and deficiency of macro and micro- nutrient elements. Variations in soil chemistry impact on most of the plant requirements: soil structure, osmotic potential of the soil solution, soil aeration, and the presence of toxic ions. Thus ‘salinity stress’ is complicated by many soil chemical processes. This review addresses the soil chemistry factors including chemical reactions and composition of soil solution interfering with crop salinity tolerance. It is asserted here that these factors could be partly responsible for the marked differences in the response to salinity found between laboratory and field grown plants, although a detailed discussion of these differences is not part of this review.

2. Soil Processes Affecting Soil Solution Composition

A number of soil processes in the soil environment influence the activities of chemical species in soil water. In addition to soil components, factors related to climate and soil management also influence these processes, which are summarised in Table 1. In general, at equilibrium, a change in one parameter effects changes in all variables.

3. Ion Exchange and Resultant Soil Structural Stability

Soil components, including clay minerals and inorganic and organic compounds have their inherent charge (+ or −), but when they are aggregated, the net charge may be different from the total charge depending on the bonding type between the components [7]. Covalent bonding between the components results in a reduction in net charge. The net charge if negative is balanced by adsorbing cations, and if positive by adsorbing anions. These adsorbed ions can change according to the concentration and the nature of the ions in solutions. Most of agricultural soils, except in tropical climates, have a net negative charge and cation exchange is the primary process, whereby cations are adsorbed in the exchange phase from the solutions of salt-affected soils. Water molecules react with the charge on soil particles inducing a weakening of soil aggregates, and as a consequence aggregates slake and clay particles disperse. These charges can vary according to soil pH [8].
The majority of salt-affected soils are dominated by sodium salts [9] and hence the exchange phase is dominated by Na. The adsorption of Na in the exchange phase from soil water depends on the proportion of divalent cations in soil solution, usually indicated by the sodium adsorption ratio (SAR) measured in soil solutions. Exchangeable sodium percentage (ESP) is related to SAR, and when it exceeds a threshold level swelling and dispersion of soil clays lead to the degradation of soil physical properties resulting in reduced water and air flow, high soil strength, and soil crusting. These physical conditions severely restrict germination, root growth, and the physiological functions of crops [10].
Recent studies have shown that, in addition to sodium, exchangeable potassium and magnesium can also increase soil swelling and dispersion affecting soil physical properties [11,12,13,14,15]. The effects of these cations in causing swelling and dispersion are not similar, but depend on the ionicity index [14], a molecular scale geochemical parameter which estimates the relative bonding (ionic and covalent) tendency of a cation with charged particles. Swelling and dispersion increase as the ionicity of the bonding increases in the order Na > K > Mg > Ca. Incorporating the effects of the cationic valence in addition to the ionicity factor, Rengasamy [16] derived the dispersive powers of these cations relative to Ca. They are: Ca = 1, Mg = 1.7, K = 25, and Na = 45. While, in dry soils, the exchangeable cations react with water molecules inducing clay dispersion, the soluble cations present in soil water oppose the dispersive reactions because of their flocculating powers [17], and relative to Na, they are: Ca = 45, Mg = 27, K = 1.8, and Na = 1. The flocculating powers of these cations were derived on the basis of covalency factor (the degree of covalency in cation-clay bonding) and the effects of cationic valence.
Recently, Rengasamy et al. 2016 [18] proposed a new concept of “net dispersive charge” which determines the amount of clay dispersed from a dispersive soil, and is defined as:
Net dispersive charge = dispersive charge − flocculating charge
The dispersive charge of a soil is derived from the concentrations of exchangeable cations (cmolc·kg−1) measured at the given soil pH, weighted by the respective dispersive power, and is defined as:
Dispersive charge (cmolc·kg−1) = (Ca) + 1.7 (Mg) + 25 (K) + 45 (Na).
Similarly, the flocculating charge is derived from the concentrations of the cations (cmolc·kg−1 on soil basis) in the dispersed soil-water suspension, weighted by the respective flocculating power, and is defined as:
Flocculating charge (cmolc·kg−1) = 45 (Ca) + 27 (Mg) + 1.8 (K) + (Na).
When the dispersive charge is above a threshold value, clay particles dissociate and form a diffuse double layer [19]. The flocculating effects of cations operate only when a diffuse double layer is developed. At lower dispersive charge, soil aggregates slake as macro aggregates break into micro aggregates; this process is not affected by the electrolyte concentration (i.e., salinity) of the soil solution [20].
If the flocculating charge contributed by the cations in a saline soil is equal to or greater than the dispersive charge, the soil structural effects of salinity will be minimal and crop growth is mainly affected by osmotic and ion toxicity effects. When the flocculating charge is lower than the dispersive charge, degradation of soil physical conditions will affect crop growth confounding the salt tolerance of crops (Figure 1). When the electrolyte concentration is low, cations do not reach toxic concentrations in the soil solution. For example, non-saline soils with high exchangeable sodium and low EC do not have toxic levels of sodium in soil solutions [1]. Thus, seasonal changes in salt concentration in the field will determine whether soil structural effect or salinity effect influence crop performance.
Because of the difficulties in the estimation of exchangeable cations, cations estimated in soil solution have been used to derive SAR to predict ESP and associated soil physical conditions. However, K is not included in the derivation of SAR and Mg is considered as equal to Ca in the SAR model. Rengasamy and Marchuk [9] have proposed the “cation ratio for soil structural stability (CROSS)” which is defined as follows:
CROSS = (Na + 0.56 K)/(Ca + 0.6 Mg) 0.5 where the concentrations of cations are expressed in mmol/L. CROSS includes the dispersive effects of K in relation to Na, and the flocculating effect of Mg in relation to Ca. CROSS has been found to be effective in predicting clay dispersion and soil physical behaviour, particularly when K and Mg are present in significant amounts in soils.

4. Soil pH in Relation to Measurement Techniques

The dissolved cations and anions react with water molecules producing hydrogen ions. The measurement of pH using electrodes indicates the activity of hydrogen ions rather than their concentration. Hydrolysis of water molecules by cations and anions changes the pH of soil solutions to be either acidic or alkaline [21]. In addition, ionic strength determined by the concentration and valence of the ions influences the activity of hydrogen ions. The ionic strength of a soil solution (affected by measurement in electrolyte solutions such as CaCl2 or highly saline soil solutions) can affect soil pH (e.g., [22]). In acidic soils, cations in electrolyte solutions can replace exchangeable H+ or Al3+ which in soil solutions can decrease soil pH. However, in alkaline soils, with exchangeable H+ or Al3+ being absent, hydrolysis by anions or other cations contributes to the changes in pH due to electrolyte levels. Measuring pH in soil suspensions instead of soil-water extracts introduces the effect of liquid junction potential or Donnan membrane potential associated with soil colloids on hydrogen ion activity [23]. Acid producing biological reactions such as nitrification can increase hydrogen ions and also ionic strength. Increase in ionic strength in acidic soil solution can change pH without any appreciable change in titratable acidity [24]. Variations of pH in different soil-water ratios, such as 1:5, 1:1, or saturation extract, are associated with changes in ionic strength and the concentration of individual ions involved in hydrolysis. Thus, many factors have to be considered in the interpretation of measured soil pH values.

5. Role of Cations and Anions in Soil pH

Hydrolysis of cations, anions, and organic substances with different functional groups play a vital role in the equilibrium of soil pH. The acidic pH (<6) of highly weathered soils with low basic exchangeable cations like Ca2+, Mg2+, K+, and Na+ arises mainly because of the hydrolysis of the cations Fe and Al [21]. By contrast, the soils of arid regions usually have alkaline pH (>7) and contain mainly Ca2+, Mg2+, K+, and Na+ as exchangeable cations. Conventionally, these cations have been called base or base-forming cations, and hydrolysis of these cations is assumed to cause alkaline pH. Brady and Weil et al 2008 described them as “non-acid cations” different from acid cations such as H+ and Al3+ [25]. Tavakkoli et al. 2015 showed that when a soil with >90% exchangeable Na+ had near neutral pH when accompanying anions were Cl− and SO42− and alkaline pH (>8) when accompanying anions were HCO3− and CO32− [21]. The weak hydrolysis reactions of Cl− and SO42− result in a small change from neutral pH. However, the hydrolysis of HCO3− and CO32− produce higher concentrations of OH− resulting in higher pH. They also showed that by increasing the ionic strength of an alkaline soil (pH 9.82) with NaCl that pH was reduced to 8.32, whereas by increasing the ionic strength by adding CaCl2, pH was reduced below 8; the precipitation of CO32− as CaCO3 was also involved in pH decrease. Al-Busaidi and Cookson 2003 found a negative relationship between soil pH and salinity (EC) in soils in Oman, the main factor contributing to this inverse relationship being the presence of soluble Ca2+ ions [26]. Thus, saline-alkaline soils have lower pH compared to alkaline soils with low ionic strength. Therefore, it is necessary to measure electrolyte concentration and composition in the interpretation of soil pH.

6. Toxicity and Deficiency of Nutrient Elements in Relation to Soil pH

Increasing salinity leads to accumulation of ions in the plant over a period of time and leads to ion toxicity or ion imbalance. However, soil pH determines the solubility, complexation, and precipitation of ionic species in soil solution affecting the ion uptake and also the root growth. Sposito 2008 has summarised the principal cationic species in relation to acidic or alkaline soil pH (Table 2). The distribution of dissolved ionic species in soil solution can be derived from their total concentrations, pH, concentration of ligands, conditional stability constants for all possible complexes, and the expressions for the mass balance of each ion [8].
For example, at low soil pH (<5), the solubility of Al from clay minerals introduce toxic cationic hydroxy species of Al which mainly affect the root growth [27]. When soil pH increases to >9, Al forms soluble anionic species such as Al (OH)4− which also affects root growth [28]. By contrast, Al-organic complexes are not toxic to crops because they are not taken up by the roots. The adsorption and desorption of ionic species by soil clays depend on soil pH which influences the charge on clays and also on the ionic species, which can lead to either deficiency or toxicity of elements. Confounding the interpretation of salinity-boron interactions is the influence of the pH of the soil solution [29]. Thus, boron adsorption on a calcareous Entisol is highly enhanced above pH 9.2 [30], when boron deficiency can be encountered. When the pH exceeds 8, the speciation of boron starts to progressively shift from boric acid B(OH)3 to anionic borate B(OH)4−. At lower soil pH values, boron availability in soil solutions may be high and may hence become toxic. Different categories of salt-affected soils based on EC, SAR, and pH have different effects on nutrient toxicity and deficiency, and these are summarised below in Table 3.

7. Soil Organic Matter and the Chemistry of Soil Solution

Soil organic matter is important in improving soil qualities such as soil structure, soil fertility, and microbial activity. The functions of soil organic matter will vary according to different fractions viz. particulate organic carbon, humus organic carbon, resistant organic carbon, and dissolved organic carbon [33]. Organic matter can improve aggregate stability by decreasing dispersive charge by covalent boding with soil surface charge. Hydrophobic organic fractions can prevent water interaction (wettability) and prevent aggregate breakdown. However, simple organic molecules with negative charge can increase soil dispersivity, as observed when farmyard manures containing uronic acid are applied to salt-affected soils [34]. The presence of uncomplexed carboxylic acids can reduce soil pH. Strong adsorption of Fe and Al species by organic matter can effectively reduce proton concentration (H+) in soil solution [35]. Dissolved organic carbon in soil solution is highly influenced by soil pH; higher dissolution of organic carbon is observed in high pH soils containing HCO3- and CO32− ions [21]. Charged fractions of organic matter can contribute to the anion or cation exchange capacity of soils in a similar manner to of clay minerals. Microbial decomposition of organic matter can releases a myriad of organic compounds into the soil solution, these include particularly important plant nutrient elements such as N, P, and S.

8. Dispersive Soils and Waterlogging

The fertility of dispersive soils with low nutrient reserves is compounded both by the low supply of water and by the low supply of oxygen to roots in dispersive soil layers. When the top soils are dispersive, waterlogging or reduction in aeration porosity of these layers lead to ion toxicity and deficiency due to changes in electron and proton activities (pE and pH) in an environment of degraded soil structure [18]. The redox status of a soil is described by the free electron activity, pE (−log (e−), where e− denotes electron), in conjunction with proton activity (pH). The relationships of pH and pE control oxidized or reduced ionic species in soil solution. Free electron activity (pE) at pH 7 for some equilibrium chemical reactions under anoxic and suboxic conditions [36] in dispersive soils are given in Table 4. Waterlogging may affect microelement concentrations in soil solutions by changes in pE, or it may affect plant roots through either changes in energy (ATP) supply or membrane integrity [37]. Under waterlogged conditions, Setter et al. 2009 found significant increases in shoot concentrations of Mn, Fe, Na, B, and Al above critical concentrations for toxicity in wheat growing soils in India and Australia [38]. The interaction between waterlogging and salinity increases the abiotic stress experienced by plants [39,40]. High dispersivity, high pH, and the low biological activity encountered in alkaline dispersive soils are not conducive for either the accumulation of organic matter or its mineralization [21]. Poor leaching conditions in these soils lead to the accumulation of toxic elements such as boron [41].

9. Variations in Soil Water Content and Changes in Total Water Potential and Ionic Composition

Under field conditions, particularly in dryland cropping with climatic variations, soil water content fluctuates depending on rainfall and evapotranspiration. The total water potential including matric and osmotic potentials will change proportionally to the salt concentration affected by soil water content. As the soil dries due to evapotranspiration, the salt concentration increases as does the osmotic pressure of soil water. Rengasamy 2010 has described a field study in South Australia where fluctuations in soil water content during the growing season led to variations in total water potential and how this caused the reduction in wheat yield [1]. Similarly, Setter et al. 2016 have detailed how changes in soil water regime influenced by rain affected the productivity of wheat and barley in dryland saline land in Western Australia [38]. Studies on yield response due to simultaneous changes in salt concentration and water content are rare. Scientists have attempted to predict yield response in relation to the subsurface solution salinity averaged spatially and temporally (e.g., [42]). Furthermore, the changes in ionic composition and exchangeable cation composition with changes in water content in the field have not been studied in detail. Wada and Otani 1998 [43] and Oster and McNeal 1971 [44] have attempted modelling of soil solution composition with variations in water content. Misra and Tyler 1999 have indicated the variations in nutrient contents influenced by changes in soil water content [45]. It has to be remembered that plants growing in soils necessarily respond to the actual soil solution concentration and composition and not to the values calculated from the extracts of salts at artificial soil water contents [46].

10. Conclusions

Crop salinity tolerance is compounded by a range of environmental factors including soil chemistry. Chemical processes such as solubility and ionic speciation dictated by the nature of cations and anions in saline soil solutions lead to nutrient deficiency or ion toxicity. Cation and anion interactions control soil pH and associated soil constraints to crops. Adsorption of cations from saline soil solutions affects soil structural stability and soil physical conditions indirectly affecting crop growth through changes in soil strength, aeration, porosity, movement of water and nutrients, and the pH-pE relationship. Furthermore, under field conditions, fluctuating levels of soil water content not only alters the total salt concentration (osmotic potential) but also the composition of constituent cations and anions [1].
Combining soil chemistry induced stresses with salt concentration related stresses may explain some of the difficulties that plant breeders are having in the development of salt tolerant crops with high growth and yield in the field. The failure of laboratory-bred NaCl-tolerant cultivars to perform well under field conditions may reflect the effects of sodicity and alkalinity [47]. In the field, crops are routinely subjected to a combination of different abiotic stresses [48]. Thus, rather than investigating the phylogenetic distribution of tolerance to one particular stress, such as salinity, one should consider the distribution of tolerance to a range of environmental stresses [49]. Henderson and Gilliham 2015 have suggested, on the basis of molecular processes occurring in different cell types within plant roots [50], the identification of the “gatekeeper” cell type which plays a key role in tolerance to a particular stress. Future research programs should focus on tolerance to combinations of different stress conditions, particularly those that occur in field environment [48].

Acknowledgments

The author thanks the Grain Research and Development Corporation of Australia for the financial support (GRDC project UA 00159).

Conflicts of Interest

The author declares no conflict of interest.

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Figure 1. Schematic diagram distinguishing saline, saline-dispersive, and dispersive soils in relation to dispersive charge, flocculating charge, and the percentage of dispersed clay. Saline soils affect plant growth through ion toxicity and osmotic effect. Dispersive soils affect plant growth because of poor soil physical conditions. Combinations of these mechanisms are likely to be responsible for poor crop performance in saline-dispersive soils. Ion toxicity or imbalance depends on the concentration and composition of aqueous ions.
Figure 1. Schematic diagram distinguishing saline, saline-dispersive, and dispersive soils in relation to dispersive charge, flocculating charge, and the percentage of dispersed clay. Saline soils affect plant growth through ion toxicity and osmotic effect. Dispersive soils affect plant growth because of poor soil physical conditions. Combinations of these mechanisms are likely to be responsible for poor crop performance in saline-dispersive soils. Ion toxicity or imbalance depends on the concentration and composition of aqueous ions.
Agronomy 06 00053 g001
Table
Table 1. Soil chemical processes affecting ionic composition and their chemical reactivity in soil solutions [6].
Table 1. Soil chemical processes affecting ionic composition and their chemical reactivity in soil solutions [6].
MechanismEffects
Ion exchangeClay minerals, organic matter and other amorphous compounds with inherent charges (negative and/or positive) are bonded to each other in soil aggregates, with the nature of the bonding determining the charge available for water interaction and ion exchange. Electrolyte concentration and soil pH alter this charge. The nature of cations or anions influences the ion exchange reactions changing in the distribution of ions in the exchange phase and soil solution at equilibrium.
Dissolution and precipitationThe partial pressure of CO2 affects the dissolution and precipitation of soil carbonates and bicarbonates and ion activities including that of protons (H+). Organic matter controls ligand exchange and chelation resulting in ionic complexes which alter the reactivity of the ions in aqueous suspensions.
Soil pH (proton activity), determined by the reactions of cations and anions, is the primary factor in the dissolution and precipitation of inorganic minerals and organic compounds. Waterlogging alters soil pH and pE (electron activity) and their relationship affecting the nature of chemical species. Waterlogging also decreases concentrations of oxygen in the soil solution which impact on the availability of metabolic energy to root cells, therefore affecting plant growth and processes like ion uptake and ion exclusion.
Ion-pair formationHigh proportions of anions result in ion-pair formation and reduced ion activity.
Chemical speciationDissolved ions in soil solutions can exist as ‘free’ (e.g., Na+, surrounded by water molecules) and also as stable complexes (e.g., Al-hydroxy species). The formation of complexes depends on stability constants relating to the concentration of complexes and free ionic species. In soil solutions pH is an important factor in the formation of the complex species. The reactivity of free and complex species differs according to the changes in their charge.
Specific adsorptionInner-sphere complexation (or ion fixation) involves covalent bonding of ions with soil particles. This phenomenon alters the particle charge available for outer-sphere complexation and readily exchangeable ions.
Microbial reactionsBiological reactions due to soil microbes lead to the decomposition, oxidation, and polymerization of organic matter, and the release of hydrophilic and hydrophobic compounds controlling the chemical reactivity of soil solutions.
Table
Table 2. Principal cationic species in soil solution in relation to pH [8].
Table 2. Principal cationic species in soil solution in relation to pH [8].
CationAcidic SoilsAlkaline Soils
Na+Na+Na+
Mg2+Mg2+Mg2+
Al3+Al-organic complex, Al(OH)n3−nAl (OH)4−
Si4+Si(OH)4Si(OH)4
K+K+K+
Ca2+Ca2+Ca2+, CaHCO3+, Ca-organic complex
Cr3+CrOH2+Cr(OH)4−
Cr6+HCrO4−CrO42−
Mn2+Mn2+Mn2+, MnHCO3+
Fe2+Fe2+FeCO3, Fe2+, FeHCO3+
Fe3+FeOH2+, Fe(OH)3, Fe-organic complexFe(OH)3, Fe-organic complex
Ni2+Ni2+NiCO3, NiHCO3+, Ni2+
Cu2+Cu-organic complexCuCO3, Cu-organic complex
Zn2+Zn2+ZnHCO3+, Zn2+, Zn-organic complex
Mo6+HMoO4−HMoO4−, MoO42−
Cd2+Cd2+, CdCl+Cd2+, CdCl+, CdHCO3+
Pb2+Pb2+, Pb-organic complexPbCO3, PbHCO3+, Pb-organic complex
Table
Table 3. Categories of salt-affected soils based on ECe (dS/m), SARe, and pH1:5 water of soil solutions and possible mechanisms of impact on plants. Toxicity, deficiency, or ion-imbalance due to various ions will depend on the ionic composition of soil solution [31]. SARe > 6 denotes sodic soils with dispersive behaviour in the Australian classification [32]. EC, electrical conductivity; SAR, sodium adsorption ratio.
Table 3. Categories of salt-affected soils based on ECe (dS/m), SARe, and pH1:5 water of soil solutions and possible mechanisms of impact on plants. Toxicity, deficiency, or ion-imbalance due to various ions will depend on the ionic composition of soil solution [31]. SARe > 6 denotes sodic soils with dispersive behaviour in the Australian classification [32]. EC, electrical conductivity; SAR, sodium adsorption ratio.
Category of Saline SoilCriteriaPossible Mechanisms
Acidic-saline soilECe > 4; SARe < 6; pH < 6Osmotic effect; microelement (Fe, Al, Mn) toxicity; Sulphate toxicity at low pH
Neutral saline soilECe > 4; SARe < 6; pH 6–8Osmotic effect; toxicity of dominant anion or cation other than Na+
Alkaline-saline soilECe > 4; SARe < 6; pH 8–9Osmotic effect; HCO3− and CO32− toxicity
Highly alkaline-saline soilECe > 4; SARe < 6; pH > 9Osmotic effect; HCO3− and CO32− toxicity; toxicity of microelements (Fe, Al, Mn)
Acidic saline-sodic soilECe > 4; SARe > 6; pH < 6Osmotic effect; microelement (Fe, Al, Mn) toxicity; Na+ toxicity
Neutral saline-sodic soilECe > 4; SARe > 6; pH 6–8Osmotic effect; Na+ toxicity; toxicity of dominant anion (Cl− or SO42−)
Alkaline-saline sodic soilECe > 4; SARe > 6; pH 8–9Osmotic effect; Na+ toxicity; HCO3− and CO32− toxicity
Highly alkaline saline-sodic soilECe > 4; SARe > 6; pH > 9Osmotic effect; Na+ toxicity; HCO3− and CO32− toxicity; microelement (Fe, Al, Mn) toxicity;
Acidic-sodic soilECe < 4; SARe > 6; pH < 6Indirect effect due to soil structural problems; seasonal waterlogging can induce microelement (Fe, Al, Mn) toxicity;
Neutral sodic soilECe < 4; SARe > 6; pH 6–8Indirect effect due to soil structural problems; seasonal waterlogging; Na+ toxicity at high SARe
Alkaline-sodic soilECe < 4; SARe > 6; pH 8–9Indirect effect due to soil structural problems; seasonal waterlogging; Na+ toxicity at high SARe; possible HCO3− and CO32− toxicity
Highly alkaline-sodic soilECe < 4; SARe > 6; pH >9Indirect effect due to soil structural problems; seasonal waterlogging; Na+ toxicity at high SARe; HCO3− and CO32− toxicity; microelement (Fe, Al, Mn) toxicity
Table
Table 4. Free electron activity (pE) at pH 7 for some equilibrium chemical reactions under anoxic and suboxic conditions in dispersive soils [36].
Table 4. Free electron activity (pE) at pH 7 for some equilibrium chemical reactions under anoxic and suboxic conditions in dispersive soils [36].
Chemical ReactionspE
O2 + 4H+ + 4 e− ↔ 2 H2O13.80
2 NO3− +12 H+ + 10 e− ↔ N2 + 6 H2O12.66
MnO2 + 4H+ + 2 e− ↔ Mn2+ + 2 H2O6.80
Fe (OH)3 + 3H+ + e− ↔ Fe2+ + 3 H2O−3.13
SO42− + 10 H+ + 8e− ↔ H2S + 4 H2O−3.63
CO2 + 8H+ + 8e− ↔ CH4 + 2 H2O−4.14
N2 + 8H+ + 6e− ↔ 2 NH4+−4.69
2H+ + 2e− ↔ H2−7.00

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Rengasamy, P. Soil Chemistry Factors Confounding Crop Salinity Tolerance—A Review. Agronomy 2016, 6, 53. https://0-doi-org.brum.beds.ac.uk/10.3390/agronomy6040053

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Rengasamy P. Soil Chemistry Factors Confounding Crop Salinity Tolerance—A Review. Agronomy. 2016; 6(4):53. https://0-doi-org.brum.beds.ac.uk/10.3390/agronomy6040053

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Rengasamy, Pichu. 2016. "Soil Chemistry Factors Confounding Crop Salinity Tolerance—A Review" Agronomy 6, no. 4: 53. https://0-doi-org.brum.beds.ac.uk/10.3390/agronomy6040053

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