Study of the effect of temperature, pH, and time on the desorption of H2S.

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DIEGO MARTINEZ CARRILLO, CARLOS ALBERTO ÁVILA-ORTA, JOSÉ CAÍN HERNANDEZ RODRÍGUEZ, and 2 more This is a preprint; it has not been peer reviewed by a journal. https://doi.org/ 10.21203/rs.3.rs-3870658/v1 This work is licensed under a CC BY 4.0 License Status: Posted Version 1 posted You are reading this latest preprint version Abstract Water is an inexhaustible natural resource, however, for use in human activities, it is required that its present certain characteristics that make it seem scarce. Hydrogen sulphide is a contaminant that occurs in well water making the water unusable for any human activity. Technology-marginalized areas that have this type of problem are affected by not having tools or equipment that can remove hydrogen sulphide from water. This study focuses on presenting an experimental design to determine the H 2 S removal kinetics under standard pressure conditions at different temperatures (23°C, 40°C and 50°C), observing that at 50°C up to 40% of the water evaporated. In addition, the effect of temperature (23°C and 40°C) and pH (7 and 11) on the removal of hydrogen sulphide was observed. An ANOVA was performed with the results obtained, determining that the significant variable in these tests was pH. Environmental Engineering Applied Statistics Environmental Chemistry aeration pH sulphide temperature well water Figures Figure 1 Figure 2 Figure 3 Figure 4 Figure 5 Figure 6 Introduction Water is a vital resource for the existence of living beings and for the development of civilization. In the last 50 years, groundwater extraction has quadrupled, and it is estimated that it supplies 36% of drinking water, 42% of water for agriculture, and 24% of water for industrial use (FAO, 2016 ). Worldwide, a problem affecting groundwater quality is the presence of hydrogen sulphide, whether of natural or anthropogenic origin (Plummer et al, 1990 ; Mukhopadhyay et al, 2006 ; Bhuiyan et al, 2010 ). Hydrogen sulphide water contamination can occur in both urban and rural areas, with rural areas being the most affected by the lack of infrastructure to treat and condition water for use (Satapathy et al, 2017 ). Dissolved H2S, involving a variety of chemical, biological, and biochemical processes in natural water, is an important indicator of natural water quality, and its concentration level varies over time (Yimei et al, 2023 ), occurs in different concentrations (0.1 to 244 mg/l) where 150 mg/L in groundwater can be considered low, medium-low, medium-high and high, respectively (Mukhopadhyay et al, 2006 ; O’Sullivan et al, 2005 ). In nature, water could be contaminated by geochemical processes by geothermal and sulphide minerals dissolves (Bondu et al, 2017 ; Akai et al, 2004 ). In other cases, sulphate ion is subject to reduction processes, especially in the presence of bacteria and organic matter. In reducing environments, at a pH below 7, the stable reduced form is H2S, while in alkaline solutions, the HS- ion predominates. Most sulphurous groundwater contains appreciable amounts of HS- or H 2 S, which even in very low concentrations give the water the typical smell of rotten eggs (EPA, 1985 ). H2S is formed from sulphate reduction, dissolves in water, and dissociates in accordance with reversible ionization reactions (EPA, 1985 ; Reiffenstein et al, 1992 ; Petrov and Srinivasan, 1996 ): $${H}_{2}S\leftrightarrow H{S}^{-}+{H}^{+}$$ 1 $$H{S}^{-}\leftrightarrow {S}^{2-}+{H}^{+}$$ 2 The effect of pH on the rate at which H2S can be released from solution into air under any condition is proportional to the H2S concentration. At pH 7, H2S will escape about half as fast as it does in a strongly acidic solution with the same dissolved sulphur content. At a pH of 9, it will escape only 1% as fast as it would from an acid solution. If some of the H 2 S escapes, the remaining dissolved sulphide will split between HS and H 2 S at the same initial ratio because equilibrium is restored almost instantly. (EPA, 1974 ). It should be noted that decreasing the pH decreases the amount of H 2 S in water if there is a means of removal, such as aeration (Powell and Lossberg, 1948 ). It is known that at pH less than 7, the percentage availability of H 2 S removal in water is greater (Fig. 1), varying exponentially and in greater proportion than in the range greater than 7 (Foxworthy and Gray, 1958 ). Similarly, the effect of temperature on the solubility of H 2 S in water is inversely proportional under standard pressure conditions (Fig. 2). As the temperature increases, the concentration of H 2 S in the water is exponentially lower (EPA, 1985 ). Yang and Allen ( 1994 ) observed that some samples with different waste compost had no significant differences in operating characteristics of their investigation, and the best temperature on H 2 S removal efficiency was between 30°C and 40°C. The aeration method has been one of the most widely used to remove hydrogen sulphide from well water. It can be done naturally by making it pass through unevenness, causing waterfalls or forced aeration through counter current devices. Pressure relief and exposure of high sulphide well water to the atmosphere is sufficient to remove a portion of the sulphur compounds, while oxygen uptake results in additional oxidative waste gas removal. Much of the total sulphides are transformed into free sulphur, and depending on the sulphide concentration, the amount of precipitated sulphur will be. The advantage of this technique is that it does not require complex installations or the consumption of reagents. However, this technique must be accompanied by filtration to remove the precipitates formed (Powell and Lossberg, 1948 ; Swistock, 2022 ). Another widely used method of removing hydrogen sulphide is chlorination. Chlorine is used as an oxidant to convert hydrogen sulphide to insoluble sulphur, which is later removed by filtration. For this method, containers or containers with agitation are used to mix the chlorine with the water to be treated, the high demand for chlorine makes this method economically impractical. The combination of aeration and chlorination methods is very common, giving good results, however, sometimes it requires expensive infrastructure, which makes its use impractical in rural areas. Hydrogen sulphide (H 2 S) is a by-product of many industrial processes and is ubiquitously present in municipal wastewater. Removal of hydrogen sulphide is of major concern in wastewater treatment and collection systems since it causes a wide range of problems, including toxicity, malodours, and corrosion (Zhang et al,2088). Sulphide concentrations of 0.5, 3.0, and 10.0 g/m 3 in the wastewater may be considered low, moderate, and high, respectively, in terms of problems that are typically reported (Hvitved-Jacobsen, 2002 ). The most common methods of hydrogen sulphide removal formed in waste streams are precipitation with metal salts (Veeken et al, 2003 ; Altaş, 2008 ; Karbanee et al, 2008 ) and oxidation using hydrogen peroxide, potassium permanganate and chlorine in alkaline solutions (Tomar and Abdullah, 1994 ) or activated carbon (Sergienko et al, 2019 ; Zulkefli et al, 2023 ). The main drawbacks of these processes are their high operating costs due to the usage of chemicals and the formation of toxic metal-containing sludge. Although biological oxidation of hydrogen sulphide is more sustainable, it is a slow process that requires pre-treatment of waste streams (Pikaar et al, 2015 ). Electrochemical processes are an alternative to the existing technologies for sulphide removal, as they offer a robust removal of hydrogen sulphide in-situ and avoid the costs and risks related to dosing, transportation, and storage of chemicals (Sergienko et al, 2019 ). This study aims to present an analysis of the relationship between the parameters of time, temperature, and pH in the removal of hydrogen sulphide using a factorial design and an ANOVA analysis. In order to explore low-cost and easy-to-use alternatives that can be implemented in rural areas where they do not have supplies of reagents, technicians, or electricity. Methodology Hydrogen sulphide desorption experiments were conducted using a (0.5 L) batch reactor. Sulphide was dosed by introducing a sulphide standard solution to a final concentration of sulphide, approximately 50 mg/L. Sulphide standard solutions were prepared regularly by dissolving appropriate amounts of disodium sulphide. Higher concentrations of sulphide as a standard solution were voided because on the work site such highly concentrated sulphide solutions would imply high health and safety hazards. To determine the concentration of hydrogen sulphide, the volumetric analysis technique by iodometry was used (Powell and Lossberg, 1948 ; APHA, 2018), with the following variant: 20 ml of the test solution were taken at a certain time, immediately then they were measured with deionized distilled water to 200 ml, to which the analysis was carried out, later the concentration of the problem solution was calculated. A factorial design was carried out to determine the evolution of H 2 S desorption as a function of time at different temperatures and pH conditions. The concentration of H 2 S in the solution reported as a percentage was defined as the relationship between the initial concentration of H 2 S and the concentration of H 2 S present at the time of its analysis. Results and discussion The results obtained from the different tests carried out are presented below and are grouped by parameters for better discussion. Effect of time on H2S removal. A test was carried out to see the kinetics of desorption of H 2 S from water under ambient conditions of pH, pressure, and temperature. Once the standard solution was prepared, the initial H 2 S concentration was measured, and programmed monitoring was carried out to observe the decrease in the H 2 S concentration for 14 days (Fig. 3). The results indicate that under ambient conditions, the H 2 S concentration gradually decreases as time passes. However, a harmonic trend is not observed since when the H 2 S is released from the solution, there is also water evaporation, and depending on the environmental conditions, the kinetics of H 2 S desorption and water evaporation are variable. Effect of time and temperature on H2S removal. Tests for the effect of temperature were performed simultaneously at 23°C, 40°C and 50°C, under ambient pressure conditions, at a pH of 10.5 with a standard deviation of ± 0.25. The results obtained show a clear trend in the release of H 2 S as a function of time (Fig. 4). The temperature condition that reached a higher percentage of desorption was 40°C, however, the higher the temperature, the greater the evaporation of water. It can be assumed that when the water evaporates, the variation rate of the remaining H 2 S concentration in the solution can become zero or positive. An exercise was carried out to observe the evaporation kinetics of water at environmental pressure conditions (Fig. 5), it was observed that its behaviour was linear, and in 12 hours, there can be a loss of water of up to 40% and 21% of its initial volume, at a constant temperature of 50°C and 40°C respectively. Effect of time and pH on H2S removal. During the tests, an average pH of 10.5 (± 0.25) and an average pH of 7 (± 0.16) were maintained. The effect of pH on sulphide desorption presents a similar behaviour under the test conditions (Fig. 6). However, a higher desorption is achieved at 40°C than at 23°C at both pH. It is also observed that at a pH of 7, a greater desorption is obtained in both cases. One of the probable reasons is that by lowering the pH with 1N HCL, the excess of hydrogen protons favours the formation of hydrogen sulphide (Eq. 1 ). Effect of time and pH on H2S removal. An ANOVA was performed with time (t), temperature (T), and pH as variables. The results indicate that the three variables influence the desorption of H 2 S, however, the pH is the most significant variable in the tests carried out (Table 1). It can be considered that the effect of pH in combination with the desorption time of H 2 S from the solution is also significant, even more than the effect of temperature itself. Temperature apparently has a minor effect on the desorption of H 2 S. However, it is recognized that temperature is a promoter in the kinetic activity of the molecules, causing the desorption kinetics to be greater. However, the relationship between H 2 O evaporation and H 2 S desorption causes the rate of change in H 2 S/H 2 O concentration to be minimal, null, or even negative in some cases. Results and discussion The study carried out shows that the desorption of H 2 S at ambient conditions is stable after 6 days. Desorption kinetics can be higher if the temperature and pH of the solution are changed. The solution temperature at 40°C presents the best desorption kinetics and is even better at a pH of 7. Higher temperatures cause greater evaporation of water, which leads to an increase in the H 2 S/H 2 O ratio. On the other hand, the solution naturally becomes basic when the chemical reaction proposed in Eq. ( 1 ) is carried out, reaching an equilibrium point where the concentration of S 2- remains constant. On the other hand, decreasing the pH favours the generation of H 2 S, which is reflected in reaching a lower concentration of S 2- in solution in less time. Finally, the ANOVA shows that, indeed, the pH adjustment is the most significant variable in the tests carried out. Declarations Authors contributions Conceptualization, DMC and CAAO; Methodology, DMC; Validation, DMC, CAAO, JCHR and CGB; Formal Analysis, DMC, JCHR and CGB.; Investigation, DMC and JCHR; Data Curation, DMC, LFCO and CGB; Writing—Original Draft Preparation, DMC; Writing—Review & Editing, DMC, CAAO, JCHR and CGB; Visualization, DMC.; Supervision, CAAO; Project Administration, DMC. Acknowledgements This research had been funded by the Consejo Nacional de Humanidades, Ciencia y Tecnología (CONAHCYT), the Universidad Autónoma de Coahuila (UAdeC), and the Centro de Investigación en Química Aplicada (CIQA). We would like to thank Centro de Investigación en Geociencias Aplicadas (CIGA) and Tecnológico Nacional de México/ITES de la Región Carbonífera for the laboratory work support. References Akai, J., Izumi, K., Fukuhara, H., Masuda, H., Nakano, S., Yoshimura, T., … Akai, K., 2004. Mineralogical and geomicrobiological investigations on groundwater arsenic enrichment in Bangladesh. 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Water Res., 42, 1–12. https://doi.org/10.1016/j.watres.2007.07.013 . Zulkefli, N., Noor Azam, A.M.I., Masdar, M.S., Isahak, W.N.R.W., 2023. Adsorption–Desorption Behavior of Hydrogen Sulfide Capture on a Modified Activated Carbon Surface. Materials, 16, 462. https://doi.org/10.3390/ma16010462 Tables Table 1 is available in the Supplementary Files section. Additional Declarations The authors declare no competing interests. Supplementary Files Table1.png Table 1. Analysis of variance of H 2 S desorption as a function of time, temperature, and pH. Cite Share Download PDF Status: Posted Version 1 posted You are reading this latest preprint version Research Square lets you share your work early, gain feedback from the community, and start making changes to your manuscript prior to peer review in a journal. As a division of Research Square Company, we’re committed to making research communication faster, fairer, and more useful. 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Also discoverable on Platform About Our Team In Review Editorial Policies Advisory Board Help Center Resources Author Services Accessibility API Access RSS feed Manage Cookie Preferences © Research Square 2026 | ISSN 2693-5015 (online) Privacy Policy Terms of Service Do Not Sell My Personal Information {"props":{"pageProps":{"initialData":{"identity":"rs-3870658","acceptedTermsAndConditions":true,"allowDirectSubmit":true,"archivedVersions":[],"articleType":"Research Article","associatedPublications":[],"authors":[{"id":267489502,"identity":"768ff970-1180-4065-9fa1-6f4befd01fee","order_by":0,"name":"DIEGO MARTINEZ CARRILLO","email":"","orcid":"https://orcid.org/0000-0002-6695-9746","institution":"CENTRO DE INVESTIGACIÓN EN GEOCIENCIAS APLICADAS, UAdeC","correspondingAuthor":false,"prefix":"","firstName":"DIEGO","middleName":"MARTINEZ","lastName":"CARRILLO","suffix":""},{"id":267491405,"identity":"419592ff-8cd1-43a3-a4c4-c39061111af7","order_by":1,"name":"CARLOS ALBERTO 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H\u003csub\u003e2\u003c/sub\u003eS desorption at room condition.\u003c/p\u003e","description":"","filename":"fig3.png","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/8fa898afd9795d2a57e96dac.png"},{"id":49821598,"identity":"a430dec5-2cc2-4e7a-a7a6-ae4ef4d60e3f","added_by":"auto","created_at":"2024-01-18 15:09:11","extension":"png","order_by":4,"title":"Figure 4","display":"","copyAsset":false,"role":"figure","size":11737,"visible":true,"origin":"","legend":"\u003cp\u003eThe kinetic curve of H\u003csub\u003e2\u003c/sub\u003eS desorption at different temperatures (23°C, 40°C, and 50°C).\u003c/p\u003e","description":"","filename":"fig4.png","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/ff3cb414990740cbf05a5ab1.png"},{"id":49821238,"identity":"90c333d9-0ab8-4506-9c68-b22a79ed075d","added_by":"auto","created_at":"2024-01-18 15:01:11","extension":"png","order_by":5,"title":"Figure 5","display":"","copyAsset":false,"role":"figure","size":15710,"visible":true,"origin":"","legend":"\u003cp\u003eKinetic line of water evaporation percentage at room condition.\u003c/p\u003e","description":"","filename":"fig5.png","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/5240fd195e51af63ce2fd9e9.png"},{"id":49821239,"identity":"0db67874-c985-4494-82e3-7f6a7889c4ee","added_by":"auto","created_at":"2024-01-18 15:01:11","extension":"png","order_by":6,"title":"Figure 6","display":"","copyAsset":false,"role":"figure","size":38302,"visible":true,"origin":"","legend":"\u003cp\u003eKinetic line of S\u003csup\u003e2-\u003c/sup\u003e desorption percentage at different pH and a) 23 °C of temperature and b) 40 °C of temperature.\u003c/p\u003e","description":"","filename":"fig6.png","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/c5b05ac188fbb7fb1b763749.png"},{"id":49822605,"identity":"46c7b6a1-90d0-46f8-ad43-42ff99122539","added_by":"auto","created_at":"2024-01-18 15:25:12","extension":"pdf","order_by":0,"title":"","display":"","copyAsset":false,"role":"manuscript-pdf","size":384212,"visible":true,"origin":"","legend":"","description":"","filename":"manuscript.pdf","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/f72cf333-f613-4c29-90af-3d5cf560e93d.pdf"},{"id":49822143,"identity":"e0a2d1ee-b1f9-47e9-b7a7-699b31bcef04","added_by":"auto","created_at":"2024-01-18 15:17:11","extension":"png","order_by":1,"title":"","display":"","copyAsset":false,"role":"supplement","size":17645,"visible":true,"origin":"","legend":"\u003cp\u003eTable 1. Analysis of variance of H\u003csub\u003e2\u003c/sub\u003eS desorption as a function of time, temperature, and pH.\u003c/p\u003e","description":"","filename":"Table1.png","url":"https://assets-eu.researchsquare.com/files/rs-3870658/v1/91c0357c83bbac66777ecb05.png"}],"financialInterests":"The authors declare no competing interests.","formattedTitle":"\u003cp\u003eStudy of the effect of temperature, pH, and time on the desorption of H\u003csub\u003e2\u003c/sub\u003eS.\u003c/p\u003e","fulltext":[{"header":"Introduction","content":"\u003cp\u003eWater is a vital resource for the existence of living beings and for the development of civilization. In the last 50 years, groundwater extraction has quadrupled, and it is estimated that it supplies 36% of drinking water, 42% of water for agriculture, and 24% of water for industrial use (FAO, \u003cspan citationid=\"CR8\" class=\"CitationRef\"\u003e2016\u003c/span\u003e). Worldwide, a problem affecting groundwater quality is the presence of hydrogen sulphide, whether of natural or anthropogenic origin (Plummer et al, \u003cspan citationid=\"CR16\" class=\"CitationRef\"\u003e1990\u003c/span\u003e; Mukhopadhyay et al, \u003cspan citationid=\"CR12\" class=\"CitationRef\"\u003e2006\u003c/span\u003e; Bhuiyan et al, \u003cspan citationid=\"CR4\" class=\"CitationRef\"\u003e2010\u003c/span\u003e). Hydrogen sulphide water contamination can occur in both urban and rural areas, with rural areas being the most affected by the lack of infrastructure to treat and condition water for use (Satapathy et al, \u003cspan citationid=\"CR19\" class=\"CitationRef\"\u003e2017\u003c/span\u003e).\u003c/p\u003e \u003cp\u003eDissolved H2S, involving a variety of chemical, biological, and biochemical processes in natural water, is an important indicator of natural water quality, and its concentration level varies over time (Yimei et al, \u003cspan citationid=\"CR25\" class=\"CitationRef\"\u003e2023\u003c/span\u003e), occurs in different concentrations (0.1 to 244 mg/l) where \u0026lt; 20, 20 to 50, 50 to 150 and \u0026gt; 150 mg/L in groundwater can be considered low, medium-low, medium-high and high, respectively (Mukhopadhyay et al, \u003cspan citationid=\"CR12\" class=\"CitationRef\"\u003e2006\u003c/span\u003e; O’Sullivan et al, \u003cspan citationid=\"CR13\" class=\"CitationRef\"\u003e2005\u003c/span\u003e). In nature, water could be contaminated by geochemical processes by geothermal and sulphide minerals dissolves (Bondu et al, \u003cspan citationid=\"CR5\" class=\"CitationRef\"\u003e2017\u003c/span\u003e; Akai et al, \u003cspan citationid=\"CR1\" class=\"CitationRef\"\u003e2004\u003c/span\u003e). In other cases, sulphate ion is subject to reduction processes, especially in the presence of bacteria and organic matter. In reducing environments, at a pH below 7, the stable reduced form is H2S, while in alkaline solutions, the HS- ion predominates. Most sulphurous groundwater contains appreciable amounts of HS- or H\u003csub\u003e2\u003c/sub\u003eS, which even in very low concentrations give the water the typical smell of rotten eggs (EPA, \u003cspan citationid=\"CR7\" class=\"CitationRef\"\u003e1985\u003c/span\u003e). H2S is formed from sulphate reduction, dissolves in water, and dissociates in accordance with reversible ionization reactions (EPA, \u003cspan citationid=\"CR7\" class=\"CitationRef\"\u003e1985\u003c/span\u003e; Reiffenstein et al, \u003cspan citationid=\"CR18\" class=\"CitationRef\"\u003e1992\u003c/span\u003e; Petrov and Srinivasan, \u003cspan citationid=\"CR14\" class=\"CitationRef\"\u003e1996\u003c/span\u003e):\u003c/p\u003e\u003cdiv id=\"Equ1\" class=\"Equation\"\u003e\u003cdiv format=\"TEX\" class=\"mathdisplay\" id=\"FileID_Equ1\" name=\"EquationSource\"\u003e\n$${H}_{2}S\\leftrightarrow H{S}^{-}+{H}^{+}$$\u003c/div\u003e\u003cdiv class=\"EquationNumber\"\u003e1\u003c/div\u003e\u003c/div\u003e\u003cdiv id=\"Equ2\" class=\"Equation\"\u003e\u003cdiv format=\"TEX\" class=\"mathdisplay\" id=\"FileID_Equ2\" name=\"EquationSource\"\u003e\n$$H{S}^{-}\\leftrightarrow {S}^{2-}+{H}^{+}$$\u003c/div\u003e\u003cdiv class=\"EquationNumber\"\u003e2\u003c/div\u003e\u003c/div\u003e\u003cp\u003e\u003c/p\u003e \u003cp\u003eThe effect of pH on the rate at which H2S can be released from solution into air under any condition is proportional to the H2S concentration. At pH 7, H2S will escape about half as fast as it does in a strongly acidic solution with the same dissolved sulphur content. At a pH of 9, it will escape only 1% as fast as it would from an acid solution. If some of the H\u003csub\u003e2\u003c/sub\u003eS escapes, the remaining dissolved sulphide will split between HS and H\u003csub\u003e2\u003c/sub\u003eS at the same initial ratio because equilibrium is restored almost instantly. (EPA, \u003cspan citationid=\"CR6\" class=\"CitationRef\"\u003e1974\u003c/span\u003e). It should be noted that decreasing the pH decreases the amount of H\u003csub\u003e2\u003c/sub\u003eS in water if there is a means of removal, such as aeration (Powell and Lossberg, \u003cspan citationid=\"CR17\" class=\"CitationRef\"\u003e1948\u003c/span\u003e). It is known that at pH less than 7, the percentage availability of H\u003csub\u003e2\u003c/sub\u003eS removal in water is greater (Fig.\u0026nbsp;1), varying exponentially and in greater proportion than in the range greater than 7 (Foxworthy and Gray, \u003cspan citationid=\"CR9\" class=\"CitationRef\"\u003e1958\u003c/span\u003e).\u003c/p\u003e \u003cp\u003eSimilarly, the effect of temperature on the solubility of H\u003csub\u003e2\u003c/sub\u003eS in water is inversely proportional under standard pressure conditions (Fig.\u0026nbsp;2). As the temperature increases, the concentration of H\u003csub\u003e2\u003c/sub\u003eS in the water is exponentially lower (EPA, \u003cspan citationid=\"CR7\" class=\"CitationRef\"\u003e1985\u003c/span\u003e).\u003c/p\u003e \u003cp\u003eYang and Allen (\u003cspan citationid=\"CR24\" class=\"CitationRef\"\u003e1994\u003c/span\u003e) observed that some samples with different waste compost had no significant differences in operating characteristics of their investigation, and the best temperature on H\u003csub\u003e2\u003c/sub\u003eS removal efficiency was between 30°C and 40°C.\u003c/p\u003e \u003cp\u003eThe aeration method has been one of the most widely used to remove hydrogen sulphide from well water. It can be done naturally by making it pass through unevenness, causing waterfalls or forced aeration through counter current devices. Pressure relief and exposure of high sulphide well water to the atmosphere is sufficient to remove a portion of the sulphur compounds, while oxygen uptake results in additional oxidative waste gas removal. Much of the total sulphides are transformed into free sulphur, and depending on the sulphide concentration, the amount of precipitated sulphur will be. The advantage of this technique is that it does not require complex installations or the consumption of reagents. However, this technique must be accompanied by filtration to remove the precipitates formed (Powell and Lossberg, \u003cspan citationid=\"CR17\" class=\"CitationRef\"\u003e1948\u003c/span\u003e; Swistock, \u003cspan citationid=\"CR21\" class=\"CitationRef\"\u003e2022\u003c/span\u003e).\u003c/p\u003e \u003cp\u003eAnother widely used method of removing hydrogen sulphide is chlorination. Chlorine is used as an oxidant to convert hydrogen sulphide to insoluble sulphur, which is later removed by filtration. For this method, containers or containers with agitation are used to mix the chlorine with the water to be treated, the high demand for chlorine makes this method economically impractical. The combination of aeration and chlorination methods is very common, giving good results, however, sometimes it requires expensive infrastructure, which makes its use impractical in rural areas.\u003c/p\u003e \u003cp\u003eHydrogen sulphide (H\u003csub\u003e2\u003c/sub\u003eS) is a by-product of many industrial processes and is ubiquitously present in municipal wastewater. Removal of hydrogen sulphide is of major concern in wastewater treatment and collection systems since it causes a wide range of problems, including toxicity, malodours, and corrosion (Zhang et al,2088). Sulphide concentrations of 0.5, 3.0, and 10.0 g/m\u003csup\u003e3\u003c/sup\u003e in the wastewater may be considered low, moderate, and high, respectively, in terms of problems that are typically reported (Hvitved-Jacobsen, \u003cspan citationid=\"CR10\" class=\"CitationRef\"\u003e2002\u003c/span\u003e). The most common methods of hydrogen sulphide removal formed in waste streams are precipitation with metal salts (Veeken et al, \u003cspan citationid=\"CR23\" class=\"CitationRef\"\u003e2003\u003c/span\u003e; Altaş, \u003cspan citationid=\"CR2\" class=\"CitationRef\"\u003e2008\u003c/span\u003e; Karbanee et al, \u003cspan citationid=\"CR11\" class=\"CitationRef\"\u003e2008\u003c/span\u003e) and oxidation using hydrogen peroxide, potassium permanganate and chlorine in alkaline solutions (Tomar and Abdullah, \u003cspan citationid=\"CR22\" class=\"CitationRef\"\u003e1994\u003c/span\u003e) or activated carbon (Sergienko et al, \u003cspan citationid=\"CR20\" class=\"CitationRef\"\u003e2019\u003c/span\u003e; Zulkefli et al, \u003cspan citationid=\"CR27\" class=\"CitationRef\"\u003e2023\u003c/span\u003e). The main drawbacks of these processes are their high operating costs due to the usage of chemicals and the formation of toxic metal-containing sludge. Although biological oxidation of hydrogen sulphide is more sustainable, it is a slow process that requires pre-treatment of waste streams (Pikaar et al, \u003cspan citationid=\"CR15\" class=\"CitationRef\"\u003e2015\u003c/span\u003e). Electrochemical processes are an alternative to the existing technologies for sulphide removal, as they offer a robust removal of hydrogen sulphide in-situ and avoid the costs and risks related to dosing, transportation, and storage of chemicals (Sergienko et al, \u003cspan citationid=\"CR20\" class=\"CitationRef\"\u003e2019\u003c/span\u003e).\u003c/p\u003e \u003cp\u003eThis study aims to present an analysis of the relationship between the parameters of time, temperature, and pH in the removal of hydrogen sulphide using a factorial design and an ANOVA analysis. In order to explore low-cost and easy-to-use alternatives that can be implemented in rural areas where they do not have supplies of reagents, technicians, or electricity.\u003c/p\u003e "},{"header":"Methodology","content":"\u003cp\u003eHydrogen sulphide desorption experiments were conducted using a (0.5 L) batch reactor. Sulphide was dosed by introducing a sulphide standard solution to a final concentration of sulphide, approximately 50 mg/L. Sulphide standard solutions were prepared regularly by dissolving appropriate amounts of disodium sulphide. Higher concentrations of sulphide as a standard solution were voided because on the work site such highly concentrated sulphide solutions would imply high health and safety hazards.\u003c/p\u003e\u003cp\u003eTo determine the concentration of hydrogen sulphide, the volumetric analysis technique by iodometry was used (Powell and Lossberg, \u003cspan citationid=\"CR17\" class=\"CitationRef\"\u003e1948\u003c/span\u003e; APHA, 2018), with the following variant: 20 ml of the test solution were taken at a certain time, immediately then they were measured with deionized distilled water to 200 ml, to which the analysis was carried out, later the concentration of the problem solution was calculated. A factorial design was carried out to determine the evolution of H\u003csub\u003e2\u003c/sub\u003eS desorption as a function of time at different temperatures and pH conditions. The concentration of H\u003csub\u003e2\u003c/sub\u003eS in the solution reported as a percentage was defined as the relationship between the initial concentration of H\u003csub\u003e2\u003c/sub\u003eS and the concentration of H\u003csub\u003e2\u003c/sub\u003eS present at the time of its analysis.\u003c/p\u003e"},{"header":"Results and discussion","content":"\u003cp\u003eThe results obtained from the different tests carried out are presented below and are grouped by parameters for better discussion.\u003c/p\u003e \u003cp\u003e \u003cb\u003eEffect of time on H2S removal.\u003c/b\u003e \u003c/p\u003e \u003cp\u003eA test was carried out to see the kinetics of desorption of H\u003csub\u003e2\u003c/sub\u003eS from water under ambient conditions of pH, pressure, and temperature. Once the standard solution was prepared, the initial H\u003csub\u003e2\u003c/sub\u003eS concentration was measured, and programmed monitoring was carried out to observe the decrease in the H\u003csub\u003e2\u003c/sub\u003eS concentration for 14 days (Fig.\u0026nbsp;3). The results indicate that under ambient conditions, the H\u003csub\u003e2\u003c/sub\u003eS concentration gradually decreases as time passes. However, a harmonic trend is not observed since when the H\u003csub\u003e2\u003c/sub\u003eS is released from the solution, there is also water evaporation, and depending on the environmental conditions, the kinetics of H\u003csub\u003e2\u003c/sub\u003eS desorption and water evaporation are variable.\u003c/p\u003e \u003cp\u003e \u003cb\u003eEffect of time and temperature on H2S removal.\u003c/b\u003e \u003c/p\u003e \u003cp\u003eTests for the effect of temperature were performed simultaneously at 23\u0026deg;C, 40\u0026deg;C and 50\u0026deg;C, under ambient pressure conditions, at a pH of 10.5 with a standard deviation of \u0026plusmn;\u0026thinsp;0.25. The results obtained show a clear trend in the release of H\u003csub\u003e2\u003c/sub\u003eS as a function of time (Fig.\u0026nbsp;4). The temperature condition that reached a higher percentage of desorption was 40\u0026deg;C, however, the higher the temperature, the greater the evaporation of water. It can be assumed that when the water evaporates, the variation rate of the remaining H\u003csub\u003e2\u003c/sub\u003eS concentration in the solution can become zero or positive.\u003c/p\u003e \u003cp\u003eAn exercise was carried out to observe the evaporation kinetics of water at environmental pressure conditions (Fig.\u0026nbsp;5), it was observed that its behaviour was linear, and in 12 hours, there can be a loss of water of up to 40% and 21% of its initial volume, at a constant temperature of 50\u0026deg;C and 40\u0026deg;C respectively.\u003c/p\u003e \u003cp\u003e \u003cb\u003eEffect of time and pH on H2S removal.\u003c/b\u003e \u003c/p\u003e \u003cp\u003eDuring the tests, an average pH of 10.5 (\u0026plusmn;\u0026thinsp;0.25) and an average pH of 7 (\u0026plusmn;\u0026thinsp;0.16) were maintained. The effect of pH on sulphide desorption presents a similar behaviour under the test conditions (Fig.\u0026nbsp;6). However, a higher desorption is achieved at 40\u0026deg;C than at 23\u0026deg;C at both pH. It is also observed that at a pH of 7, a greater desorption is obtained in both cases. One of the probable reasons is that by lowering the pH with 1N HCL, the excess of hydrogen protons favours the formation of hydrogen sulphide (Eq.\u0026nbsp;\u003cspan refid=\"Equ1\" class=\"InternalRef\"\u003e1\u003c/span\u003e).\u003c/p\u003e \u003cp\u003e \u003cb\u003eEffect of time and pH on H2S removal.\u003c/b\u003e \u003c/p\u003e \u003cp\u003eAn ANOVA was performed with time (t), temperature (T), and pH as variables. The results indicate that the three variables influence the desorption of H\u003csub\u003e2\u003c/sub\u003eS, however, the pH is the most significant variable in the tests carried out (Table\u0026nbsp;1).\u003c/p\u003e \u003cp\u003eIt can be considered that the effect of pH in combination with the desorption time of H\u003csub\u003e2\u003c/sub\u003eS from the solution is also significant, even more than the effect of temperature itself.\u003c/p\u003e \u003cp\u003eTemperature apparently has a minor effect on the desorption of H\u003csub\u003e2\u003c/sub\u003eS. However, it is recognized that temperature is a promoter in the kinetic activity of the molecules, causing the desorption kinetics to be greater. However, the relationship between H\u003csub\u003e2\u003c/sub\u003eO evaporation and H\u003csub\u003e2\u003c/sub\u003eS desorption causes the rate of change in H\u003csub\u003e2\u003c/sub\u003eS/H\u003csub\u003e2\u003c/sub\u003eO concentration to be minimal, null, or even negative in some cases.\u003c/p\u003e"},{"header":"Results and discussion","content":"\u003cp\u003eThe study carried out shows that the desorption of H\u003csub\u003e2\u003c/sub\u003eS at ambient conditions is stable after 6 days. Desorption kinetics can be higher if the temperature and pH of the solution are changed. The solution temperature at 40\u0026deg;C presents the best desorption kinetics and is even better at a pH of 7. Higher temperatures cause greater evaporation of water, which leads to an increase in the H\u003csub\u003e2\u003c/sub\u003eS/H\u003csub\u003e2\u003c/sub\u003eO ratio. On the other hand, the solution naturally becomes basic when the chemical reaction proposed in Eq.\u0026nbsp;(\u003cspan refid=\"Equ1\" class=\"InternalRef\"\u003e1\u003c/span\u003e) is carried out, reaching an equilibrium point where the concentration of S\u003csup\u003e2-\u003c/sup\u003e remains constant. On the other hand, decreasing the pH favours the generation of H\u003csub\u003e2\u003c/sub\u003eS, which is reflected in reaching a lower concentration of S\u003csup\u003e2-\u003c/sup\u003e in solution in less time. Finally, the ANOVA shows that, indeed, the pH adjustment is the most significant variable in the tests carried out.\u003c/p\u003e"},{"header":"Declarations","content":"\u003ch2\u003eAuthors contributions\u003c/h2\u003e \u003cp\u003eConceptualization, DMC and CAAO; Methodology, DMC; Validation, DMC, CAAO, JCHR and CGB; Formal Analysis, DMC, JCHR and CGB.; Investigation, DMC and JCHR; Data Curation, DMC, LFCO and CGB; Writing\u0026mdash;Original Draft Preparation, DMC; Writing\u0026mdash;Review \u0026amp; Editing, DMC, CAAO, JCHR and CGB; Visualization, DMC.; Supervision, CAAO; Project Administration, DMC.\u003c/p\u003e\u003ch2\u003eAcknowledgements\u003c/h2\u003e \u003cp\u003eThis research had been funded by the Consejo Nacional de Humanidades, Ciencia y Tecnolog\u0026iacute;a (CONAHCYT), the Universidad Aut\u0026oacute;noma de Coahuila (UAdeC), and the Centro de Investigaci\u0026oacute;n en Qu\u0026iacute;mica Aplicada (CIQA). We would like to thank Centro de Investigaci\u0026oacute;n en Geociencias Aplicadas (CIGA) and Tecnol\u0026oacute;gico Nacional de M\u0026eacute;xico/ITES de la Regi\u0026oacute;n Carbon\u0026iacute;fera for the laboratory work support.\u003c/p\u003e"},{"header":"References","content":"\u003col\u003e\u003cli\u003e\u003cspan\u003eAkai, J., Izumi, K., Fukuhara, H., Masuda, H., Nakano, S., Yoshimura, T., \u0026hellip; Akai, K., 2004. Mineralogical and geomicrobiological investigations on groundwater arsenic enrichment in Bangladesh. Applied Geochemistry, 19(2), 215\u0026ndash;230. \u003cspan class=\"ExternalRef\"\u003e\u003cspan class=\"RefSource\"\u003ehttps://doi.org/10.1016/j.apgeochem.2003.09.008\u003c/span\u003e\u003cspan address=\"10.1016/j.apgeochem.2003.09.008\" targettype=\"DOI\" class=\"RefTarget\"\u003e\u003c/span\u003e\u003c/span\u003e\u003c/span\u003e\u003c/li\u003e \u003cli\u003e\u003cspan\u003eAltaş, L., B\u0026uuml;y\u0026uuml;kg\u0026uuml;ng\u0026ouml;r, H., 2008. 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Materials, 16, 462. \u003cspan class=\"ExternalRef\"\u003e\u003cspan class=\"RefSource\"\u003ehttps://doi.org/10.3390/ma16010462\u003c/span\u003e\u003cspan address=\"10.3390/ma16010462\" targettype=\"DOI\" class=\"RefTarget\"\u003e\u003c/span\u003e\u003c/span\u003e\u003c/span\u003e\u003c/li\u003e\u003c/ol\u003e"},{"header":"Tables","content":"\u003cp\u003eTable 1 is available in the Supplementary Files section.\u003c/p\u003e"}],"fulltextSource":"","fullText":"","funders":[],"hasAdminPriorityOnWorkflow":false,"hasManuscriptDocX":true,"hasOptedInToPreprint":true,"hasPassedJournalQc":"","hasAnyPriority":true,"hideJournal":true,"highlight":"","institution":"CONSEJO NACIONAL DE HUMANIDADES, CIENCIAS Y TECNOLOGIAS","isAcceptedByJournal":false,"isAuthorSuppliedPdf":false,"isDeskRejected":"","isHiddenFromSearch":false,"isInQc":false,"isInWorkflow":false,"isPdf":false,"isPdfUpToDate":true,"isWithdrawnOrRetracted":false,"journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true},"keywords":"aeration, pH, sulphide, temperature, well water","lastPublishedDoi":"10.21203/rs.3.rs-3870658/v1","lastPublishedDoiUrl":"https://doi.org/10.21203/rs.3.rs-3870658/v1","license":{"name":"CC BY 4.0","url":"https://creativecommons.org/licenses/by/4.0/"},"manuscriptAbstract":"\u003cp\u003eWater is an inexhaustible natural resource, however, for use in human activities, it is required that its present certain characteristics that make it seem scarce. Hydrogen sulphide is a contaminant that occurs in well water making the water unusable for any human activity. Technology-marginalized areas that have this type of problem are affected by not having tools or equipment that can remove hydrogen sulphide from water. This study focuses on presenting an experimental design to determine the H\u003csub\u003e2\u003c/sub\u003eS removal kinetics under standard pressure conditions at different temperatures (23\u0026deg;C, 40\u0026deg;C and 50\u0026deg;C), observing that at 50\u0026deg;C up to 40% of the water evaporated. In addition, the effect of temperature (23\u0026deg;C and 40\u0026deg;C) and pH (7 and 11) on the removal of hydrogen sulphide was observed. An ANOVA was performed with the results obtained, determining that the significant variable in these tests was pH.\u003c/p\u003e","manuscriptTitle":"Study of the effect of temperature, pH, and time on the desorption of H2S.","msid":"","msnumber":"","nonDraftVersions":[{"code":1,"date":"2024-01-18 15:01:07","doi":"10.21203/rs.3.rs-3870658/v1","editorialEvents":[{"type":"communityComments","content":0}],"status":"published","journal":{"display":true,"email":"[email protected]","identity":"researchsquare","isNatureJournal":false,"hasQc":true,"allowDirectSubmit":true,"externalIdentity":"","sideBox":"","snPcode":"","submissionUrl":"/submission","title":"Research Square","twitterHandle":"researchsquare","acdcEnabled":true,"dfaEnabled":false,"editorialSystem":"","reportingPortfolio":"","inReviewEnabled":false,"inReviewRevisionsEnabled":true}}],"origin":"","ownerIdentity":"48ba7e3c-e13c-483a-9a52-29634cff8ee7","owner":[],"postedDate":"January 18th, 2024","published":true,"recentEditorialEvents":[],"rejectedJournal":[],"revision":"","amendment":"","status":"posted","subjectAreas":[{"id":28182935,"name":"Environmental Engineering"},{"id":28182936,"name":"Applied Statistics"},{"id":28182937,"name":"Environmental Chemistry"}],"tags":[],"updatedAt":"2024-01-18T15:01:07+00:00","versionOfRecord":[],"versionCreatedAt":"2024-01-18 15:01:07","video":"","vorDoi":"","vorDoiUrl":"","workflowStages":[]},"version":"v1","identity":"rs-3870658","journalConfig":"researchsquare"},"__N_SSP":true},"page":"/article/[identity]/[[...version]]","query":{"redirect":"/article/rs-3870658","identity":"rs-3870658","version":["v1"]},"buildId":"qtupq5eGEP_6zYnWcrvyt","isFallback":false,"isExperimentalCompile":false,"dynamicIds":[84888],"gssp":true,"scriptLoader":[]}