calcium carbonate and nitric acid experiment

Rate of Reaction - Calcium Carbonate & Hydrochloric Acid ( OCR A Level Chemistry )

Revision note.

PAG 9.2: Rate of Reaction - Calcium Carbonate & Hydrochloric Acid

The reaction of calcium carbonate and hydrochloric acid.

• Large chips
• Small chips
• The reaction itself cannot change

CaCO 3 (s) + 2HCl (aq) → CaCl 2 (aq) + H 2 O (l) + CO 2 (g)

• However, the application and analysis of the results shifts more towards the mathematical skills of accurately plotting graphs, drawing tangents and calculating gradients
• The volume of carbon dioxide gas produced
• The mass loss from the reaction vessel

Method 1 - Volume of CO 2 produced

• Support a gas syringe with a stand, boss and clamp.
• Add 50 cm 3   of dilute hydrochloric acid to a conical flask
• Loosely connect the gas syringe 
• Measure 0.40 g of calcium carbonate
• Add the 0.40 g of calcium carbonate into the conical flask, replace the gas syringe and start the stopwatch
• Record the volume of gas produced every 10 seconds. Continue timing until no more carbon dioxide appears to be given off
• This method still records the volume of carbon dioxide produced

Specimen results 1 - Volume of CO 2 produced

• Here is a set of typical results for this experiment

Rate of carbon dioxide production in the reaction of calcium carbonate and hydrochloric acid table

Graphing the results 1 - Volume of CO 2 produced

Analysis 1 - Volume of CO 2 produced

• The curve of best fit is drawn on the graph
• A tangent can then drawn starting from (0,0) to find the   initial rate   of reaction
• This is the rate of reaction

Method 2 - Mass of the reaction vessel

• Measure 0.40 g of calcium carbonate into a weighing boat
• Add 50 cm 3  of dilute hydrochloric acid to a conical flask
• Place the conical flask of hydrochloric acid AND the weighing boat of calcium carbonate onto the balance
• Measure the combined mass and record this as the  t = 0 result
• Add the 0.40 g of calcium carbonate into the conical flask, replace the weighing boat onto the balance and start the stopwatch
• Record the mass every 10 seconds. Continue timing until no further mass is lost
• It may be necessary to use more dilute concentrations of hydrochloric acid because it may not be realistically possible to record the mass every second
• A data logger could be connected to the balance (if available) and this can track the mass over time 

Specimen results 2 - Mass of the reaction vessel

Rate of change in mass in the reaction of calcium carbonate and hydrochloric acid table

Graphing the results 2 - Mass of the reaction vessel

Analysis 2 - Mass of the reaction vessel

• This then records the mass lost and can be used to give a graph with a curve more like the volume of CO 2 produced graph

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Author: Richard

Richard has taught Chemistry for over 15 years as well as working as a science tutor, examiner, content creator and author. He wasn’t the greatest at exams and only discovered how to revise in his final year at university. That knowledge made him want to help students learn how to revise, challenge them to think about what they actually know and hopefully succeed; so here he is, happily, at SME.

3:15 practical: investigate the effect of changing the surface area of marble chips and of changing the concentration of hydrochloric acid on the rate of reaction between marble chips and dilute hydrochloric acid

The rate of a chemical reaction can be measured either by how quickly reactants are used up or how quickly the products are formed.

The rate of reaction can be calculated using the following equation:

The units for rate of reaction will usually be grams per min (g/min)

An investigation of the reaction between marble chips and hydrochloric acid:

Using the apparatus shown the change in mass of carbon dioxide can be measure with time.

As the marble chips react with the acid, carbon dioxide is given off.

The purpose of the cotton wool is to allow carbon dioxide to escape, but to stop any acid from spraying out.

The mass of carbon dioxide lost is measured at intervals, and a graph is plotted:

Experiment to investigate the effects of changes in surface area of solid on the rate of a reaction:

The experiment is repeated using the exact same quantities of everything but using larger chips. For a given quantity, if the chips are larger then the surface area is lesson. So reaction with the larger chips happens more slowly.

Both sets of results are plotted on the same graph.

Experiment to investigate the effects of changes in concentration of solutions on the rate of a reaction:

The experiment is again repeated using the exact same quantities of everything but this time with half the concentration of acid. The marble chips must however be in excess. The reaction with the half the concentration of acid happens slower and produces half the amount of carbon dioxide.

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• 2.10 describe the qualitative effect of changing resistance on the current in a circuit

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PMMA (Polymethyl Methacrylate) – Chemical Resistance Chart

When selecting chips for microfluidic applications, ensuring chemical resistance is crucial for maintaining system integrity and performance. PMMA (Polymethyl Methacrylate) is a popular choice due to its optically clear nature, lightweight properties, and shatter-resistant characteristics. It is commonly used in medical, pharmaceutical, and food processing applications because of its excellent resistance to water, alcohols, and a variety of chemicals.

However, like all materials, PMMA has its limitations, and not every chemical is compatible with it. Therefore, understanding resistance is essential for preventing chip degradation and ensuring safety. In this guide, we present a comprehensive table of chemical resistance for PMMA chips. This table, based on the chemical resistance data (at 20°C) provided by Reichelt Chemietechnik , is designed to help engineers, technicians, and researchers quickly determine whether PMMA chips are suitable for their specific applications, ensuring reliable and long-lasting performance in various chemical environments.

Refer to this table to make informed choices and maintain the efficiency and safety of your system.

💡 The chemical resistance rating key is as follows:

• resistant = no effect to slight effect
• limited resistance = moderate effect 

🚨 The resistance ratings provided in these tables are for general guidance only and may not be complete or accurate. They do not address potential contamination or changes in fluid properties due to tubing interaction. We do not guarantee the suitability of any material for specific purposes or the impact of tubing on fluid quality. For critical applications, conduct specific tests or seek expert advice.

PMMA Chips: Chemical Resistance Table

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Acid–base back titration

By Sandrine Bouchelkia and Jo Haywood

• Five out of five

Experiment and develop learners’ quantitative analysis skills

This resource accompanies the article The essential guide to teaching quantitative chemistry in  Education in Chemistry , where you will find tips, common misconceptions and further ideas for teaching reacting masses and limiting reagents. 

Use the technician notes to prepare the practical and find the experimental procedure in the student worksheet.

Download this

Use the experiment and accompanying resources, including answers, to develop your post-16 learners' quantitative chemistry skills.

Learning objectives

• Apply your knowledge of mole calculations to practical experimental data.
• Write balanced equations for practical experiments.
• Review practical techniques.

Learners will address all three objectives throughout the experiment. They should successfully carry out the practical, write relevant balanced equations and utilise these to carry out mole calculations. Learners will draw their findings together in a conclusion and evaluation, comparing their experimental and theoretical data. Find the answers in the teacher notes and use the accompanying mole calculator spreadsheet to check learners’ calculations.

Scaffolding

Some learners will be keen to work through the whole task independently. Others will benefit from you checking the calculation steps as they go along, ensuring they have correctly balanced the equations and found the masses and moles before they write their conclusion and evaluation. Use the PowerPoint  (also available as a  pdf ) to model each step of the calculation. Remove the example tables in the student sheet to encourage learners to draw their own or leave them in for support.

As an extension, ask learners to titrate the original HCl against the NaOH to check the concentration is correct. They can also investigate the effect of CO 2 dissolving on the pH of water .

Safety and hazards

• Read our standard health and safety guidance  and carry out a risk assessment before running any live practical.
• Eye protection must be worn.
• The flask containing hydrochloric acid and calcium carbonate may get warm.
• Instruct learners to take care not to spill solutions, particularly phenolphthalein, on their skin. If they do get any on their skin, rinse well.
• Fill the burette at eye level.

Do the experiment individually or as a pair/small group. Each learner/group will require:

• Two 100 ml conical flasks
• 25 ml or 50 ml pipette
• 10 ml pipette
• Pipette fillers sized to match pipettes
• Mass balance measuring three decimal places (0.001 g)*
• Clamp and retort
• Cotton wool
• Safety equipment: safety glasses

*If a mass balance measuring three decimal places is not available then use a mass balance measuring two decimal places (0.01 g). This will be less accurate though.

• Hydrochloric acid, 1.00 mol dm -3
• Calcium carbonate chips (approx 1.00 g)
• Sodium hydroxide, 0.400 mol dm -3
• Phenolphthalein indicator solution in dropper bottles

More resources

• Develop learners’ practical skills by ensuring your feedback is meaningful with the  Common Practical Assessment Criteria (CPAC) tracker .
• Use the  Quantitative chemistry starters to practice skills relating to concentration, mass and gas calculations with your 16–18 learners. 
• Bring together organic chemistry and moles calculations with the  Aspirin screen experiment .
• Review your 14–16 year-old learners’ understanding of key ideas, words and phrases relating to quantitative chemistry by downloading the  scaffolded, partially scaffolded and unscaffolded worksheets .
• Solidify you knowledge with the  Quantitative chemistry online CPD course  and download the accompanying resources  too.
• Prepare tables for your results before you start your experiments.
• Using the pipette, accurately measure out 50 ml of 1.00 mol dm -3 hydrochloric acid and add this to the conical flask. Place a piece of cotton wool in the top of the flask.
• Measure the mass of the flask, cotton wool and hydrochloric acid. Record this in the table.
• Using the three decimal places (dp) mass balance, accurately weigh out between 1.000 and 1.500 g (1.00 to 1.50 g for the two dp mass balance) of calcium carbonate and record the mass in the table.
• Add the calcium carbonate to the hydrochloric acid and swirl the flask until all of the calcium carbonate has reacted.
• Measure the final mass of the flask and contents and record in the table.
• Fill the burette with sodium hydroxide solution (0.400 mol dm -3 ) using a funnel and pouring at your eye level.
• Using a 10 ml pipette, measure out 10 ml of your reaction mixture into a clean 100 ml conical flask.
• Add a few drops of phenolphthalein to the flask containing your reaction mixture. The mixture should remain colourless.
• Titrate your mixture with the sodium hydroxide from your burette, recording how much sodium hydroxide you require to turn the mixture pink.
• Rinse the conical titration flask with distilled water.
• Repeat steps 6–11 until you have two results, excluding the rough titration, which are within 0.05 ml of each other (or you run out of reaction mixture).
• Calculate the average titre to use in the calculations.

Acid–base back titration student sheet

Acid–base back titration teacher notes, acid–base back titration technician notes, acid–base back titration calculation slides, acid–base back titration mole calculator, additional information.

Resource created by Jo Haywood. Technician notes adapted by Sandrine Bouchelkia.

• 16-18 years
• Practical experiments
• Presentation
• Teacher notes
• Technician notes
• Maths skills
• Practical skills and safety
• Investigation
• Applying scientific method
• Acids and bases
• Quantitative chemistry and stoichiometry
• Asking scientific questions
• Observing and measuring
• Recording data
• Interpreting data
• Reactions and synthesis

Specification

• C5.1b describe the technique of titration
• Students should be able to: describe how to carry out titrations using strong acids and strong alkalis only (sulfuric, hydrochloric and nitric acids only) to find the reacting volumes accurately
• (HT) Calculate the chemical quantities in titrations involving concentrations in mol/dm³ and in g/dm³.
• C5.4.7 describe and explain the procedure for a titration to give precise, accurate, valid and repeatable results
• C5.3.6 describe and explain the procedure for a titration to give precise, accurate, valid and repeatable results
• AT f: Use acid–base indicators in titrations of weak/strong acids with weak/strong alkalis.
• Titrations of acids with bases.
• Students should be able to perform calculations for these titrations based on experimental results.
• 11. be able to calculate solution concentrations, in mol dm⁻³ and g dm⁻³, including simple acid-base titrations using a range of acids, alkalis and indicators. The use of both phenolphthalein and methyl orange as indicators will be expected.
• 4. use laboratory apparatus for a variety of experimental techniques, including:
• titration, using burette and pipette
• 6. use acid-base indicators in titrations of weak/strong acids with weak/strong alkalis
• di) use of laboratory apparatus for a variety of experimental techniques including: i) titration, using burette and pipette
• f) use of acid–base indicators in titrations of weak/ strong acids with weak/strong alkalis
• d) the techniques and procedures used when preparing a standard solution of required concentration and carrying out acid–base titrations
• carrying out a back titration
• quantitative stoichiometric calculations
• Back titration is used to find the number of moles of a substance by reacting it with an excess volume of reactant of known concentration.
• The resulting mixture is then titrated to work out the number of moles of the reactant in excess.
• From the initial number of moles of that reactant the number of moles used in the reaction can be determined, making it possible to work back to calculate the initial number of moles of the substance under test.
• A back titration is useful when trying to work out the quantity of substance in a solid with a low solubility.
• Stoichiometry is the study of quantitative relationships involved in chemical reactions.
• The ability to balance and interpret equations enabling calculations to be carried out involving any of the above skills/techniques is an important part of chemistry at this level and is examinable in both the Unit and Course assessments.
• process and analyse data using appropriate mathematical skills as exemplified in the mathematical appendix for each science
• consider margins of error, accuracy and precision of data
• follow written instructions
• make and record observations
• keep appropriate records of experimental activities
• present information and data in a scientific way
• evaluate results and draw conclusions with reference to measurement uncertainties and errors
• comment on experimental design and evaluate scientific methods
• use laboratory apparatus for a variety of experimental techniques including: titration, using burette and pipette
• use acid-base indicators in titrations of weak/strong acids with weak/strong alkalis
• carry out experimental and investigative activities, including appropriate risk management, in a range of contexts
• evaluate methodology, evidence and data, and resolve conflicting evidence
• (f) acid-base titrations
• PRACTICAL: Back titration, for example, determination of the percentage of calcium carbonate in limestone
• (f) relationship between grams and moles
• (g) concept of concentration and its expression in terms of grams or moles per unit volume (including solubility)
• (j) concept of stoichiometry and its use in calculating reacting quantities, including in acid-base titrations
• 5.3.4 demonstrate understanding of the method of back titration, for example by determining the purity of a Group II metal oxide or carbonate.
• determine the purity of a Group II metal oxide or carbonate by back titration;
• use volumetric flasks to prepare standard solutions of various volumes and safely use a burette and a pipette with acid-base indicators to carry out titrations of weak or strong acids with weak or strong alkalis;
• Calculations involving excess of one reactant.
• Apparatus used in volumetric analysis.
• Correct titrimetric procedure.
• Acid-base titrations.

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The facile production of p -chloroaniline facilitated by an efficient and chemoselective metal-free n/s co-doped carbon catalyst.

1. Introduction

3. discussion, 4. materials and methods, 4.1. materials synthesis, 4.2. material characterization, 4.3. catalytic tests, 5. conclusions, supplementary materials, author contributions, institutional review board statement, informed consent statement, data availability statement, conflicts of interest.

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Villora-Picó, J.-J.; Gil-Muñoz, G.; Sepúlveda-Escribano, A.; Pastor-Blas, M.M. The Facile Production of p -Chloroaniline Facilitated by an Efficient and Chemoselective Metal-Free N/S Co-Doped Carbon Catalyst. Int. J. Mol. Sci. 2024 , 25 , 9603. https://doi.org/10.3390/ijms25179603

Villora-Picó J-J, Gil-Muñoz G, Sepúlveda-Escribano A, Pastor-Blas MM. The Facile Production of p -Chloroaniline Facilitated by an Efficient and Chemoselective Metal-Free N/S Co-Doped Carbon Catalyst. International Journal of Molecular Sciences . 2024; 25(17):9603. https://doi.org/10.3390/ijms25179603

Villora-Picó, Juan-José, Gema Gil-Muñoz, Antonio Sepúlveda-Escribano, and M. Mercedes Pastor-Blas. 2024. "The Facile Production of p -Chloroaniline Facilitated by an Efficient and Chemoselective Metal-Free N/S Co-Doped Carbon Catalyst" International Journal of Molecular Sciences 25, no. 17: 9603. https://doi.org/10.3390/ijms25179603

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• Published: 03 September 2024

Nano silica-mediated stabilization of heavy metals in contaminated soils

• Maryam Samani 1 ,
• Yogesh K. Ahlawat 2 ,
• Ahmad Golchin 1 ,
• Hossein Ali Alikhani 3 ,
• Arzhang Fathi-Gerdelidani 3 ,
• Umang Ahlawat 4 ,
• Anurag Malik 5 ,
• Reetika Panwar 6 ,
• Deva Shri Maan 7 ,
• Meraj ahmed 8 ,
• Princy Thakur 8 &
• Sadhna Mishra 9  

Scientific Reports volume  14 , Article number:  20496 ( 2024 ) Cite this article

Metrics details

• Biogeochemistry
• Environmental sciences

Soil contamination with heavy metals presents a substantial environmental peril, necessitating the exploration of innovative remediation approaches. This research aimed to investigate the efficiency of nano-silica in stabilizing heavy metals in a calcareous heavy metal-contaminated soil. The soil was treated with five nano-silica levels of 0, 100, 200, 500, and 1000 mg/kg and incubated for two months. The results showed that nano-silica had a specific surface area of 179.68  \({\text{m}}^{2}/\text{g}\) . At 1000 mg/kg, the DTPA-extractable concentrations of Pb, Zn, Cu, Ni, and Cr decreased by 12%, 11%, 11.6%, 10%, and 9.5% compared to the controls, respectively. Additionally, as the nano-silica application rate increased, both soil pH and specific surface area increased. The augmentation of nano-silica adsorbent in the soil led to a decline in the exchangeable (EX) and carbonate-bound fractions of Pb, Cu, Zn, Ni, and Cr, while the distribution of heavy metals in fractions bonded with Fe–Mn oxides, organic matter, and residue increased. The use of 1000 mg/kg nano-silica resulted in an 8.0% reduction in EX Pb, 4.5% in EX Cu, 7.3% in EX Zn, 7.1% in EX Ni, and 7.9% in EX Cr compared to the control treatment. Overall, our study highlights the potential of nano silica as a promising remediation strategy for addressing heavy metal pollution in contaminated soils, offering sustainable solutions for environmental restoration and ecosystem protection.

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Introduction.

Soil, a critical component of the ecosystem, significantly affects the health of plants, animals, and humans. In the ongoing battle against environmental pollution, soil contamination with heavy metals presents a significant challenge, threatening both ecosystems and human health. The behavior of heavy metals in soils varies with soil type, and composition, and over time, with chemical reactions often reducing their bioavailability and solubility. Unlike organic pollutants, heavy metals remain in the soil for long periods, resisting chemical and microbial decomposition, necessitating their relocation, removal, or impact reduction 1 . Traditional remediation methods often fail to effectively address the complex nature of heavy metal contamination in soils. However, emerging technologies are offering innovative and sustainable solutions to remediate heavy metal-contaminated soils.

A cost-effective method for mitigating heavy metal contamination in soil is immobilization 2 . This environmentally friendly approach aims to prevent toxic compounds from entering biological cycles by reducing their solubility or toxicity 3 . Immobilization involves mixing contaminated soil with suitable compounds, which induces changes in pH, specific surface area (SSA), ion exchange, adsorption, and stabilization processes, thereby reducing the mobility and toxicity of pollutants 4 . Various soil components, such as silicate minerals, organic matter, clay minerals, and iron and manganese oxides, can trap heavy metals in their lattice structures or form bonds with them. The strength of these bonds affects the retention or release of heavy metals from the soil 5 .

Heavy metals in soils exist in different geochemical forms. The distribution of these geochemical forms in soils varies based on pH, cation exchange capacity, soil texture, redox state, organic matter, lime, and Fe–Mn oxide contents 6 . An understanding of the distribution of heavy metals among these various geochemical forms is crucial in determining their solubility, availability, and toxicity in the soil 7 . The sequential extraction method 5 serves as a valuable tool for identifying the chemical forms of heavy metals and assessing their bioavailability 8 .

The traditional stabilizers for the immobilization of heavy metals include lime, hydroxyapatite, zeolite, phosphates 9 , bentonite 10 , fly ash and red mud, and so on 11 . Furthermore, new materials, such as nano-materials 12 , biochar 13 , 14 , polymer 15 and modified material 16 are also used as stabilizer to remediate heavy metal contaminated soils. These stabilizers can reduce the activity of heavy metals in soils to a certain extent, but their specificity and long-term stability are not enough, and their influence on soil properties has not been detected, which limits their large-scale application. Therefore, it is necessary to develop a new stabilizer with strong specificity, long-term stability and few adverse effects on soil environment.

Silica or functionalized silica can be used as an adsorbent to remove heavy metals from aqueous systems and to immobilize them in soil. Silica is an inorganic solid that is made of a three-dimensional network structure and a porous structure with a very large surface area. Silica is mainly composed of siloxane groups (Si–O–Si) inside and silanol groups (Si–OH) on the particle surface. Silanol groups can be separated into three types (single classified silanol), geminal (binary), and adjacent silanol. Silanol groups located on the surface of silica easily react with various agents. Many properties such as adsorption, adhesion, catalytic, and chemical properties of silica depend on the chemistry of these surface groups 17 . In addition to the surface, silanol groups may also be found inside the silica skeleton. Silanol groups are hydrophilic and siloxanes are hydrophobic 18 .

Nanoparticles are used in many sciences. Many nanoparticles have very different properties from micro and macro materials. The main reason for using nanoparticles is their very small size and large specific surface area, which play an important role in chemical reactions. Nanoparticles are widely used in the stabilization of heavy metals in soils due to their high adsorption capacity, high reactivity, and unsaturated surfaces. Silicon dioxide modified nanoparticles have been used in some studies as a sorbent to remediate heavy metals in soil and alleviate the stress of heavy metals on plants. For example, Zhang 19 reported that the application of modified nano-silica transformed Cu, Pb, and Zn to a more stable fraction in soil. Lian 20 indicated that the nano-silica decreased the DTPA-extractable Cd in soil effectively. However, the application rates of nano-silica in their research were much higher than an acceptable rate for large-scale applications (the maximum application rate is 6%). In recent years, research on the application of nano-silica for the removal or stabilization of heavy metals in aquatic environments 21 , 22 , 23 , 24 , 25 , 26 and functionalized nano-silica for the stabilization of heavy metals in soils 27 , 28 , 29 , 30 at high rates economically unfeasible has shown promising results. However, the use of un-functionalized silica nanoparticles for the remediation of heavy metals in complex soil environments, especially at economically feasible rates, has been relatively overlooked. Building on this foundation, a new study has been conducted to explore using un-functionalized silica nanoparticles to stabilize heavy metals in soil. This innovative approach not only aims to improve the efficiency of metal stabilization but also seeks to understand the impact of nano-silica on soil properties and the re-distribution of metals within different soil solid phases.

The goals of this research include (i) investigating the influences of un-functionalized nano-silica on specific surface area and pH of calcareous soil as two important soil factors affecting the sorption and availability of heavy metals, (ii) assessing the effectiveness of un-functionalized nano-silica in stabilizing heavy metals in calcareous soil, and (iii) unraveling the mechanisms underlying the stabilization of heavy metals by un-functionalized nano-silica. By shedding light on these aspects, the study provides valuable insights into the potential of un-functionalized nano-silica for the remediation of heavy metal-contaminated soils.

Materials and methods

Soil analysis.

A composite soil sample at a depth of 0–15 cm was collected from an urban park located in Tehran, Iran. The sample was air-dried at room temperature, passed through a 2 mm sieve, analyzed for physico-chemical properties, and used for this study. Soil texture was determined by the hydrometer method 31 . The pH at a 1:5 soil-to-water ratio and the electrical conductivity of saturated paste extract (ECe) were measured using a pH meter and an EC meter, respectively 32 , 33 . Organic carbon and calcium carbonate contents in the soil were measured by using Walkley–Black 34 and the Calcimetry methods 35 . Cation exchange capacity (CEC) was determined using the sodium acetate method 36 , and specific surface area (SSA) was measured by BET. The available fractions of heavy metals in the soil were extracted by DTPA 37 , and their concentrations were determined using ICP-MS. Total concentration of heavy metals in the soil was measured by ICP-MS after aqua regia digestion 38 .

Soil amendment

Nano-silica with a chemical formula \({\text{SiO}}_{2}\) and a purity of 99.5% was prepared by Pasargad Novin Chemical Company. Some characteristics of the prepared nano-silica were determined using XRF, XRD, SEM, FTIR, and BET techniques.

Pot experiment

To investigate the effect of nano-silica on the immobilization of Pb, Zn, Cu, Ni, and Cr in the soil, a pot experiment was conducted under greenhouse conditions using a completely randomized design and three replications. The nano-silica was mixed with three kg of urban soil at five rates of 0, 100, 200, 500, and 1000 mg nano-silica per kg soil. Treated and untreated (control) soil samples were incubated for two mouths at the moisture of field capacity. At the end of the incubation period, treated and untreated soil samples were air-dried at room temperature and used to evaluate the impacts of different levels of nano-silica on available and chemical fractions of Pb, Zn, Cu, Ni, and Cr in the soil.

Sequential extraction

Chemical fractions of heavy metals were determined in treated and untreated soil samples by the sequential extraction method 5 . This procedure partitions the total content of heavy metal into five fractions: exchangeable (EX), bound to carbonates (CAR), bound to Fe–Mn oxides (OX), bound to organic matter (OM), and residual (RES). Each fraction was extracted by a special extractant at a given time and temperature presented in Table 1 .

Statistical analysis

The experimental data were analyzed using the SPSS 21.0 statistical software package and Microsoft Excel 2016. The experiment was conducted based on a completely randomized design (CRD) with three replicates for each treatment. The treatments included five nano-silica levels of 0, 100, 200, 500, and 1000 mg/kg. A one-way ANOVA was performed to determine the effect of different levels of nano-silica on each response variable. The means for each treatment group were compared using Duncan’s multiple range test at a significance level of P  < 0.05.

Results and discussion

Soil characteristics.

Some physico-chemical properties of the soil used in this study are summarized in Table 2 . The studied soil was non-saline, calcareous, poor in OC content, and with a basic pH and a silty loam texture.

Nano-silica characteristics

Xrf analysis.

The results of the chemical analysis of nano-silica by XRF are shown in Table 3 . Silica nanoparticles have more than 99% silicon dioxide, and the impurities include Fe and Na, with amounts less than 20 and 50 mg/kg, respectively. Calcium and Ti are also present, with values less than 70 and 120 mg/kg, respectively.

XRD analysis

The XRD pattern of silica nano adsorbent is shown in Fig.  1 . Intense peaks at 22.15 and 44.3 angles indicate the presence of \({\text{SiO}}_{2}\) crystal structure in the tetragonal crystal system. Parameters a, b, and c are determined as 4.7, 4.7, and 7.4, respectively. Among other crystallographic parameters of this material, we can mention alpha, beta, and gamma, all of which are 90° (Fig.  1 ).

The XRD pattern of nano-silica. Crystallin structure in tetragonal crystal system.

The SEM image

The surface morphology of silica particles determined by a scanning electron microscope (SEM) is shown in Fig.  2 . Silica nanoparticles have a spherical shape.

SEM image of nano-silica.

The FTIR spectrum

FTIR analysis was used to determine surface functional groups affecting adsorption. The FTIR spectrum of silica nanoparticles is shown in Fig.  3 . The strong peaks in the regions of 471.04, 812.12, and 1138.25  \({\text{cm}}^{-1}\) are related to the asymmetric stretching vibrations of siloxane groups (Si–O–Si). The peak in the region of 3427.6  \({\text{cm}}^{-1}\) corresponds to the vibrational stretching of the O–H group, which overlaps with the silanol (Si–OH) group 39 , 40 .

FTIR spectrum showing Siloxan (Si–O–Si), O–H and Silanol (Si–OH) groups in nano-silica.

BET specific surface area

Based on the results of the BET technique, the adsorption and desorption curve of nano-silica is type IV, indicating the mesoporous structure of silica. Silica nanoparticles have a specific surface area of 179.68  \({\text{m}}^{2}/\text{g}\) and the percentage of porosity is 93.95% (Fig.  4 a). The mesopore volume and diameter are obtained from the BJH curve. According to the BJH curve, the total volume and diameter of the nano-silica pores were 0.397  \({\text{cm}}^{3}/\text{g}\) and 2.42 nm, respectively (Fig.  4 b).

( a ) Adsorption/desorption isotherm used to calculate the specific surface area of nano-silica using the BET technique. ( b ) BJH plot used to calculate the total volume and the diameter of the nano-silica pores using the BET technique.

The nano-silica effect on soil pH

The results of The nano-silica effects on soil pH are presented in Fig.  5 . The results showed that application of nano-silica caused an increase in soil pH compared to the control treatment. The pH value increased from 7.43 in the control to 7.87 and 7.88 with the application of 500 and 1000 mg of silica per kg of soil, respectively. pH is one of the important factors in controlling the balance between heavy metal solution in soil 41 . Previous reports indicated that the addition of Si-based materials changed the pH of the soil 42 , which was observed in the present research.

The effect of different nano-silica levels on soil pH.

The nano-silica effect on the DTPA-extractable concentrations of metals

The mean comparison results of the effects of different nano-silica levels on the DTPA extractable concentration of heavy metals showed that the highest available concentration of metals was in the control treatment, while the lowest available concentration of metals was in the 1000 mg/kg Nano-silica treatment (Fig.  6 ).

The effect of different nano-silica levels on concentration of DTPA heavy metals. For each metal, means with a common letter are not significantly different (P \(<\) 0.05).

The highest and lowest concentrations of DTPA extractable Pb were 7.54 and 6.63 mg/kg, with a 12% decrease observed when applying 1000 mg/kg of nano-silica compared to the control treatment. For Zn and Cu, the highest concentrations found in the control treatment were 27.12 and 7.75 mg/kg, respectively, while the lowest concentrations observed in the 1000 mg/kg treatment were 24.08 and 6.85 mg/kg, resulting in an 11% decrease for Zn and an 11.6% decrease for Cu compared to the control. Similarly, for Ni and Cr, the highest concentrations found in the control treatment were 6.24 and 9.42 mg/kg, respectively, and the lowest concentrations observed in the 1000 mg/kg treatment were 5.61 and 8.52 mg/kg, corresponding to a 10% decrease for Ni and a 9.5% decrease for Cr compared to the control treatment. Overall, the most significant reduction in the available concentration of heavy metals in the tested soil was observed for Pb, followed by Cu, Zn, Ni, and Cr ( 4 ).

Unique properties exist between different heavy metal ions, such as ionic radius, electronegativity, and hydration radius 43 . Previous studies have shown that these intrinsic properties are inseparable from the adsorption properties of heavy metal ions, and the adsorption stability and adsorption energy are also affected by them 43 . In a study conducted by Pan 43 , they stated the modified biomass-based adsorption technique has attracted much attention in heavy metal ions removal, a carboxylated biogas residue (BR–COOH) was prepared to remove the \({\text{Cu}}^{2+}\) and \({\text{Zn}}^{2+}\) from single/binary heavy metal ions solution and explore selective adsorption mechanism. The results exhibited that the adsorption capacities of BR–COOH for \({\text{Cu}}^{2+}\) was higher than that for \({\text{Zn}}^{2+}\) obviously, whether in the single or binary heavy metal ions solution. Meanwhile, the inconsistency in the change of adsorption capacity for \({\text{Cu}}^{2+}\) and \({\text{Zn}}^{2+}\) also confirmed that differences in affinity exist between BR–COOH and different heavy metal ions, and \({\text{Cu}}^{2+}\) seems to be more readily captured. The maximum adsorption capability of \({\text{Cu}}^{2+}\) was visibly higher than that of \({\text{Zn}}^{2+}\) , indicating that the \({\text{Cu}}^{2+}\) preferentially adsorbed to the carboxyl functional groups and occupied the active sites at the same time. The adsorbed \({\text{Cu}}^{2+}\) was unable to be exchanged into solution by \({\text{Zn}}^{2+}\) . They also reported the adsorbed quantities of these metal ions followed the order of \({\text{Hg}}^{2+}\) > \({\text{Cu}}^{2+}\) > \({\text{Pb}}^{2+}\) > \({\text{Fe}}^{2+}\) > \({\text{Cd}}^{2+}\) > \({\text{Zn}}^{2+}\) > \({\text{Mn}}^{2+}\)  >  \({\text{Mg}}^{2+}\) . The difference in the amounts of Pb, Cu and Zn adsorbed may be due to the acid–base theory. Pb belongs to hard acids and tends to complex with hydroxy (hard base) groups on the surface of silica more than Cu and Zn. Thus, Pb is more prone to immobilization than Cu and Cd 44 . The amount of specific adsorption of ions on solid surfaces depends largely on the electric charge, the hydration radius of the ions, the sealing energy, and the electronegativity of the ions. Reducing the hydrated radius and energy, and increasing the electronegativity increases the tendency to ion-specific adsorption 45 . The reason for the higher adsorption of Pb and Cu ions than Zn is likely due to the lower hydrated radius of the Pb (0.401 nm), and Cu (0.419 nm) compared to the Zn (0.43 nm) and their higher electronegativity 46 , 47 . Pan 43 stated that \({\text{Cu}}^{2+}\)  was more easily adsorbed onto carboxylated biosorbent than \({\text{Zn}}^{2+}\) .

In the present study, it was observed that soil pH increased with increasing the application level of nano-silica, but the concentration of DTPA-extractable Cr decreased from 9.4 mg/kg in the control treatment to 8.5 mg/kg at the highest nano-silica application level. A negative correlation between soil pH and heavy metal mobility in soil and bioavailability to plants has been well documented in the literature 48 . However, the effect of soil pH on Cr sorption/desorption in soil varies with its chemical form and oxidation state. Chromium in soil exists in two common oxidation states: Cr(III), and Cr (VI). In the Cr(III) valence state, Cr is a metal cation (as the free \({\text{Cr}}^{3+}\) species or as a hydrolysis product: \({\text{CrOH}}^{2+}\) or \({\text{Cr}(\text{OH})}_{2}^{+}\) depending on solution pH). In the Cr (VI) state, Cr occurs in the chromate species: \({\text{HCrO}}_{4}^{-}\) and \({\text{CrO}}_{4}^{2-}\) 49 . Thus, increasing soil pH has a contrary effect on the sorption of Cr(III) and Cr (VI) species. The sorption of Cr(III) on soil solids increases with an increase in pH, while Cr (VI) sorption on soil particles decreases with an increase in pH 48 . Nano-silica induced coordination, co-precipitation, and other geochemical behaviors with Cr, which inhibit the increased electrostatic repulsion of Cr (VI) with soil colloids resulted from an increase in soil pH, could be reasons for this decreased DTPA-extractable concentration of Cr observed in the present study 50 , 51 .

It seems that the application of 1000 mg/kg nano-silica provided sufficient surfaces for the adsorption of heavy metals thus decreasing their concentration in the soil solution. The surfaces of nano-silica have hydroxyl active groups that have high adsorption capacity and are in the forms of free silanol (Si–OH) groups, free silanol diol groups ( \({\text{Si}-(\text{OH})}_{2}\) ) and atomic bridges with oxygen ions (Si–O–Si) in surface 17 . Silanol groups on the silica surface react easily with a variety of agents. The adsorption capacity of the silica depends on the charge and electronegativity of the metals; the metal cations in the solution form a chemical bond with the siloxane oxygen attached to the surface of the silica. Both silanol and siloxane groups in the nano-silica surface play a very important role in the adsorption capacity of metals 52 . Lian 20 reported that \({\text{SiO}}_{2}-\text{SH}\) can significantly (P \(<\) 0.05) decrease the heavy metal concentration in the plants, which indicates that the \({\text{SiO}}_{2}-\text{SH}\) can immobilize the heavy metals in the contaminated soil and reduce their phytoavailability. Some Si-based materials have been used to remediate heavy metals in soil and alleviate the stress of heavy metals on plants 13 , 53 .

Zhang 27 reported that the application of modified nano-silica transformed Cu, Pb, and Zn to a more stable fraction in soil. Lian 20 indicated that the nano-silica decreased the DTPA-extractable Cd in soil effectively. Silica nanoparticles ( \({\text{NSiO}}_{2}\) ) are very efficient in removing metal ions due to the surface characteristics of silica 54 . Investigations showed that among various organic and inorganic modifiers, silica nanoparticles are widely used due to their large surface area and suitable places for metal adsorption. Studies on the adsorption of heavy metals Ni, Cd, and Pb by porous silica nanoparticles in aqueous environments have been also carried out. Rezvani-Barojni 55 stated that nano-silica has a high adsorption capacity for Hg and this adsorbent had inhomogeneous adsorption sites that had different adsorption potentials.

The soil pH effect on the DTPA-extractable concentrations of metals

The results showed by increasing the soil pH, the DTPA extractable concentrations of heavy metals decreased (Fig.  7 ). The surface charge of silica increases with increasing pH, and at higher pH, the negative charge of the silica surface causes more metal cations to be adsorbed 56 . An increase in pH causes a decrease in metals in the available fractions of heavy metals and a reduction in their bioavailability in the soil 10 , 57 . Heidari 57 also reported that by increasing the pH of the solution, the adsorption capacity of silica for Ni, Cd, and Pb increased.

The pH effect on DTPA-extractable concentrations of heavy metals in the studied soil. For each metal, means with a common letter are not significantly different (P \(<\) 0.05).

In the adsorption process, solution pH is crucial; it influences both the contaminants’ ionization level and the adsorbent’s surface charge 58 . Meky 26 in a study about the pH effect on removing Pb by nano-silica from aqua medium reported when pH falls below 3, the synthesized nano \({\text{SiO}}_{2}\) ’s zeta potential data shows that it has reached the isoelectric point, which is the point at which the positive and negative charges produced by the silanol groups on the surface of the silica particles are equal. The silanol groups with the Si–OH structure are stable at that moment. The zeta potential grows in negative proportion as the pH value rises over 3.5, signifying a rise in the amount of negative charges on the particle surface. The equilibrium of the SiOH/SiO—acid/base dissociation means that an increase in negative charges will lead to an increase in \({\text{SiO}}^{-}\) species and the surface energy 59 . Subsequently, the surface of \({\text{SiO}}_{2}\) is positively charged at any pH value below the pzc and negatively charged at any pH value over the pzc. For Pb (II), when the pH of the solution increases (pH > 3), the surface of the synthesized nano- \({\text{SiO}}_{2}\) becomes negatively charged, and as a result, the adsorption of positively charged Pb (II) is enhanced due to the electrostatic attraction. Ahmad 60 also investigated the effect of silica nanoparticles on Cu adsorption in the aqueous medium and found that by increasing the pH of the solution from 4 to 6.5, the amount of Cu adsorption increased. This shows that at lower pH, the concentration of \({\text{H}}^{+}\) ions is high and these ions are competing with other metal ions to form chelate and complexation in the exchange sites of the silica surface. At higher pH, hydroxyl ions in the reaction medium increase, and metal ions tend to form hydroxide or react with surface hydroxyls.

The nano-silica effect on soil SSA and the relationship between soil SSA and DTPA-extractable concentrations of metals

The application of nano-silica to soil increased its SSA. The soil SSA increased from 19.63 \({\text{m}}^{2}/\text{g}\) in the control treatment to 21.23, 22.83, 24.43, and 26.03  \({\text{m}}^{2}/\text{g}\) with the application of 100, 200, 500, and 1000 mg/kg nano-silica, respectively. Increasing the soil SSA by applying nano-silica reduced the DTPA-extractable concentrations of heavy metals (Fig.  8 ). There was a good correlation coefficient \({\text{R}}^{2}\) between the soil SSA and DTPA extractable concentrations of heavy metals. The R 2 s obtained were obtained were 87% for Pb and Cu > 86% for Zn and Cr > 83% for Ni. The inverse correlation between soil SSA and DTPA extractable concentrations of heavy metals suggests that the increased surface area of the soil due to the application of nano-silica leads to increased adsorption of heavy metals, resulting in a reduction of their concentrations in the solution phase. The higher the amount of nano-silica present, the greater the available surface area provided, leading to increased metal adsorption. Specific surface area is the most effective property in the soil treated with silica Si nanoparticles, leading to many changes in physico-chemical properties 61 , 62 . Bayat 63 reported the positive effects of different nanomaterials on soil surface area using magnesium oxide (MgO).

Relationship between the soil SSA and DTPA-extractable concentrations of heavy metals.

A material with a higher SSA can adsorb more heavy metal ions per unit mass compared to a material with a lower surface area. This is because a larger surface area provides more sites for the heavy metal ions to attach to the adsorbent material. Specific surface area is often correlated with the pore structure of the adsorbent material. Materials with higher surface areas tend to have a greater proportion of mesopores and micropores, which can provide additional surface area for adsorption and offer diffusion pathways for heavy metal ions into the material. The SSA influences the kinetics and thermodynamics of the adsorption process. A higher surface area can accelerate the adsorption kinetics by providing more sites for heavy metal ions to interact with the adsorbent material. Additionally, it can enhance the thermodynamic driving force for adsorption, leading to higher adsorption capacities. The high surface area of the silica compared to soil, provided high reactive sites, which allowed metal ions to be adsorbed on them 64 . Silica nanoparticles ( \({\text{SiO}}_{2}\) ) are very efficient in removing metal ions due to the surface characteristics of silica 54 . Investigations showed that among various organic and inorganic modifiers, silica nanoparticles are widely used due to their large surface area and suitable places for metal absorption.

In a study by Al-Saeed 65 on the contribution of nano-silica in affecting some of the physico-chemical properties of cultivated soil, it was noted that varying rates of nano-silica have a significant effect on the percentage of clay particles, cation exchange capacity (CEC), sodium adsorption ratio (SAR), porosity, saturation percentage, SSA, and the concentrations of total nitrogen (N) and silicon ( \({\text{Si}}^{4+}\) ).

The effect of different silica nano levels on the fractionation of heavy metals in soil

The distribution of different geochemical forms of heavy metals Pb, Zn, Cu, Ni and Cr in untreated soil (control treatment) was as follow: CAR (43.79%) > OX (16.98%) > OM (14.49%) > RES (12.78%) > EX (11.1%) for Pb; CAR (45%) > OX (17%) > RES (15.5%) > OM (13.2%) > EX (9.3%) for Zn; CAR \(=\) OX (28.13%) > RES (23.49%) > OM \(=\) EX (10.19%) for Cu; OX (44.8%) > CAR (20.78%) > RES (14.48%) > EX (11.9%) > OM (8.04%) for N; and CAR (40.8%) > OX (18.52%) > RES (15.19%) > OM (14.19%) > EX (11.3%) for Cr (Table  5 and Fig.  9 ).

Effect of different nano-silica levels on the distribution of geochemical fractions of heavy metals in the studied soil. F1: Exchangeable, F2: Carbonated bound, F3: Fe/Mn Oxyhydroxide, F4: Organic matter bound, and F5: Residual fraction.

Mean comparisons showed that with increasing the nano-silica application level in the soil, the exchangeable and carbonate-bounded fractions of Pb, Cu, Zn, Ni, and Cr decreased but the Fe–Mn OX, OM, and RES fractions increased (Table 5 and Fig.  9 ).

At the nano-silica application level of 1000 mg/kg, the concentration of the EX and CAR bound fractions of Pb decreased from 6.73 and 26.03 mg/kg in the control treatment to 6.19 and 25.42 mg/kg, accounting for 8.02% and 2.34%, respectively. However, when applying nano-silica at a level of 1000 mg/kg, the concentration of the OX fraction of Pb increased from 10.28 mg/kg in the control treatment to 10.59 mg/kg. Similarly, the concentration of the OM fraction of Pb rose from 8.75 to 8.92 mg/kg, and the concentration of the RES fraction of Pb increased from 8.03 to 8.33 mg/kg. The increase in the concentration of different chemical forms of Pb using silica nanoparticles follows the order: RES (3.73%) > OX (3.01%) > OM (1.94%).

For Cu, by an increase in the amount of nano-silica in the soil, the concentration of EX and CAR fractions of Cu decreased by 4.46% and 2.26%, respectively, compared to the control treatment, so that the concentration of EX fraction of Cu was 6.27 mg/kg in the control treatment reached to 5.99 mg/kg in the 1000 mg/kg nano-silica treatment. The CAR fraction of Cu decreased from 17.22 mg/kg in the control treatment to 16.83 mg/kg in the 1000 mg/kg of nano-silica. In 1000 mg/kg nano-silica, the amount of OX fraction of Cu increased from 17.24 mg/kg in the control treatment to 17.39 mg/kg. The OM fraction of Cu also increased from 6.27 mg/kg in the control treatment to 6.63 mg/kg with the application of nano-silica. Similarly, the Res fraction of Cu increased from 14.44 mg/kg in the control treatment to 14.57 mg/kg. The augmentation of Cu chemical forms through the application of silica nanoparticles followed this order: OM (5.74%) > RES (0.9%) > OX (0.87%).

The concentration of the EX and CAR bound fractions of Pb decreased from 6.27 and 17.22 mg/kg in the control treatment to 5.99 and 16.83 mg/kg at the nano-silica application level of 1000 mg/kg, representing 4.46% and 2.26% reductions, respectively. Conversely, in the 1000 mg/kg nano-silica treatment, the concentration of the OX fraction of Cu increased from 17.24 mg/kg in the control treatment to 17.39 mg/kg.

The concentration of the EX and CAR bound fractions of Zn decreased from 18.68 and 90.42 mg/kg in the control treatment to 17.32 and 88.7 mg/kg at the nano-silica application level of 1000 mg/kg, representing 7.28% and 1.9% reductions, respectively. Conversely, in the 1000 mg/kg nano-silica treatment, the concentration of the OX and Res fractions of Zn increased from 26.52 and 31.14 mg/kg in the control treatment to 26.88 and 31.25 mg/kg, in 1000 mg/kg nano-silica treatment, respectively. The effect of silica nanoparticles on changing the distribution of Zn chemical forms followed as OX (6.76%) > OM (1.35%) > RES (0.35%).

For Ni, the concentration of the EX and CAR bound fractions of Ni decreased from 4.76 and 8.31 mg/kg in the control treatment to 4.42 and 7.97 mg/kg at the nano-silica application level of 1000 mg/kg, corresponding to 7.14% and 4.09% reductions, respectively. Conversely, in the 1000 mg/kg nano-silica treatment, the concentration of the OX and Res fractions of Ni increased from 17.93 and 5.76 mg/kg in the control treatment to 18.26 and 5.96 mg/kg, in 1000 mg/kg nano-silica treatment, respectively. The effect of silica nanoparticles on changing the distribution of Ni chemical forms followed the order OM (6.54%) > RES (3.47%) > OX (1.88%).

For Cr, the concentration of the EX and CAR bound fractions of Cr decreased from 8.87 and 32.03 mg/kg in the control treatment to 8.17 and 31.77 mg/kg at the nano-silica application level of 1000 mg/kg, accounting for 7.9% and 0.8%, respectively. Conversely, in the 1000 mg/kg nano-silica treatment, the concentration of the OX, OM, and Res fractions of Cr increased from 14.53, 11.14, and 12.32 mg/kg in the control treatment to 14.77, 11.22, and 12.47 mg/kg, in 1000 mg/kg nano-silica treatment, respectively. The effect of silica nanoparticles on changing the distribution of Cr chemical forms followed the order OX (1.72%) > RES (1.21%) > OM (0.71%).

In the present study, the exchangeable and carbonate-bounded fractions of heavy metals decreased by using nano-silica. Previous research indicated that the exchangeable and carbonate-bounded fractions of heavy metals usually determine the real environmental risk 14 , which means the addition of nano-silica reduced the risk of heavy metals in the contaminated soil. Similar results have also been reported by Lian 20 and Wang 53 .

Several mechanisms, such as adsorption, complexation, co-precipitation, and changes in soil properties like pH and surface area, have been reported in the literature for the redistribution and immobilization of heavy metals in soils induced by the nanosilica application. Nano-silica has a high specific surface area and can provide numerous active sites for adsorption of heavy metals such as Pb, Cu, Zn, Ni, and Cr through inner-sphere surface complexation 20 , 66 , 67 . The sorption of heavy metals onto \({\text{SiO}}_{2}\) surfaces can reduce their concentrations in the more easily extractable fractions (e.g., exchangeable, and carbonated bound), effectively sequestering them and preventing their leaching or mobility 20 . Heavy metals that are strongly adsorbed to the nano-silica surface will also be associated with the residual fraction, as they become more resistant to extraction 20 . \({\text{SiO}}_{2}\) can also co-precipitate with trace metals, incorporating them into the \({\text{SiO}}_{2}\) mineral structure 66 . The co-precipitation of heavy metals with \({\text{SiO}}_{2}\) can reduce their concentrations in the carbonated bound and Fe–Mn oxide fractions, as the co-precipitated metals will be associated with the residual fraction, which represents the most recalcitrant and structurally incorporated forms of the metals 5 . Nano-silica can alter the soil pH, which can influence the solubility and mobility of heavy metals. A higher pH can lead to the precipitation of metal hydroxides, which can then become associated with Fe/Mn oxyhydroxides 30 . This transformation can result in a decrease in the exchangeable and carbonate bounded fractions as metals are immobilized in less bioavailable forms 30 . The presence of nano-silica can also enhance the binding of heavy metals to organic matter in the soil, as it can act as a bridge between the metal ions and organic functional groups 68 . This results in an increase in the organic matter bounded fraction of heavy metals 53 .

Conclusions

Applying the nano-silica increased the soil pH and SSA but decreased the DTPA-extractable concentrations of heavy metals in the studied calcareous soil. The nano-silica caused a significant decrease in the concentrations of Pb, Cu, Zn, Ni, and Cr in the exchangeable and carbonate-bound fractions, while the distribution of heavy metals in fractions bonded with Fe–Mn oxides, organic matter, and residue increased. The highest effect of silica nano sorbent in reducing the available concentration of heavy metals in the studied soil was Pb > Cu > Zn > Ni > Cr. There was a good correlation coefficient ( \({\text{R}}^{2}\) ) between the soil SSA and DTPA-extractable concentrations of heavy metals. Nano-silica could be used to remediate heavy metal-contaminated agricultural soils. The stabilization mechanism of heavy metals could be attributed to the -SH and -OH bonds of Nano-silica. This study suggests that nano-silica has advantages and potential in the remediation of heavy metal-contaminated agricultural soils.

While nano-silica-mediated stabilization of heavy metals in contaminated soils holds great promise, further research is warranted to address certain aspects and optimize its application. The following future directions could guide ongoing investigations: Understanding the interactions at the nanoscale is essential for tailoring nano-silica to target different contaminants. Transitioning from laboratory experiments to field-scale trials is critical for validating the efficacy of nano-silica under real-world conditions. This step will provide insights into its performance in diverse soil types, climates, and contaminant scenarios. Also, a comprehensive assessment of the ecological impact of nano-silica on non-target organisms, plant growth, and overall soil biodiversity is necessary. This will ensure that the technology does not inadvertently lead to unintended environmental consequences.

Evaluating the economic feasibility of large-scale nano-silica applications is crucial for its practical implementation. Assessing the cost-effectiveness of the technology will contribute to its adoption by regulatory bodies and industries involved in environmental remediation.

Data availability

All data generated or analysed during this study are included in this published article [and its supplementary information files ].

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M.S., A.G., and H.A.A.; Writing-original draft, Visualization, Methodology, Investigation, Formal analysis, Data curation, Conceptualization. A.F.G., and Y.K.A, A.M, U.A, R.P, D.S.M, M.A, P.T, S.M.; Writing-review & editing, Methodology, Investigation, Data curation, Conceptualization. A.G., and H.A.A.; Supervision, Project administration, Funding acquisition. All authors have read and agreed to the published version of the manuscript.

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Samani, M., Ahlawat, Y.K., Golchin, A. et al. Nano silica-mediated stabilization of heavy metals in contaminated soils. Sci Rep 14 , 20496 (2024). https://doi.org/10.1038/s41598-024-69182-0

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DOI : https://doi.org/10.1038/s41598-024-69182-0

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