INTRODUCTION
Water is indispensable for sustaining life and maintaining essential biological functions, as it plays a critical role in human health and ecosystem stability. Nevertheless, the progressive contamination of water resources by diverse pollutants, including synthetic dyes, heavy metals, pesticides, microbial contaminants, pharmaceutical residues, and radioactive substances, poses a serious environmental challenge, leading to ecological imbalance and adverse effects on living organisms. [1–3]. Dyes are one of the most significant of these pollutants because they are released in large amounts by a great variety of industries: textiles, leather processing, cosmetics, food production, and even medical usage. Millions of tons of dye-containing effluents are discharged into water systems each year all over the world [4]. Dyes can be broadly described as substances that are organic and can absorb light in the visible color spectrum, thus giving them a specific coloration [5]. One of the most commonly used synthetic dyes is crystal violet (CV), also known as gentian violet, basic violet 3, methyl violet 10B, or hexamethylpararosaniline chloride. It is described as purple in color, which is of an intense nature, but it is not naturally obtained. The molecular formula of the compound is C₂₅H₃₀ClN₃, and the molecular weight is 407.98 g/mol. Crystal violet (CV) is a triarylmethane dye that is part of the triarylmethane group of dyes that also include malachite green and bromophenol blue [6]. The group of dyes is regarded as one of the most dangerous environmental pollutants because it is very toxic, persistent, andresistant to biodegradation, and has been found to be potentially carcinogenic [7,8]. Crystal violet is capable of producing serious color contamination in water bodies even at low concentrations, and this disturbs photosynthetic processes and aquatic ecosystems by lowering light penetration. This results in an imbalance of the ecology and adversely influences the existence and physiological functions of aquatic organisms [9,10]. In order to deal with such contamination, different water treatment methods have been devised. The most successful and cost-effective method of these has been adsorption, which is simple, environmentally friendly, and removes with high efficiency [11].
Nanomaterials have received significant interest in recent years due to their distinctive physicochemical characteristics at the nanoscale, contributing to their better performance in environmental use [12-15]. One of the main benefits of nanomaterials is that nanomaterials have a high surface area-to-volume ratio that contributes to high surface reactivity and adsorption capacity [16, 17]. This is an advantage of nanotechnology that requires a significant amount of energy and is thus effective in treating wastewater to remove a broad spectrum of pollutants, including heavy metals, organic pollutants, and pathogenic bacteria and viruses [18]. AgNPs are one of the most promising nanomaterials, as they have such unique characteristics as low-cost production, environmental friendliness, and high antimicrobial activity, especially against multidrug-resistant microorganisms. Notably, they show moderate levels of toxicity to normal cells at regulated levels [19]. As a result, AgNPs have been given much attention regarding various uses such as antibacterial therapy and environmental cleanup [20–23]. Moreover, silver nanoparticle materials have outstanding optical, electrical, and antimicrobial characteristics that render them very useful in the field of water sanitation, elimination of pollutants, environmental sensing, and energy-related technologies [24–29].
The present study focuses on three main aspects. First, silver nanoparticles were synthesized using a simple, rapid, and cost-effective laboratory method. Second, the synthesized nanoparticles were characterized to confirm their successful formation and nanoscale features. Third, and most importantly, their efficiency was evaluated in the removal of C.V dye as a representative organic pollutant from aqueous solutions.

MATERIALS AND METHODS
Materials
Silver Nitrate (99.9%, Reagn World), chemical formula (AgNO3) and molecular weight = 169.87 g/mol. Sodium Citrate (99.0 %, ACS Chemicals), chemical formula (C6H5Na3O7) and molecular weight=294.10g/mol .Sodium Borohydride (98.0%, CDH), chemical formula (NaBH4 ) and molecular weight = 37.83 g/mol. Crystal Violet has chemical formula (C25H30ClN3)and molecular weight = 407.98 g/mol .Citric acid anhydrous (99.5%, HiMedia), chemical formula (C6H8O7) and molecular weight =192.123 g/mol. Hydrogen Peroxide (35%, ACS Chemicals), chemical formula (H2O2 ) molecular weight 34.01g/mol.

Instrumentation 
All absorbance measurements were carried out using a UV–Visible spectrophotometer, and the maximum absorption wavelength (λmax) was identified using a Shimadzu UV-1700 spectrophotometer. The pH values were determined using an Oakton 2100 series pH meter. Sample weighing was performed with a Pioneer PA214 analytical balance (Ohaus). Additional instruments employed in this study included a centrifuge (Cen12190), a magnetic stirrer with hot plate, Fourier Transform Infrared Spectroscopy (FTIR) for functional group analysis, Transmission Electron Microscopy (TEM) and Scanning Electron Microscopy analysis (SEM) for morphological characterization.

Solutions preparation
Silver Nitrate solution 0.05 mol/L;Prepared by dissolving 0.8494 g of AgNO3in 100 mL of deionized water in a suitable volumetric flask .Sodium Citrate solution 0.075 mol/L;The tri sodium citrate (TSC) solution was prepared by dissolving 2.2057g in 100 ml of deionized water in a suitable volumetric flask.Sodium Borohyride solution 0.1 mol/L;Prepared by dissolving 0.3783g in 100mL of deionized water in a suitable volumetric flask.Citric acid solution 0.1 mol/L;it was prepared by dissolving 1.9213g in 100 mL distilled water. C.V solution 100 mg/L.
A stock solution was prepared by dissolving 0.0100 g of C.V dye in 100mL distilled water, and working solution were obtained by further dilution.

Procedure
The first method of preparing silver nanoparticles
A 100 mL aqueous solution of silver nitrate (AgNO3) at a concentration of 2 × 10⁻³ mol·L⁻¹ was heated on a hot plate with continuous magnetic stirring at 80_90 °C for 5 minutes. Subsequently, 15 mL of Trisodium citrate (TSC) solution (1.5%, w/v) was added dropwise under constant stirring. The initiation of the reduction process was indicated by a visible color change from a clear solution to pale yellow, confirming the formation of silver nanoparticles (AgNPs).The reaction mixture was further maintained under continuous stirring at 80–90 °C for an additional 20 minutes to ensure complete reduction and nanoparticle formation. The resulting nanoparticles were then separated by centrifugation and stored at 8 ± 1 °C for subsequent stability evaluation [30].

The second method of preparing silver nanoparticles
Silver nitrate (0.05 molar, 5 ml), trisodium citrate (0.075 molar, 50 ml), and hydrogen peroxide (35% by weight, 6 ml) were vigorously mixed at room temperature in air. Sodium borohydride (NaBH4, 0.1 molar, 25 ml) was rapidly injected into this mixture to initiate the reduction process, immediately resulting in a light yellow solution. After about 3 minutes, the colloidal solution turned dark yellow due to the formation of small silver nanoparticles. Within the next few seconds, the morphology began to change from nanoparticles to nanosheets, accompanied by a colour change of the solution from dark yellow to red, green, and blue. The complete transition from nanoparticles to nanosheets typically took 2 to 3 minutes [31].

Adsorption Batch Studies
The adsorption efficiency of crystal violet (CV) dye was optimized by systematically varying key parameters, including the dosage of silver nanoparticles, contact time, and initial dye concentration. A known mass of silver nanoparticles was added to 3 mL of the crystal violet dye solution, and the removal efficiency was determined using Eq. 1:

Where C1, C2 (mg·L⁻¹) represent the initial and equilibrium concentrations of crystal violet dye, respectively.

RESULTS AND DISCUSSION
Synthesis of silver nanoparticles
In this study, silver nanoparticles were synthesized using two different methods, as shown in Figs. 1 and 2. The results indicated that the second method provided a higher yield and was easier to perform compared to the first method; therefore, it was selected as the primary synthesis approach for the current study. The resulting nanoparticles were thoroughly characterized using available analytical techniques, including ultraviolet–visible (UV–Vis) spectroscopy, Fourier-transform infrared (FTIR) spectroscopy, and transmission electron microscopy (TEM)and Scanning Electron Microscopy analysis (SEM) to confirm their formation at the nanoscale.

Wavelength selected for maximum absorption for C.V dye in different medium
The wavelength of C.V dye was measured at different media (pH 3-10) using a Shimadzu UV-1700 spectrophotometer, where the maximum absorbance of crystal violet is at 587 nm. The best medium was at the acidic medium, which showed the highest absorption peak at acidic medium, accompanied by the highest dye solubility and highest sensitivity for measurement. As shown in Fig. 3.

Calibration Curve of C.V Before Adsorption
A calibration curve for C.V. dye was established at a maximum absorption wavelength of 587 nm prior to the adsorption experiments. This was achieved by preparing a series of standard solutions within the concentration range of 0.1– 8 mg·L⁻¹ and measuring their corresponding absorbance values, as illustrated in Fig. 4. Several analytical parameters were subsequently derived from the calibration curve, including the slope, Sandell’s sensitivity, molar absorptivity, specific absorptivity, The calculated values were 0.2123 for the slope, 4.708 × 10⁻³ µg·cm⁻² for Sandell’s sensitivity, 8.6 × 104 L·mol⁻¹·cm⁻¹ for molar absorptivity, and 212.3 L·g ⁻¹·cm⁻¹ for specific absorptivity.

Identification of silver nanoparticles (Ag Nps) with FTIR spectroscopy [32,33]
For precise characterization of the formation of silver nanoparticles, diagnostic analysis was performed using Fourier Transform Infrared (FTIR) spectroscopy (Fig. 5). According to the spectrum obtained for the first preparation method, the results are summarized in Table 1.
From the FTIR spectrum, it can be concluded that the spectrum is consistent with the formation of stable silver nanoparticles stabilized by citrate. The spectrum demonstrates that sodium citrate covers the surface of the nanoparticles, with direct interaction of carboxyl groups with the metallic surface, which prevents particle aggregation and maintains stability.
The Fourier Transform Infrared (FTIR) spectrum reveals the functional groups associated with the surface of silver nanoparticles (AgNPs) synthesized using silver nitrate, sodium citrate, hydrogen peroxide, and sodium borate (the second method), shown in Fig. 6. Analysis of the peaks in the spectrum helps identify the nature of molecules attached to the nanoparticle surface, which are responsible for oxidation, reduction, and stabilization processes. Table 2 summarizes the main peaks and their interpretation.
From the FTIR analysis, it can be concluded that sodium citrate acts simultaneously as a stabilizing and reducing agent. It reduces silver ions (Ag⁺) to metallic silver (Ag⁰), forming silver nanoparticles. The carboxylate groups (COO⁻) then bind to the nanoparticle surface, forming a protective layer that prevents aggregation. Additionally, the presence of B–O peaks indicates the contribution of sodium borate in stabilizing the reaction medium and assisting in nanoparticle stabilization.

Transmission electron Microscopy (TEM) analysis
In this study, the results of Transmission Electron Microscopy (TEM) analysis were conducted for silver nanoparticles synthesized; the results shown in Figs. 7 and 8. The TEM images revealed that the silver nanoparticles were predominantly quasi-spherical in shape, accompanied by noticeable aggregation in some regions. The observed dark contrast can be attributed to the higher electron density of the nanoparticles compared to the surrounding background, in addition to van der Waals forces between the particles during solvent evaporation on the microscope grid, confirming the formation of silver nanoparticles.
Using the 50 nm scale bar as a reference, particle sizes were analyzed by measuring approximately 15 relatively isolated nanoparticles, along with the dimensions of highly aggregated regions to ensure measurement accuracy. The results indicated that the calculated average particle diameter was 17.9 ± 4 nm of the second method, while 42.5± 3 nm of the first method. The relatively narrow size distribution suggests the efficiency of the preparation method in producing small nanoparticles; however, slight variations in size indicate incomplete homogeneity in growth kinetics during the nucleation and particle development stages. This confirms that the particles fall within the nanoscale range, accompanied by moderate size dispersion. The average particle diameter was calculated according to Eq. 2 [34]. 

Where: Davg = Average particle diameter (nm), di = Individual particle diameter (nm), n = Number of measured particles, For the present analysis, Davg = 268 / 15 = 17.9 nm of second method, Davg = 425 / 10 = 42.5 nm of First method.

Scanning Electron Microscopy analysis (SEM)
The SEM analysis results presented in Figs. 9 and 10 reveal the formation of nanoparticles exhibiting morphologies ranging from quasi-spherical to irregular shapes. A pronounced degree of agglomeration among the nanoparticles is also evident. This phenomenon is commonly observed in nanomaterial’s and is primarily attributed to their exceptionally high specific surface area and surface energy, which promote antiparticle attractive forces and consequently lead to particle aggregation [35].

Optimum conditions study 
Study of pH influence 
The effect of pH on the adsorption of C.V. dye was investigated over a pH range of 3–11. The experiments were conducted using a dye concentration of 10 mg·L⁻¹, 0.01 g of silver nanoparticles, and a shaking time of 5 minutes. The results indicated that the maximum removal efficiency was achieved at pH 3, which was therefore selected as the optimal pH for subsequent experiments, as illustrated in Fig. 11.

Study of shaking time
The effect of shaking time on the adsorption of C.V. dye was investigated over a time range of 3–13 minutes. The experiments were performed using an initial dye concentration of 10 mg·L⁻¹, an adsorbent dose of 0.01 g of silver nanoparticles, and measurements were taken at a wavelength of 587 nm.The results demonstrated that the removal efficiency increased with increasing shaking time, reaching a maximum at 8 minutes. Beyond this point, no significant improvement was observed. Therefore, 8 minutes was identified as the optimal contact time, as illustrated in Fig. 12.

Study of changing the mass of the silver nanoparticles (AgNPS)
The effect of adsorbent mass on the removal of C.V. dye was investigated under the previously optimized conditions. Silver nanoparticle (AgNPs) mass in the range of 0.001–0.03 g was employed to evaluate its influence on adsorption efficiency. The results indicated that the removal efficiency increased with increasing adsorbent mass, reaching a maximum at 0.03 g. This mass was therefore selected as the optimal amount for achieving the highest removal percentage of C.V. dye, as illustrated in Fig. 13.

Study of temperature change
The effect of temperature on the adsorption of C.V dye was investigated under the previously established experimental conditions. The experiments were conducted over a temperature range of 10–30 °C to assess its impact on dye removal efficiency. The results showed that the maximum removal rate was achieved at 25 °C, which was therefore selected as the optimal temperature for the adsorption process, as illustrated in Fig. 14.

Calibration curve for crystal violet
Under the optimized experimental conditions, a calibration curve for C.V. was constructed at 587 nm using a series of standard solutions. The proposed method allowed the quantitative determination of C.V. within the concentration range of 0.3–15 mg·L⁻¹. Linear regression analysis of the calibration data yielded a correlation coefficient of R² = 0.9973, as shown in Fig. 15. Several analytical parameters were derived from the calibration curve, including the slope, Sandell’s sensitivity, molar absorptivity, specific absorptivity, limit of detection (LOD), and limit of quantification (LOQ). The corresponding values were: slope = 0.0095, Sandell’s sensitivity = 0.105 µg·cm⁻², molar absorptivity = 3.8 × 10³ L·mol⁻¹·cm⁻¹, specific absorptivity = 9.5 L·g⁻¹·cm⁻¹, LOD = 0.221 mg·L⁻¹, and LOQ = 0.736 mg·L⁻¹.

Applications
Samples were prepared by stabilizing the acid function of the tap water, beach water, and well water at pH =3, and the dye was added, and the removal is applied using the silver nanoparticles. And the relative error percentage and recovery were calculated using Eqs. 3 and 4 respectively as Table 3.

From the obtained results, it was observed that the recovery percentages ranged between 91.4 and 93.83%. This indicates that the proposed analytical method in the study possesses high efficiency and accuracy, effectively contributing to the removal of the dye under investigation from various aqueous solutions.

CONCLUSION 
It can be concluded from this study that the silver nanoparticles synthesized in the laboratory characterized by a preparation method that is simple, precise, rapid, and economically feasible are highly suitable for the removal of crystal violet dye contamination from aqueous solutions. The obtained recovery percentages were excellent, indicating that the proposed analytical method used in this study possesses high accuracy and efficiency.

ACKNOWLEDGMENTS 
We would like to express our sincere gratitude to the Ministry of Higher Education and Scientific Research, as well as to our university and college, for providing an appropriate scientific environment that supports the conduct of research contributing directly to solving important environmental problems, such as water pollution, and proposing possible treatment methods. Their support through the provision of the necessary requirements for sound scientific research is highly appreciated.

CONFLICT OF INTEREST
The authors declare that there is no conflict of interests regarding the publication of this manuscript.