Related Experiment Video
Updated: Nov 15, 2025
08:01
Removal of Arsenic Using a Cationic Polymer Gel Impregnated with Iron Hydroxide
Published on: June 28, 2019
7.7K
Arsenic removal in aqueous solutions using FeS2
Dun Fu1, Tonni Agustiono Kurniawan2, Lan Lin3
1National Engineering Research Center of Coal Mine Water Hazard Controlling, School of Resources and Civil Engineering, Suzhou University, Suzhou 234000, Anhui, PR China; College of the Environment & Ecology, Xiamen University, Xiamen, 361102, Fujian, PR China.
Journal of Environmental Management
|March 5, 2021
Summary
Pyrite and persulfate effectively remove arsenic from water. Adding persulfate to pyrite treatment ensures complete arsenic removal, meeting World Health Organization standards for safe drinking water.
Area of Science:
- Environmental Chemistry
- Water Treatment Technologies
- Materials Science
Background:
- Arsenic contamination in water poses significant health risks.
- Conventional arsenic removal methods can be inefficient or costly.
- Pyrite is a potential low-cost adsorbent for contaminant removal.
Purpose of the Study:
- To assess the technical feasibility of using pyrite and persulfate for arsenic removal.
- To investigate the synergistic effects of pyrite and persulfate in arsenic remediation.
- To elucidate the adsorption mechanisms and redox processes involved.
Main Methods:
- Batch studies were conducted to explore arsenic-pyrite interactions.
- Physico-chemical properties and adsorption mechanisms were analyzed.
- The integrated pyrite-persulfate system was tested under various conditions.
Main Results:
- Pyrite effectively adsorbed arsenic in a pH range of 6-11.
- As(III) required longer equilibrium time (8h) than As(V) (2h).
- Optimal conditions (0.25 g/L pyrite, pH 8.0, 5 mg/L As(III)) with 0.5 mM persulfate achieved complete arsenic removal (<10 μg/L).
Conclusions:
- Pyrite is a viable adsorbent for arsenic removal from aqueous solutions.
- Persulfate addition significantly enhances arsenic removal efficiency.
- The combined system meets stringent arsenic maximum contaminant limits.
Related Concept Videos
01:17Precipitation and Co-precipitation
3.2K
Precipitation and coprecipitation methods can be used to separate a mixture of ions in a solution. In qualitative inorganic analysis, ions that form sparingly soluble precipitates with the same reagent are separated based on the differences in solubility products. For example, consider the separation of Cu(II) and Fe(II) ions by precipitation as insoluble sulfides. First, copper(II) sulfide is precipitated by the addition of acidic H2S, where the dissociation of H2S is suppressed. Adding H2S...
3.2K
00:56Extraction: Advanced Methods
774
Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is...
774
01:08Sample Preparation for Analysis: Advanced Techniques
861
Accurate analysis of complex samples often requires advanced preparation techniques to achieve reliable and reproducible results. Samples containing inorganic or organic materials can be challenging to dissolve or decompose effectively. Standard sample preparation methods include acid digestion, fusion, dry ashing, and wet digestion.
Acid digestion with strong acids is commonly used to dissolve inorganic materials that are insoluble (do not dissolve) in water. This method can be useful for...
Acid digestion with strong acids is commonly used to dissolve inorganic materials that are insoluble (do not dissolve) in water. This method can be useful for...
861
04:01Factors Affecting Solubility
35.6K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
35.6K
03:10Precipitation Reactions
60.4K
In a precipitation reaction, aqueous solutions of soluble salts react to give an insoluble ionic compound – the precipitate. The reaction occurs when oppositely charged ions in solution overcome their attraction for water and bind to each other, forming a precipitate that separates out from the solution. Since such reactions involve the exchange of ions between ionic compounds in aqueous solution, they are also referred to as double displacement, double replacement, exchange reactions, or...
60.4K
03:11Precipitation of Ions
29.1K
Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
29.1K