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Related Concept Videos

Factors Affecting Solubility04:01

Factors Affecting Solubility

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:
Acid Halides to Alcohols: LiAlH4 Reduction01:19

Acid Halides to Alcohols: LiAlH4 Reduction

Acid halides are reduced to alcohols in the presence of a strong reducing agent like lithium aluminum hydride.
The mechanism proceeds in three steps. First, the nucleophilic hydride ion attacks the carbonyl carbon of the acid halide to form a tetrahedral intermediate. Next, the carbonyl group is re-formed, and the halide ion departs as a leaving group, generating an aldehyde. A second nucleophilic attack by the hydride yields an alkoxide ion, which, upon protonation, gives a primary alcohol as...
Washing, Drying, and Ignition of Precipitates00:52

Washing, Drying, and Ignition of Precipitates

After filtration, the precipitate is washed to remove coprecipitated impurities and any remaining mother liquor. Colloidal precipitates, such as silver chloride, are washed with an electrolyte (such as dilute nitric acid) to prevent the peptization of the precipitate. In the case of slightly soluble precipitates, the wash solution contains a common ion to reduce solubility. Lead sulfate, which is slightly soluble in water, is washed with dilute sulfuric acid. Similarly, wash solutions may be...
Extraction: Advanced Methods00:56

Extraction: Advanced Methods

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 formed in...
Phosphate Buffer01:22

Phosphate Buffer

The phosphate buffer system is a critical biological mechanism for maintaining pH stability in the body. This system operates primarily through two components: sodium dihydrogen phosphate (NaH2PO4), which acts as a weak acid, and sodium hydrogen phosphate (Na2HPO4), which serves as a weak base.
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Synthesis of Ionic Liquid Based Electrolytes, Assembly of Li-ion Batteries, and Measurements of Performance at High Temperature
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Published on: December 20, 2016

Phosphate removal from water using lithium intercalated gibbsite.

Shan-Li Wang1, Chia-Yi Cheng, Yu-Min Tzou

  • 1Department of Soil and Environmental Sciences, National Chung Hsing University, Taichung, Taiwan. slwang@dragon.nchu.edu.tw

Journal of Hazardous Materials
|January 24, 2007
PubMed
Summary

Lithium intercalated gibbsite (LIG) effectively removes phosphate from water primarily via anion exchange. This efficient phosphate scavenger demonstrates strong adsorption capacity, particularly at lower pH.

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Published on: May 18, 2018

Area of Science:

  • Environmental Chemistry
  • Materials Science
  • Water Treatment

Background:

  • Phosphate contamination in water bodies is a significant environmental concern, leading to eutrophication.
  • Developing efficient and cost-effective adsorbents for phosphate removal is crucial for water remediation.

Purpose of the Study:

  • To investigate the efficacy of lithium intercalated gibbsite (LIG) for phosphate removal from water.
  • To elucidate the adsorption mechanisms of phosphate onto LIG.
  • To determine the adsorption capacity and influencing factors such as pH and ionic strength.

Main Methods:

  • Preparation of lithium intercalated gibbsite (LIG) by intercalating LiCl into gibbsite.
  • Batch adsorption experiments conducted at various pH values and ionic strengths.
  • Analysis of adsorption isotherms using the Langmuir model.
  • Investigation of adsorption mechanisms including anion exchange and surface complexation.

Main Results:

  • LIG exhibited an L-shaped adsorption isotherm, well-fitted by the Langmuir model.
  • The maximum adsorption capacity was 3.0 mmol g(-1) at pH 4.5, decreasing with increasing pH.
  • Phosphate adsorption occurred mainly through chloride ion displacement (anion exchange), with surface complexation also contributing at lower pH.
  • Adsorption was pH-dependent, influenced by the phosphate species ratio and surface charge of LIG.
  • Anion exchange was rapid, while surface complexation was slow; adsorption decreased with increased ionic strength at lower pH but was unaffected at higher pH.

Conclusions:

  • Lithium intercalated gibbsite (LIG) is a promising adsorbent for efficient phosphate removal from water.
  • The primary mechanism is fast anion exchange, complemented by surface complexation.
  • LIG demonstrates high selectivity for phosphate, especially at higher pH, indicating its potential for water treatment applications.