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Colloidal precipitates01:09

Colloidal precipitates

5.7K
The high insolubility of some precipitates can result in an unfavorable relative supersaturation. This can lead to colloidal particles with a large surface-to-mass ratio, where adsorption is promoted. For instance, in the precipitation of silver chloride, silver ions are adsorbed on the surface of the colloidal particles, forming a primary layer. This layer attracts ions of opposite charge (such as nitrate ions), forming a diffuse secondary layer of adsorbed ions. This electric double layer...
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The Colloidal State01:29

The Colloidal State

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The formation of a colloidal system is exemplified by an aqueous solution containing Cl− ions is introduced to another containing Ag+ ions, resulting in the precipitation of solid AgCl as extremely tiny crystals. Instead of settling out as a filterable precipitate, these crystals remain suspended in the liquid, showcasing a colloidal system.A colloidal system involves colloidal particles within the approximate range of 1 to 1000 nm in at least one dimension, dispersed in a medium called...
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Colloids03:22

Colloids

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Children at play often make suspensions such as mixtures of mud and water, flour and water, or a suspension of solid pigments in water known as tempera paint. These suspensions are heterogeneous mixtures composed of relatively large particles that are visible to the naked eye or can be seen with a magnifying glass. They are cloudy, and the suspended particles settle out after mixing. On the other hand, a solution is a homogeneous mixture in which no settling occurs and in which the dissolved...
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Formation of Complex Ions03:45

Formation of Complex Ions

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A type of Lewis acid-base chemistry involves the formation of a complex ion (or a coordination complex) comprising a central atom, typically a transition metal cation, surrounded by ions or molecules called ligands. These ligands can be neutral molecules like H2O or NH3, or ions such as CN− or OH−. Often, the ligands act as Lewis bases, donating a pair of electrons to the central atom. These types of Lewis acid-base reactions are examples of a broad subdiscipline called coordination...
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Complexation Equilibria: Factors Influencing Stability of Complexes01:09

Complexation Equilibria: Factors Influencing Stability of Complexes

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In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
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Factors Affecting Solubility04:01

Factors Affecting Solubility

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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:
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Tangential Flow Ultrafiltration: A “Green” Method for the Size Selection and Concentration of Colloidal Silver Nanoparticles
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Protein-silver nanoparticle interactions to colloidal stability in acidic environments.

Jui-Ting Tai1, Chao-Shun Lai, Hsin-Chia Ho

  • 1Department of Chemical Engineering, National Tsing Hua University , Hsinchu, Taiwan 30013, Republic of China.

Langmuir : the ACS Journal of Surfaces and Colloids
|October 9, 2014
PubMed
Summary

We studied silver nanoparticles (AgNPs) in acidic conditions and found that bovine serum albumin (BSA) significantly improves their stability. BSA coating prevents aggregation and dissolution, crucial for nanoparticle applications.

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Area of Science:

  • Nanomaterials Science
  • Physical Chemistry
  • Biomaterials Science

Background:

  • Silver nanoparticles (AgNPs) are widely used but their stability in acidic environments is a concern.
  • Protein interactions can significantly influence nanoparticle behavior and stability.
  • Understanding AgNP colloidal stability is crucial for their safe and effective application.

Purpose of the Study:

  • To investigate the colloidal stability of AgNPs in acidic conditions (pH 2.3 to ~7).
  • To determine the impact of protein interactions, using bovine serum albumin (BSA), on AgNP stability.
  • To elucidate the mechanisms governing AgNP aggregation and dissolution under varying acidity.

Main Methods:

  • Electrospray-differential mobility analysis (ES-DMA) for particle size and concentration.
  • Transmission electron microscopy (TEM) for visualizing AgNP morphology.
  • Kinetic studies to determine aggregation rate constants and binding affinities.

Main Results:

  • Unconjugated AgNPs showed increased aggregation and particle size with higher acidity.
  • Aggregation rate constant (kD) correlated with acidity: log(kD) = -1.627(pH)-9.3715.
  • BSA strongly bound to AgNPs (K ≈ 1.1 × 10^6 L/mol), forming a protective corona.
  • BSA-functionalized AgNPs exhibited enhanced colloidal stability, suppressing aggregation and dissolution in acidic media.

Conclusions:

  • AgNP aggregation is the dominant factor affecting colloidal stability in acidic environments.
  • BSA corona formation effectively mitigates both particle aggregation and interfacial dissolution.
  • Protein functionalization is a key strategy for enhancing the stability of AgNPs in challenging conditions.