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Precipitation of Ions03:11

Precipitation of Ions

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Predicting Precipitation
The equation that describes the equilibrium between solid calcium carbonate and its solvated ions is:
30.3K
Precipitation and Co-precipitation01:17

Precipitation and Co-precipitation

4.3K
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...
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Precipitation Reactions03:10

Precipitation Reactions

65.6K
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...
65.6K
Precipitation Processes01:12

Precipitation Processes

6.3K
The experimental conditions in a gravimetric analysis should be optimized to maximize the particle size and purity of the obtained precipitate. Ideally, the concentration of the precipitating reagent should be low with effective stirring to maintain low relative supersaturation for the growth of large crystals. In homogeneous precipitation, the precipitant is slowly generated by a chemical reaction in the solution to avoid local reagent excesses. For example, urea decomposes gradually to...
6.3K
Precipitation Gravimetry01:03

Precipitation Gravimetry

15.5K
Precipitation gravimetry is based on converting an analyte into a sparingly soluble precipitate, which is separated by filtration and weighed. An ideal precipitate should be pure, insoluble, of known composition, and easily filtered from the reaction mixture.
In determining nickel by gravimetric analysis, a precipitant of ethanolic dimethylglyoxime is added to a hot nickel salt solution. This is quickly followed by the dropwise addition of dilute ammonia solution until precipitation occurs. A...
15.5K
Colloidal precipitates01:09

Colloidal precipitates

6.5K
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...
6.5K

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Macroscale precipitation kinetics: towards complex precipitate structure design.

Nirmali Prabha Das1, Brigitta Müller, Ágota Tóth

  • 1Department of Physical Chemistry and Materials Science, University of Szeged, Rerrich Béla tér 1., Szeged, H-6720, Hungary. schuszti@chem.u-szeged.hu.

Physical Chemistry Chemical Physics : PCCP
|June 5, 2018
PubMed
Summary
This summary is machine-generated.

Researchers developed a spectrophotometric method to measure precipitation reaction timescales. This method helps control inorganic precipitate structures for materials science and pharmaceutical applications.

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Area of Science:

  • Materials Science
  • Chemical Engineering
  • Physical Chemistry

Background:

  • Self-assembled inorganic precipitates offer potential in materials science and pharmaceuticals.
  • Controlling precipitate yield requires understanding reaction kinetics, especially under flow conditions.
  • Coupling between hydrodynamics and chemical reactions is crucial for structure formation.

Purpose of the Study:

  • To present a spectrophotometric method for experimentally determining precipitation reaction timescales.
  • To investigate the kinetic description of the nickel-oxalate system.
  • To demonstrate the application of the method in flow systems.

Main Methods:

  • Spectrophotometric analysis to measure reaction timescales.
  • Utilizing the nickel-oxalate model system.
  • Employing injection experiments to study hydrodynamics-chemistry coupling.

Main Results:

  • A reliable spectrophotometric method for determining precipitation timescales was established.
  • The nickel-oxalate system's kinetics were successfully described by Classical Nucleation Theory and homogeneous kinetics.
  • Power law functions were found suitable for characterizing precipitation kinetics in flow systems.

Conclusions:

  • The developed method enables precise control over precipitation processes.
  • Understanding precipitation kinetics is key for tailoring inorganic micro- and macro-structures.
  • The findings facilitate applications in materials science and the pharmaceutical industry.