Related Experiment Video
Updated: Aug 7, 2025
06:24
Preparation of Nanoparticles for ToF-SIMS and XPS Analysis
Published on: September 13, 2020
8.1K
Can Differently Stabilized Silver Nanoparticles Modify Calcium Phosphate Precipitation?
Suzana Inkret1, Marija Ćurlin2, Kristina Smokrović3
1Laboratory for Biocolloids and Surface Chemistry, Division of Physical Chemistry, Ruđer Bošković Institute, Bijenička c. 54, 10000 Zagreb, Croatia.
Materials (Basel, Switzerland)
|March 11, 2023
Summary
This study shows that silver nanoparticles (AgNPs) influence calcium phosphate (CaP) precipitation, affecting the formation of amorphous calcium phosphate and crystalline phases like hydroxyapatite. This offers a simple method for creating CaP/AgNP composites for biomaterials.
Area of Science:
- Biomaterials Science
- Nanotechnology
- Materials Chemistry
Background:
- Orthopedic implant-associated infections pose a significant challenge, driving the need for novel antimicrobial strategies.
- Calcium phosphates (CaPs) and silver nanoparticles (AgNPs) show promise for combating these infections.
- Room-temperature precipitation is an advantageous method for CaP-based biomaterial preparation, but its application with AgNPs is unexplored.
Purpose of the Study:
- To investigate the influence of different types and concentrations of stabilized AgNPs on CaP precipitation.
- To explore the potential of using precipitation as a method for preparing CaP/AgNP composites.
Main Methods:
- Precipitation of CaPs in the presence of citrate-stabilized (cit-AgNPs), poly(vinylpyrrolidone)-stabilized (PVP-AgNPs), and AOT-stabilized (AOT-AgNPs) silver nanoparticles.
- Characterization of the precipitated phases using Powder X-ray Diffraction (PXRD) and Electron Paramagnetic Resonance (EPR) spectroscopy.
- Analysis of the morphology and stability of amorphous calcium phosphate (ACP) and subsequent crystalline phases.
Main Results:
- Amorphous calcium phosphate (ACP) was the initial precipitate, with its stability significantly affected only by high concentrations of AOT-AgNPs.
- AgNPs altered ACP morphology, leading to gel-like precipitates alongside typical chain-like aggregates.
- A mixture of calcium-deficient hydroxyapatite (CaDHA) and octacalcium phosphate (OCP) formed, with OCP content decreasing as AgNP concentration increased.
- The type of stabilizing agent on the AgNPs influenced the precipitation outcomes.
Conclusions:
- Silver nanoparticles can effectively modify the precipitation process of calcium phosphates.
- The properties of CaP/AgNP composites can be fine-tuned by selecting appropriate AgNP stabilizing agents.
- Precipitation offers a simple, fast, and advantageous method for preparing CaP/AgNP composites for biomaterial applications.
Related Concept Videos
01:09Colloidal precipitates
659
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...
659
00:52Washing, Drying, and Ignition of Precipitates
1.0K
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...
1.0K
03:11Precipitation of Ions
28.1K
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:
28.1K
01:16Precipitate Formation and Particle Size Control
857
In precipitation gravimetry, the precipitating agent should react specifically or selectively with the analyte. While a specific reagent reacts with the analyte alone, a selective reagent can react with a limited number of chemical species.
The obtained precipitate should be either a pure substance of known composition or easily converted to one by a simple process, such as ignition or drying. In addition, the precipitate should be insoluble and easily filterable. In general, filterability...
The obtained precipitate should be either a pure substance of known composition or easily converted to one by a simple process, such as ignition or drying. In addition, the precipitate should be insoluble and easily filterable. In general, filterability...
857
04:01Factors Affecting Solubility
33.7K
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:
33.7K
03:45Formation of Complex Ions
23.8K
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...
23.8K