Influence of dissolved oxygen on aggregation kinetics of citrate-coated silver nanoparticles

Biological responses of silver-coated thermosets: An in vitro and in vivo study

“…Dissolution of silver in aqueous solutions is dependent on electrolyte type and concentration, pH, temperature and the presence of dissolved oxygen [44][45][46][47][48]; in particular, the presence of electrolytes in aqueous solution diminishes the electrostatic energy barrier to nanoparticle aggregation [45]. The release rate of silver strongly depends also on the initial concentration of nanoparticles on the surface and on the rate at which the soaking solution diffuses into the coating, which both decrease upon leveling-off of the corresponding gradients [49,50].…”

Perturbation of cellular mechanistic system by silver nanoparticle toxicity: Cytotoxic, genotoxic and epigenetic potentials

“…In the absence of dissolved oxygen Ag+ release will be completely inhibited which in turn affect toxicity [41]. Due to decrease in the pH, dissolution of Ag NPs occurs; it is also related to size of Ag NPs [202]. Particle agglomeration do affect toxicity as shown in a recent study on zebrafish embryo development in various ionic strength medium, such as CaCl2, ultrapure water and embryo medium, due to agglomeration the toxicity of Ag NPs varies in various mediums, there was inverse relation between toxicity and agglomeration [ 211].…”

Modeling physicochemical interactions affecting in vitro cellular dosimetry of engineered nanomaterials: application to nanosilver

“…AgNP is known to be oxidized by dissolved oxygen (DO) in the media and the reaction is also influenced by the protons (H + ) in the media (Zhang et al 2011; Tejamaya et al 2012). The chemical reaction for the oxidation of Ag in solution can be expressed as Zhang et al (2011): $$\mathrm{Ag}\left(\mathrm{normals}\right)+\frac{1}{4}{\mathrm{normalO}}_2\left(\mathrm{aq}\right)+{\mathrm{normalH}}^{+}\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+\frac{1}{2}{\mathrm{normalH}}_2\mathrm{O}\left(1\right)$$ The chemical equilibrium for the above reaction can be assessed using Nernst equation, as $$E_{\mathrm{net}}=E^{\mathrm{normalo}}-\frac{RT}{nF}\log true(\frac{\left[{\mathrm{Ag}}^{+}\right]}{\left[{\mathrm{normalH}}^{+}\right]{\left[{\mathrm{normalO}}_2\right]}^{1∕4}}true)$$ Here, R is the Universal Gas constant, T is the temperature of the reaction medium, F is Faraday's constant, and n is the difference in the number of molecules between reactants and products based on reaction stoichiometry. E o is the standard reaction potential (at 25 °C) for the reaction whose value is 0.47 volts (Zhang et al 2011).…”