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According to the solubility table, nitrates are always soluble, so the strong ionic bond between silver ions and nitrate ions are broken by water molecules because of ion-dipole attraction. By definition, acids ionize in water to give mobile ions, so hydrogen chloride in aqueous solution gives out hydrogen ions (and form hydronium ions) and ...
4) The above explains the hard stuff. The reduction of silver is easy: $\ce{[Ag(NH3)_2]+ + e^- -> Ag + 2NH3}$ The silver in the silver ammonia complex ion has an oxidation state of +1; gaining an electron allows solid silver to precipitate out, giving a positive Tollens test for aldehydes. The ammonia remains unchanged.
The molecular formula for silver oxalate is Ag2C2O4.Silver oxalate is a white powder that is produced as a result of a reaction between silver nitrate and oxalic acid. What is the molecular ...
The chemical formula for aqueous silver nitrate is AgNO3, where Ag is the symbol for silver and NO3 is the polyatomic ion nitrate. When silver nitrate is dissolved in water, it dissociates into ...
When silver nitrate reacts with sodium phosphate, silver phosphate precipitate is formed along with sodium nitrate. The balanced chemical equation for the reaction is: 3AgNO3 + Na3PO4 -> Ag3PO4 ...
The easiest way to decide is by looking at thermodynamic stability--solid silver chloride is more stable. We can experimentally prove this, or use standard enthalpies. Reactions proceed in the direction of more stability, so the above reaction goes forward.
Decomposition of silver nitrate is different as it yields elemental silver. $$\ce{2AgNO3 -> 2Ag + O2 + 2NO2}$$ Usually the metals which lie very low in the activity series decompose to give their elemental form. I don't think it's possible to extract metals from just any nitrate by strong heating.
Compound made from 63.50 silver 8.25 nitrogen and 28.25 oxygen with a total molar mass 169.91g? The compound is silver nitrate (AgNO3). By calculating the molar mass of the compound, which is 169. ...
Situation would get complicated, if nitric acid starts to react with metallic silver or residual ascorbic acid. These side reactions would decrease mineral and eventually also organic acidity. $$\ce{3 Ag + 4 HNO3 -> 3 AgNO3 + 2 H2O + NO}$$ $$\ce{3 C6H8O6 + 2 HNO3 -> 3 C6H6O6 + 4 H2O + 2 NO}$$
It would be soluble potassium silver cyanide K[Ag(CN)2](commercially available), with silver strongly bound to cyanide. Silver (or metal in general) ions too easily available for deposition on cathodes, as are silver ions from silver nitrate, lead to diffusion controlled metal deposition. This prefers exposed metals surfaces which are amplified.