You don't dissolve anything IN cyanide as it is mostly stored as a sodium or potassium salt. I guess if you exposed such a salt to acid you could get a mildly acidic solvent akin to acetonitrile, but I doubt it.
To dissolve elemental silver, you just need something which "more willing to take electrons than elemental silver is willing to keep them" (electro potential dumbed down a bit)
I think that hydrochloride acid readily dissolves silver, as does any acid, as the proton (H+ / H3O+) is a sufficiently strong oxidizer.
Or maybe I am think of nitric acid.
But still I think that the proton is the actual oxidizer, it is for iron, copper and aluminium, I know without looking at tables, so I bet silver is oxidized by the proton too, OR the nitrate ion is the oxidized.
If HCl where used the result would NOT be dissolving of silver, as AgCl is very insoluble in water, the silver would just be converted to a white precipitate. IF the proton has a high enough potential, someone look it up.
Cyanide I would guess does NOT oxidize elemtal silver, as the compund is very electron rich with the tripple bond, I would guess is was a mild reducing agent rather than an oxidizing agent, but look it up, I never finished my chemistry degree, so...:D
AgCN
In industry, cyanide compounds are widely used during the extraction of gold and silver from ores through processes such as cyanidation. This method involves dissolving the metals in a cyanide solution, allowing for efficient recovery. Additionally, cyanides are utilized in the production of various chemicals, electroplating, and as a precursor in the synthesis of certain plastics and dyes. Due to their toxicity, strict regulations govern their use and disposal to minimize environmental and health risks.
The main uses are the gold and silver extraction; also as precursor of nylon.
Oh, dude, cyanide compounds are like the rockstars of the mining industry. They're used to extract gold and silver from ore in a process called cyanidation. So, yeah, cyanide is basically the VIP guest at the precious metal extraction party.
KCN + RCl ------------>RCN + KCl : this is in aqueous medium. here K+ ions displace the less electropositive R+ ions and hence the rxn is a simple rxn of alkyl halides. AgCN + RCL --------------> R=N-->C + AgCl : but this rxn is in alcoholic medium. N & C ions can both donate a lone pair of electrons. such groups are called ambident nucleophile
The molecular formula for silver cyanide is AgCN.Silver cyanide is often used in silver plating.
The cyanide radical consists of a carbon atom triple bonded to a nitrogen atom, and has a -1 charge. It's CN- as we write it. The only difference between silver and gold cyanide is the silver and the gold. Both precious metals will form a bond with the radical in their +1 valence state, so the observer will see either AgCN or AuCN molecules. The former is, of course, silver cyanide, and the latter is gold cyanide.
When cyanide reacts with silver, it forms a complex coordination compound known as silver cyanide (AgCN). The chemical reaction can be represented as: Ag + CN- → AgCN. Silver cyanide is a white solid that is sparingly soluble in water.
Zinc is used for the recovery of silver from cyanide complex because zinc has a stronger affinity for cyanide compared to silver. When zinc is added to the cyanide solution, it displaces silver from the complex, forming insoluble silver-zinc alloy particles that can be easily separated. Copper is not used because it does not have a strong enough affinity for cyanide to displace silver effectively.
Silvger (Ag) Carbon (C) Nitrogen (N) WRONG Silver (Ag) CN is cyanide Thus Silver Cyanide
AgCN
AgCn
AgCN
AgCN
The chemical formula for silver cyanide is AgCN. It is a white solid compound that is highly toxic and can release hydrogen cyanide gas in contact with acids.
no
Cyanide copper salts are typically prepared by dissolving copper oxide or copper carbonate in hydrocyanic acid. The hydrocyanic acid releases cyanide ions, which react with the copper to form the salt. It is important to handle cyanide compounds with extreme caution due to their toxicity.