Silver:

(A) Ores:

• Argentite (silver glance) Ag₂S,
• Horn silver (AgCl) Ruby silver (Pyrargyrite) 3Ag₂S.Sb₂S₃.

(B) Extraction: Cyanide process or Mac Arthus-Forrest cyanide process: This process relies upon the fact that silver, the sulphide or chloride of it, makes soluble complex along with alkali cyanides in the silver. In the existence of blast of air this process indicates that the silver compounds will dissolve in solution of alkali cyanides.

The reaction below explained the process:

The reaction along with the sulphide is reversible and accumulation of Na₂S has to be avoided. The excess of air is constantly passed via the solution that oxidizes Na₂S into sulphate and thiosulphate.

The reaction of it is like this:

 (C) Extraction of Ag from argentiferrous lead (PbS + Ag₂S)- Parke's Process : It is based upon the following facts

a)      Molten Zn and Pb are immiscible; the upper layer is formed by zinc

b)      In molten Zn, Ag is much more soluble

c)      Zn-Ag alloy solidifies previous than molten Pb

d)      Zn being volatile can be separated from Ag through the distillation method. Ag can be purified by using cupellation.

Properties of Silver: 

The properties of silver are as follow:

a)      It is best conductor of heat and electricity.

b)      Silver being soft and it is alloyed.

c)      The formation of the silver alloy is expressed like its purity i.e. the quantity of Ag present in 1000 parts of the alloy Ag does not respond with dilute HCl or dilute H₂SO₄ and aqua regia although alloy reacts with dilute HNO₃ and concentrated HNO₃ anf creating NO and NO₂ correspondingly.

d)      Silver is the white lustrous metal

e)      Chlorine as well reacts with Ag to make AgCl.

f)       Silver alloy is employed for making jewellery consists of 80% Ag and 20% Cu.

2Ag + Cl₂ → 2AgCl

Hot conc. H₂SO₄ reacts with Ag forming SO₂ like Cu

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