Question

the process of seperation of ions present in an ionic compound?

Answer 1

$\sf\blue{An}\sf\orange{s}\sf\red{w}\sf\green{er :-}$Chemical Separation of Metal Ions. Formation of crystals from a saturated solution is a heterogeneous equilibrium phenomenon, and it can be applied to separate various chemicals or ions in a solution. When solubilities of two metal salts are very different, they can be separated by precipitation

Answer 2

Answer:

There are no definite dividing lines between insoluble salts, sparingly soluble, and soluble salts, but concentrations of their saturated solutions are small, medium, and large. Solubility products are usually listed for insoluble and sparingly soluble salts, but they are not given for soluble salts. Solubility products for soluble salts are very large.

What type of salts are usually soluble, sparingly soluble and insoluble? The following are some general guidelines, but these are not precise laws.

All nitrates are soluble. The singly charged large NO−3 ions form salts with high solubilities. So do ClO−4 , ClO−3 , NO−2 , HCOO− , and CH3COO− .

All chlorides, bromides, and iodides are soluble except those of Ag+ , Hg2+2 , and Pb2+ . CaF2 , BaF2 , and PbF2 are also insoluble.

All sulfates are soluble, except those of Ba2+ , Sr2+ , and Pb2+ . The doubly charged sulfates are usually less soluble than halides and nitrates.

Most singly charge cations K+ , Na+ , NH+4 form soluble salts. However, K3Co(NO2)6 and (NH4)3Co(NO2)6 are insoluble.

These are handy rules for us to have if we deal with salts often. On the other hand, solubility is an important physical property of a substance, and these properties are listed in handbooks.