Question

DEFINE FAMILY OF SALT

Answer 1

Family of salt is related to numbers of actions.

Answer 2

Salts are formed by a chemical reaction between: 

A base and an acid, e.g., NH3 + HCl → NH4Cl 
A metal and an acid, e.g., Mg + H2SO4 → MgSO4 + H2 
A metal and a non-metal, e.g., Ca + Cl2 → CaCl2 
A base and an acid anhydride, e.g., 2 NaOH + Cl2O → 2 NaClO + H2O 
An acid and a basic anhydride, e.g., 2 HNO3 + Na2O → 2 NaNO3 + H2O 
Salts can also form if solutions of different salts are mixed, their ions recombine, and the new salt is insoluble and precipitates (see: solubility equilibrium), for example: 
Pb(NO3)2(aq) + Na2SO4(aq) → PbSO4(s) + 2 NaNO3(aq) 

Common salt-forming cations include: 


Iron (II) oxide (FeO) 
Iron (III) oxide (Fe2O3)Ammonium NH4+ 
Calcium Ca2+ 
Iron Fe2+ and Fe3+ 
Magnesium Mg2+ 
Potassium K+ 
Pyridinium C5H5NH+ 
Quaternary ammonium NR4+ 
Sodium Na+ 
Common salt-forming anions (parent acids in parentheses) include: 

Acetate CH3COO− (acetic acid) 
Carbonate CO32− (carbonic acid) 
Chloride Cl− (hydrochloric acid) 
Citrate HOC(COO−)(CH2COO−)2 (citric acid) 
Cyanide C≡N− (hydrogen cyanide) 
Hydroxide OH− (water) 
Nitrate NO3− (nitric acid) 
Nitrite NO2− (nitrous acid) 
Oxide O2− (water) 
Phosphate PO43− (phosphoric acid) 
Sulfate SO42− (sulfuric acid) 
ACIDIC SALTS:- 
Acid salt is a somewhat obscure term for a class of salts formed by the partial neutralization of diprotic or polyprotic acids. Because the parent acid is only partially neutralized, one or more replaceable hydrogen atoms remain. Typical acid salts have one or more alkali (alkaline) metal ions as well as one or more hydrogen atoms. Well known examples are sodium bicarbonate (NaHCO3), sodium hydrosulfide (NaHS), sodium bisulfate (NaHSO4), monosodium phosphate (NaH2PO4), and disodium phosphate (Na2HPO4). Often acid salts are used as buffers.[1] 

For example, the acid salt sodium bisulfate is the main species formed upon the half neutralization of sulfuric acid with sodium hydroxide: 

H2SO4 + NaOH → NaHSO4 + H2O 
Acid salts compounds can act either as an acid or a base: addition of a suitably strong acid will protonate anions, and addition of a suitably strong base will split off H+. The pH of a solution of an acid salt will depend on the relevant equilibrium constants and the amounts of any additional base or acid. A comparison between the Kb and Ka will indicate this: if Kb > Ka, the solution will be basic, whereas if Kb < 'Ka, the solution will be acidic. 
BASIC SALTS:- 
Alkali salts or basic salts are salts which are the product of the neutralization of a strong base and a weak acid. 

Rather than being neutral, as some salts are, basic salts are, as their name suggests, bases. What makes these compounds basic is that the conjugate base from the weak acid hydrolyzes to form a basic solution. In sodium carbonate, for example, the carbonate from the carbonic acid hydrolyzes to form a basic solution. The chloride from the hydrochloric acid in sodium chloride does not hydrolyze, though, so sodium chloride is not basic. 

The difference between a basic salt and an alkali is that an alkali is the insoluble hydroxide compound of an alkali metal or an alkaline earth metal. A basic salt is any salt that hydrolyzes to form a basic solution. The hydroxide compounds are not salts. 

Another definition of a basic salt would be a salt that contains amounts of both hydroxide and other anions. White lead is an example. It is basic lead carbonate, or lead carbonate hydroxide. 

These salts are insoluble and are obtained through precipitation reactions