what are the products formed when metal chloride reacts with water?give an example
what are the products formed when metal chloride reacts with water?give an example
Reaction of metallic chlorides in water
The chloride ion has a low surface density charge and does not attract water sufficiently strongly for it to hydrolyse. Hence, any reaction of a chloride with water depends upon the element attached to the chloride.
NaCl and MgCl2 are ionic and water soluble. Mg2+ has a higher surface density of charge than Na+ and hydrolysis occurs to a very small extent. Hence, the aqueous solution of MgCl2 is slightly acidic.
when NaCl is added to water it gets dissociated into ions. Only hydration occurs. No hydrolysis occurs.
NaCl + H2O -------------> Na+( ion) + Cl- ( ion) + H2O
Na+(aq) + 6H2O → [Na(H2O)6]2+(aq)
Hydration:
MgCl2(s) + 6H2O(l) → [Mg(H2O)6]2+(aq) + 2Cl-(aq)
Slightly hydrolysis occurs.
[Mg(H2O)6]2+(aq) + H2O (l) → [Mg(OH)(H20)5]+(aq) + H3O+(l)
AlCl3 shows some covalent character, however it still remains soluble in water. The Al3+ ion produces sufficient surface density of charge for hydrolysis to occur. In the case of AlCl3 the large hydration energy of the Al3+ ion results in a vigorous exothermic reaction with water and the solution formed is quite acidic: pH 3.
Hydration:
AlCl3(s) + 6H2O(l) → [Al(H2O)6]3+(aq) + 3Cl-(aq)
Hydrolysis:
[Al(H2O)6]3+(aq) + H2O(l) → [Al(OH)(H2O)5]2+(aq) + H3O+(l)
Reaction of metallic chlorides in water
The chloride ion has a low surface density charge and does not attract water sufficiently strongly for it to hydrolyse. Hence, any reaction of a chloride with water depends upon the element attached to the chloride.
NaCl and MgCl2 are ionic and water soluble. Mg2+ has a higher surface density of charge than Na+ and hydrolysis occurs to a very small extent. Hence, the aqueous solution of MgCl2 is slightly acidic.
when NaCl is added to water it gets dissociated into ions. Only hydration occurs. No hydrolysis occurs.
NaCl + H2O -------------> Na+( ion) + Cl- ( ion) + H2O
Na+(aq) + 6H2O → [Na(H2O)6]2+(aq)
Hydration:
MgCl2(s) + 6H2O(l) → [Mg(H2O)6]2+(aq) + 2Cl-(aq)
Slightly hydrolysis occurs.
[Mg(H2O)6]2+(aq) + H2O (l) → [Mg(OH)(H20)5]+(aq) + H3O+(l)
AlCl3 shows some covalent character, however it still remains soluble in water. The Al3+ ion produces sufficient surface density of charge for hydrolysis to occur. In the case of AlCl3 the large hydration energy of the Al3+ ion results in a vigorous exothermic reaction with water and the solution formed is quite acidic: pH 3.
Hydration:
AlCl3(s) + 6H2O(l) → [Al(H2O)6]3+(aq) + 3Cl-(aq)
Hydrolysis:
[Al(H2O)6]3+(aq) + H2O(l) → [Al(OH)(H2O)5]2+(aq) + H3O+(l)
