what is the ionic equation for the hydrolysis reaction of
[Al(H2O)6]Cl3
[Al(H2O)6]Cl3(s) + H2O(l) ==> [Al(H2O)5(OH)]^2+(aq) + H3O^+(aq) + 3Cl^-(aq)
To write the ionic equation for the hydrolysis reaction of [Al(H2O)6]Cl3, we need to consider the dissociation of the compound in water.
Step 1: Dissociation of [Al(H2O)6]Cl3 in water.
The compound [Al(H2O)6]Cl3 can dissociate into its ions in water:
[Al(H2O)6]3+ + 3 Cl-
Note: The water molecules coordinated to the aluminum cation [Al(H2O)6]3+ are not involved in the hydrolysis reaction.
Step 2: Hydrolysis of the Cl- ions.
In the hydrolysis reaction, the Cl- ions react with water molecules to form hydrochloric acid (HCl) and hydroxide ions (OH-):
Cl- + H2O → HCl + OH-
Step 3: Combining the equations.
Now, we can combine the dissociation of [Al(H2O)6]Cl3 and the hydrolysis of Cl- to write the overall reaction and the ionic equation:
Overall reaction:
[Al(H2O)6]3+ + 3 Cl- + 3 H2O → [Al(H2O)3(OH)3] + 3 HCl
Ionic equation:
[Al(H2O)6]3+ + 3 H2O → [Al(H2O)3(OH)3] + 3 H3O+
To determine the ionic equation for the hydrolysis reaction of [Al(H2O)6]Cl3, you need to understand the concept of hydrolysis and identify the ions involved in the reaction.
Hydrolysis occurs when a compound reacts with water and splits into two or more ions. In this case, [Al(H2O)6]Cl3 will hydrolyze into its constituent ions.
Let's break down the compound [Al(H2O)6]Cl3:
[Al(H2O)6]Cl3 consists of a central aluminum ion (Al) coordinated with six water molecules (H2O) and three chloride ions (Cl-).
When this compound undergoes hydrolysis, the water molecules will take part in the reaction. Water can act as both an acid and a base, so it can donate a proton (H+) or accept a proton (H-).
In this reaction, one of the water molecules (H2O) will act as a base and accept a proton from the [Al(H2O)6]3+ ion, resulting in the formation of a hydronium ion (H3O+). Simultaneously, the aluminum ion (Al3+) will combine with a hydroxide ion (OH-) formed from another water molecule acting as an acid.
Now, let's write the balanced ionic equation for this hydrolysis reaction:
[Al(H2O)6]3+ (aq) + H2O(l) ⇌ Al(OH)2+ (aq) + H3O+ (aq)
In this equation, (aq) indicates that the species is present in the aqueous solution, and (l) represents liquid water.
Remember that this is an equilibrium reaction, meaning it can occur in both forward and reverse directions. The double-headed arrow (⇌) is used here to depict the reversible nature of the reaction.
So, the ionic equation for the hydrolysis reaction of [Al(H2O)6]Cl3 is [Al(H2O)6]3+ (aq) + H2O(l) ⇌ Al(OH)2+ (aq) + H3O+ (aq).