Question

Solid aluminum hydroxide reacts with a solution of hydrobromic acid. write a balanced molecular equation and a balanced net ionic equation, including the states of each species.

Answer 1

Aluminium hydroxide base [Al(OH)₃] reacts with the HBr (hydrobromic acid) to produce AlBr₃ (aluminium bromide) and water (H₂O).

The molecular equation showing the reaction between the Ba(OH₂) and HBr is as follows:

Al (OH)₃ (s) + 3HBr (aq) → AlBr₃ (aq) + 3H₂O (l)

Total ionic equation:

All the aqueous solutions dissociate into their composite ions. As Al(OH)₃ is solid, so it will remain as it is in the solution.

Al(OH)₃ (s) + 3H⁺ (aq) + 3Br⁻ (aq) → Al³⁺ (aq) + 3Br⁻ (aq) + 3 H2O (l)

On cancelling the ions, which are common on both the sides of the equation the net ionic equation is obtained.

Net ionic equation:

Al(OH)₃ (s) + 3H⁺ (aq) → Al³⁺ (aq) + 3H₂O (l)

Answer 2

To find the balanced molecular equation, we need to find the symbols for each element and their charges and then balanced the equation. This comes out to: Al(OH)3(aq) + 3HBR(aq) ---> AlBr3(aq) + 3H2O(l) The net ionic equation is adding the charges and separating them into basic components. Al3+ + 3OH- + 3H+ + 3BR- --> Al3+ + 3Br + H3O+ We can cancel out the aluminum and bromine to get: 3OH-(aq) + 3H+(aq) --> 3H2O(l)