What is the net ionic equation of AlPO4(s) dissolved in H3O+(aq)
To determine the net ionic equation for the dissolution of AlPO4(s) in H3O+(aq), we need to first write the balanced equation for the dissociation of AlPO4 in water.
The chemical formula for aluminum phosphate is AlPO4, and when it dissolves in water, it can break apart into its constituent ions. The balanced chemical equation for the dissolution of AlPO4 in water is:
AlPO4(s) + 3H3O+(aq) → Al3+(aq) + PO4^(3-)(aq) + 3H2O(l)
In this equation, AlPO4 (s) is the solid aluminum phosphate, and H3O+(aq) represents the hydronium ions in water. Al3+ is the aluminum ion, PO4^(3-) is the phosphate ion, and H2O(l) represents water molecules.
Now, to obtain the net ionic equation, we need to exclude the spectator ions, which are the ions that do not undergo any change during the reaction. In this case, the hydronium ions (H3O+) and water molecules (H2O) act as spectator ions.
The net ionic equation for the dissolution of AlPO4(s) in H3O+(aq) can be written as:
AlPO4(s) → Al3+(aq) + PO4^(3-)(aq)
This equation simply shows the solid aluminum phosphate breaking apart into its constituent ions.
Hmmm. Aluminum phosphate tribasic DISSOLVED? This is firebrick, insoluble in water, very slighty soluble in HCl or HNO3. I am wondering if this is a trick question.
So the question is, I suppose, what is the net ionic question if the firebrick is dissolved in an acid.
IF it is, then Al(PO4)>>Al+3 + PO4-3
Aluminum hydroxide is soluble in acidic solutions as ions, so there is no precipate.
My feeling is this is some trick question.