Write molecular, ionic, and net ionic equations.
HIO2(aq) + Ba(OH)2(aq) -->
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To write the molecular, ionic, and net ionic equations for the reaction between HIO2(aq) and Ba(OH)2(aq), follow these steps:
Step 1: Write the balanced molecular equation
The molecular equation shows all reactants and products in their molecular forms, without indicating their ionic nature or interactions.
HIO2(aq) + Ba(OH)2(aq) → Ba(IO2)2(aq) + 2H2O(l)
Step 2: Split the molecules into their respective ions
Next, we break apart the ionic compounds into their constituent ions. Only compounds that are soluble and dissociate in water will be separated into ions.
HIO2(aq) splits into H+(aq) and IO2-(aq).
Ba(OH)2(aq) splits into Ba2+(aq) and 2OH-(aq).
Ba(IO2)2(aq) remains as a complete molecule, as it is not a strong electrolyte.
The ionic equation is as follows:
H+(aq) + IO2-(aq) + Ba2+(aq) + 2OH-(aq) → Ba(IO2)2(aq) + 2H2O(l)
Step 3: Write the net ionic equation
The net ionic equation shows only the species involved in the chemical reaction. It excludes spectator ions - those ions that appear unchanged on both sides of the equation.
In this case, the spectator ions are the H+ and OH- ions. They appear on both the left and right sides of the equation but do not participate in the reaction. Therefore, they are not included in the net ionic equation.
The net ionic equation for this reaction is:
IO2-(aq) + Ba2+(aq) → Ba(IO2)2(aq)
This equation specifically represents the ions involved in the reaction and excludes any spectator ions.