Use solubility rules to write the balanced molecular, complete ionic, and net ionic equations for the aqueous reaction between BaI2 and Hg(NO3)2. Include phase subscripts on all substances.
I got to the part where you switch the elements
Ba(NO3)2 +HgI2 I don't know where to go from there?
Thanks for telling me where you're stuck but why didn't you show what you had done so I could check it first. The molecular equation is as follows:
BaI2(aq) + Hg(NO3)2(aq) ==> HgI2(s) + Ba(NO3)2(aq)
Now change that to a complete ionic equation. The rules are that if it dissolves and ionizes write it as ions, if gas or covalent write as molecule. Write insoluble materials as molecule.
Ba^2+(aq) + 2I^-(aq) + Hg^2+(aq) + 2NO3^-(aq) ==> HgI2(s) + Ba^2+(aq) + 2NO3^-(aq)
Now cancel those ions that occur on both sides. So can cancel Ba^2+ on left and right as well as 2NO3^- on left and right. That leaves the net ionic equation.
2I^-(aq) + Hg^2+(aq) ==> HgI2(s)
To write the balanced molecular equation, complete ionic equation, and net ionic equation for the reaction between BaI2 and Hg(NO3)2, you need to use solubility rules to determine the states of each compound in the reaction.
First, let's start by writing the balanced molecular equation by simply switching the elements, as you did so far:
Ba(NO3)2 + HgI2
To determine the states of each compound, you need to refer to the solubility rules. Based on the rules, nitrates (NO3-) and most iodides (I-) are soluble in water, so both Ba(NO3)2 and HgI2 are aqueous (aq).
Now, let's write the balanced molecular equation with the correct phase subscripts:
Ba(NO3)2(aq) + HgI2(aq)
To write the complete ionic equation, you need to separate each compound into its respective ions. In this case, Ba(NO3)2 dissociates into Ba^2+ and 2 NO3-, while HgI2 dissociates into Hg^2+ and 2 I-.
The complete ionic equation becomes:
Ba^2+(aq) + 2 NO3-(aq) + Hg^2+(aq) + 2 I-(aq)
Finally, to write the net ionic equation, you need to eliminate the spectator ions (ions that appear on both sides of the equation without undergoing any change). In this case, the nitrate ions (NO3-) are spectator ions.
The net ionic equation becomes:
Ba^2+(aq) + Hg^2+(aq) + 2 I-(aq)
And there you have it! The balanced molecular, complete ionic, and net ionic equations for the reaction between BaI2 and Hg(NO3)2.