What is the total ionic and net ionic equation for this aqueous reaction?:
Sr(OH)2(aq) + HClO2 (aq)
-I wrote the molecular as:
Sr(OH)2 (aq) + HClO2 (aq) ---> SrClO2 (aq) + H20 (l)
-Is the Total Ionic:
Sr2+ (aq) + 2OH- (aq) + H+ (aq) + 2ClO- (aq) ---> Sr2+ (aq) + 2ClO-(aq) + H2O (l)
The molecular should be written:
Sr(OH)2 (aq) + HClO2 (aq) --> Sr(ClO2)2 (aq) + 2H2O (l)
The complete ionic equation would then be:
Sr2+ (aq) + 2OH- (aq) + 2H+ (aq) + 2ClO2-(aq) --> Sr2+ (aq) + 2OH- (aq) + 2ClO2-(aq) + 2H2O (l)
You were close but chlorite ion is ClO2- instead of 2ClO- and since strontium has a 2+ charge, there would have to be two chlorite ions.
Also the net ionic equation is 2OH- (aq) + 2H+ (aq) --> 2H2O (l)
I hope this helps!
If you need any further help, khan academy has some good article. Just look up "complete and net ionic equations".
The molecular equation you wrote is correct:
Sr(OH)2(aq) + HClO2(aq) ---> SrClO2(aq) + H2O(l)
To write the total ionic equation, you need to split all the soluble ionic compounds into their respective ions:
Sr2+(aq) + 2OH-(aq) + H+(aq) + ClO2-(aq) ---> Sr2+(aq) + ClO2-(aq) + H2O(l)
Note that the Sr2+ ion remains unchanged on both sides of the equation, and the ClO2- ion remains unchanged as well.
Finally, to write the net ionic equation, you need to remove any spectator ions that appear on both sides of the equation:
2OH-(aq) + H+(aq) ---> H2O(l)
So, the net ionic equation for this reaction is:
2OH-(aq) + H+(aq) ---> H2O(l)
To determine the total ionic and net ionic equation for the given aqueous reaction, you need to first write the complete balanced molecular equation.
The balanced molecular equation you wrote is correct:
Sr(OH)2(aq) + HClO2(aq) → SrClO2(aq) + H2O(l)
Now, to write the total ionic equation, you need to dissociate all the soluble ionic compounds into their respective ions. In this case, only Sr(OH)2 is soluble, so it will be dissociated into Sr2+ and 2OH- ions:
Sr2+(aq) + 2OH-(aq) + H+(aq) + ClO2-(aq) → Sr2+(aq) + ClO2-(aq) + H2O(l)
As you can see, Sr2+ and ClO2- ions appear on both sides of the equation. These are called spectator ions and do not participate in the actual reaction. To write the net ionic equation, you can remove the spectator ions from the equation:
2OH-(aq) + H+(aq) → H2O(l)
This is the net ionic equation for the given reaction, representing the actual species involved in the chemical transformation.