To write the net ionic equation, first write the total (complete) ionic equation, remove ions that appear on both sides of the equation, the net ionic equation is what is left. Try that on this one. You should be left with H^+(aq) + OH^-(aq) ==> H2O(l)
I included the phases although your question didn't ask to do that.
The balanced net ionic equation for the neutralization reaction involving equal molar amounts of HNO3 and KOH is ________. Express your answer as a chemical equation. Identify all of the phases in your answer. I thought it was
Consider the reaction in aqueous solution: 6 HCl + 2 KMnO4 + 5 H2O2 ---> 5 O2 + 2 MnCl2 + 2 KCl + 8 H2O 1.) Write the total ionic equation. 2.) Write the net ionic equation. 3.) For each species (molecule or ion) in the net
Complete and balance each of the following equations for gas-evolutions. Express answer as a chemical equation. Identify all the phases in your answer. HCl(aq)+K2SO3(aq)--> HCl(aq)+KHCO3(aq)--> HC2H3O2(aq)+NaHSO3(aq)-->
We are determining the molarity of HCl by titration of HCl. What would be the complete equation and the net ionic equation? THanks What are you titrating it with? Won't that make a difference in the equation we write? It's
Write reactions showing how each of the following buffers would neutralize added HCl. HF and NaF Express your answer as a balanced chemical equation. Identify all of the phases in your answer. HC2H3O2 and KC2H3O2 Express your