Half-Acidic




Click below to see the other techniques for balancing redox equations. 


Half-Acidic

Balancing Redox Equations for Reactions in Acidic Conditions Using the Half-reaction Method

Redox reactions are commonly run in acidic solution, in which case the reaction equations often include H2O(l) and H+(aq). This page will show you how to write balanced equations for such reactions even when you do not know whether the H2O(l) and H+(aq) are reactants or products. For example, you may know that dichromate ions, Cr2O72-, react with nitrous acid molecules, HNO2, in acidic conditions to form chromium ions, Cr3+, and nitrate ions, NO3-. Because the reaction requires acidic conditions, you assume that H2O(l) and H+(aq) participate in some way, but you do not know whether they are reactants or products, and you do not know the coefficients for the reactants and products. An unbalanced equation for this reaction might be written

      Cr2O72-(aq) + HNO2(aq)  -->  Cr3+(aq) + NO3-(aq)   (acidic)

In order to balance equations of this type, we need a special technique called the half-reaction method or the ion-electron method

Click here to see the sample study sheet for this method.

Click here to see an example.

Click here to see an exercise that will allow you to try this task yourself. 

Return to the Balancing Redox Equations Page.

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