# Balancing Redox Equations

I was taught to balance redox equations with acid/base considerations. Instead of arbitrarily adding $\ce{H^+}$ and $\ce{HO^-}$ ions and memorizing separate rules for acidic and basic solutions, I was taught simply to keep these four things in mind:

1) Charge must be conserved.

2) Mass is similarly conserved.

3) Do what's thermodynamically more favorable. For example, in strongly basic solution, $\ce{O^2-}$ oxygen ions come from not hydronium ion (because that doesn't exist in significant quantity in basic solution) and not from water (because that requires heterolytic clevage of 2 $\ce{H-O}$ bonds but instead $\ce{HO^-}$ because that only requires clevage of only one $\ce{H-O}$ bond.

4) Strongest base reacts with strongest acid.

On the other hand, here's a gem from Chem Wiki by UC Davis:

My question is:

1) How come I've never seen my professor's method mentioned anywhere? I've Googled, looked at scholarly papers; looked in advanced analytical textbooks, etc.

2) How were you taught?

3) Which way do you think is more advantageous?

1) How come I've never seen my professor's method mentioned anywhere? I've Googled, looked at scholarly papers; looked in advanced analytical textbooks, etc.

It is entirely possible that no one has published that approach! It is certainly not common in introductory chemistry textbooks.

2) How were you taught?

I was taught (and currently teach) the "standard" algorithm you found on the Chem Wiki.

3) Which way do you think is more advantageous?