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I was looking at the examples on page 563-569 in the textbook and there are two different situations presents. The first is about balancing redox reactions in acidic solutions and the second is in basic solution. I don't quite understand how the acidity/basicity of the solution affects the redox reaction. No matter what I would write out the half reactions then balance.
Hi there! So the only difference between reactions in basic and acidic conditions is that blaancing reactions in a base, you would first balance it like how you would in an acid, but since you're in a basic solution now, you would add enough OH- to both sides of the equation to neutralize the H+. So, just given an equation, to tell if the reaction is in an acid or base, you would see whether there are free H+ or free OH- in the equation. Hope this helps!
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