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After separating the redox reactions into two half reactions, you add H2O to balance oxygens in each half reaction, and add H+ to balance hydrogen in each half reaction.
From their oxidation numbers determine the species being oxidized and reduced and then from their unbalanced equations balance the half reactions, then have the electrons in both equations cancel by multiplying both equations to make them cancel, then you can combine the equations, cancel stuff out, and voila u got the balanced redox equation.
The difference between balancing in an acidic or a basic solution is when you are balancing H. If you have an acidic solution you just add H+ to the side that needs H+. But with a basic solution you need to add H2O to the side that needs the H+ and OH- to the other side, so that the net difference is just H+
Ohh so is it only H+ that you add in acidic solutions to balance it out and use no H20? Because when I solved this problem I got 6H+ + Cl2O7(g) ---> 2ClO2- (aq) + H2O + 5e-...I got this problem partially wrong and I was wondering why I did.
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