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I think that the process is the same for both redox reactions of acidic and basic solutions. The difference will come in balancing the equation and whether you are adding H+ (acidic reactions) or OH- (basic reactions).
The main difference is how you would balance the half reactions in the redox reaction. Under acidic conditions, you would balance the hydrogen atoms by adding protons (H+). For reactions in basic conditions, you would follow the same process as if it was under acidic conditions, but you would add hydroxide ions (OH-) to balance any H+.
For acidic reactions, we have to add water to the reduction and oxidation reactions to balance out the oxygens. Do we have to add water to balance oxygens in basic conditions, or do we only add OH- to balance oxygen molecules?
the difference in acid or basic solutions is based on whether the situation calls for oxidation or reduction. In the case of reduction, the product will include a H+ but for oxidation it is OH-. the acronym OILRIG helps. oxidation is losing and reduction is gaining
The main difference comes from how you balance the equation. For basic solutions, you would balance out the equation by adding hydroxide ions (OH-). For acidic solutions, you would balance out the equation by adding protons (H+).
Shanzey wrote:For acidic reactions, we have to add water to the reduction and oxidation reactions to balance out the oxygens. Do we have to add water to balance oxygens in basic conditions, or do we only add OH- to balance oxygen molecules?
You use water to balance in both acidic and basic solutions. In both, you use water to balance the oxygens on each side. The difference:
in acidic solutions, you balance hydrogens with protons (H+)
in basic solutions, you balance hydrogens with water as well. If you need to add 2 hydrogens to the left side of a half reaction, you add 2 waters to the left and add 2 hydroxides (OH-) to the right. This cancels out one of the 2 hydrogens in a water molecule so that there is are 2 net hydrogens on the left.
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