So we can add/subtract in chemical equations, but its can't just simply make mathematical sense, it also has to make sense in a chemistry context. So it's not much that we're adding chemicals rather we're discovering the actual reaction occurring.
However if it's an aqueous solution, these added chemicals are technically always present in the reaction solution and what we're actually doing is recognizing that some of them are actually part of the redox reaction.
Now in this case where we're adding chemicals to the equation it may just seem like we're adding chemicals out of convenience to make the math work out. Chemistry - Varsity Tutors Heat of formation (video) Thermochemistry Khan preciitate formation reaction mcat questions WebA precipitate will form if a. In redox reaction it's common to add water, H+, and OH- ion to the equations when balancing them. So since they're not participating in the reaction, subtract them is allowed because it doesn't affect the reaction if they're absent from the equation. So these are ions which are present in the reaction solution, but don't really participate in the actual reaction (they don't change as a product compared to when they were a reactant). For ionic equations like these it's possible for us to eliminate, essentially subtract out, spectator ions from an equation. Mathematically it's completely acceptable to do so, however we have to consider the actual chemical makeup of our reaction if we do so.
This reaction is represented by the molecular equation below. If we could zoom in on the contents of the reaction beaker, though, we wouldn't find actual molecules of AgNO 3 \text_4(aq) Na 2 SO 4 ( a q ) start text, N, a, end text, start subscript, 2, end subscript, start text, S, O, end text, start subscript, 4, end subscript, left parenthesis, a, q, right parenthesis.
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