I'm reading the instructions for a lab, and I'm becoming more convinced that whoever wrote it had no idea what they were talking about. Maybe some of you could shed some light on this.
This was step one:
1. Take two beakers. In the first, prepare a solution of 76% sulfuric
acid, 23% nitric acid, and 1% water. In the other beaker, prepare
another solution of 57% nitric acid and 43% sulfuric acid (percentages
are on a weight ratio rather than volume).
Ok, I'm sure you see the problem with this. When someone says a solution is 76% sulfuric acid by weight, they mean that for every 100 g of the solution, 76 of those grams are taken up by the H2SO4. With the solution density of 76% sulfuric acid being around 1.5 g/mL, I calculated this to be around 12 mol/L sulfuric acid. The problem is that it claims there is only 1% water by weight. A solution like that would be impossible to make, and 12 mol/L is already incredibly acidic, so I'm going to have to assume that it refers to pouring 76% by weight of a sulfuric acid solution of unknown concentration into 23% by weight of a nitric acid solution of unknown concentration and one percent by weight water. If that is the case (and it's the only thing I can think would be reasonable), then it is entirely useless, as it gives absolutely no indication to the concentrations of these solutions. Thanks a lot.