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I have a question about acid/base problem. the problem says. What is the pH of a...

I have a question about acid/base problem.

the problem says. What is the pH of a mixture of 0.042 M of NaH2PH4 and 0.058 M of Na2HP04? Note that pKa is 6.86

So it gave the solution and said it's pH = 6.86 + log 0.058/0.042 and then it said how do we know which one is the acid or base? Just look who has more H+.

SO this is where I'm confused because the Henderson Hasselbalch equation is pH = pKa + log Base/Acid and the note above said how do we know which is the base or acid by who has the most H+. Well, isn't a solution that has MORE hydrogen ions, isn't that a base? which would be the 0.042 ?? and the one with less hydrogen ions is an acid which is 0.058 ?? But the answer flipped those 2 part of the Henderson equation. shouldn't it be pH = 6.86 + log 0.042/0.058 ???

Please let me know and explain in great detail! Thank you! and any tips that you might have to work these type of problems out. I have an exam next Friday. Thanks!

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