Those of us old enough to remember the car batteries that weren't sealed also remember the holes left in our clothes and skin from the acid that got on us. Why would acid in anything else be different?
"Why would acid in anything else be different?"
The holes referenced are a property of being corrosive, not acidic. Both strong acids and strong bases can be corrosive.
To the second point, acids are not created equal. Some acids are very strong (like hydrochloric/muriatic or sulfuric/battery acid) whereas other acids are weak, like Phosphoric acid or citric acid. You drink phosphoric acid in your pop, but it's clearly not burning holes in you from the inside out, nor is molasses.
For only those that are actually interested, I post a link here that shows strengths of various acids. The pKa is a value that tells how strong an acid is; it is inversely related to the Ka of an acid, which is its dissociation constant. An acid that readily dissociates and donates hydrogen ions is a strong acid, whereas an acid that does not dissociate as easily and likes to hold on to its hydrogen ions will have a lower dissociation constant. In other words, one is charitable whereas the other is not. That's a lot of boring background most of you will never need to ever care about. But it puts these numbers in the link in context. The lower the pKa, the stronger the acid. pKa values less than 0 are very strong, while those above 0 get progressively weaker as the number gets higher. Inversely, the higher the Ka, the stronger the acid.
So look at where HCl and sulfuric (H2SO4) sit on the chart, vs phosphoric acid H2PO4.
It's also interesting to see where other acids sit as well.