Can acids contain OH-? [closed]








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Given that a solution contains $\ce{OH-}$ ions can we sufficiently determine the substance is a base? From my understanding, an acid may still contain $\ce{OH-}$ ions. However, the concentration of $\ce{H+}$ ions must exceed this. Is this correct?




An acid can have some $\ce{OH-}$ ions, as well as $\ce{H+}$. It is the **relative ratio** that determines if the substance is acid or alkaline. Think of it as mismatching socks, where you must pair 10,000,000 red with 10,000,001 blue socks. There's one blue left over, so blue wins. (Hmm... in that analogy, think red and blue litmus, and there's one more $\ce{OH-}$ ion.)


Also, a [zwitterion](https://en.wikipedia.org/wiki/Zwitterion) has both acidic and basic groups, and one can predominate over another, depending on the the pH.


[Amino acids](https://www.chemguide.co.uk/organicprops/aminoacids/acidbase.html) and [sulfamic acid](https://en.wikipedia.org/wiki/Sulfamic_acid) are two examples. Some amino "acids", such as [arginine](https://en.wikipedia.org/wiki/Arginine), are more basic, while [aspartic acid](https://en.wikipedia.org/wiki/Aspartic_acid) is more acidic. [The bumbling biochemist](https://thebumblingbiochemist.com/365-days-of-science/arginine-basic-vs-acidic-amino-acids/) offers a more complete explanation of the behavior of zwitterions.


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