Does anyone know a conversion of the molarity of an acid to it's pH or a place where there is a table with this information?

If it's a monoprotic strong acid, pH is just -log(molarity). If it's a weak acid, you'll have to look up its Ka to find [H+] and calculate pH as -log[H+].

What molarity or acid would constitute a weak acid in this equation? I have 3 and 6 mol nitric, hydrochloric, and sulfuric and I may need to reduce the molarity in some cases to get the desired pH.

All of those are strong acids. Sulfuric is diprotic so the dissociation of the second hydrogen has a Ka, but its works out to not being too important when calculating pH in practical applications.

 

Molarity doesn't determine how weak or strong an acid is, but the molarity of a strong acid does affect pH. Meaning, the more of a strong acid per liter of water, the lower the pH. A strong acid is a strong acid because it gives up it's proton readily in aqueous solution. Basically, as much HCl as you put into solution is as much H+ you're going to get.

 

A weak acid doesn't give up this proton as readily. Meaning, you're going to get less H+ than as much you put in.

 

I hope that helps.

 

Also, note that you have 3 and 6 moles of these acids. You're going to need molarity which is the moles/liters of water.

Ok thanks. It helps a lot.