A 20.00 mL sample of H3PO4 is titrated to a phenolphthalein end point with 18.67 mL of NaOH. If the phenolphthalein color change occurs at the second eqivalence point, whats the molarity of the acid? (please show the work so I can learn it)
A 0.542 g sample of an unknown monoprotic weak acid requires 28.67 mL of 0.1093 M NaOH for neutralization. What is the molar mass of the acid?
When I did it I got 173 g/mol, but Im uncertain.
What is the pH at the equivalence point of a titration of 0.20 M formic acid with 0.20 M NaOH? 11) (Ka for formic acid = 1.8 x 10-4) I'm not sure how to get this without the mL.