A student in lab titrated a diprotic weak acid with 0.100 M NaOH. To reach the equivalence point required 22.58 mL of NaOH solution. How many moles of diprotic acid were present in the titration

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Explanation:

moles H₂A in soln = moles NaOH used in titration

moles = Molarity x Volume in Liters

moles H₂A = moles NaOH used = (0.100M)(0.02258L) = 0.0023 mol H₂A

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