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 solut ion. How many moles of diprotic acid were present in the titration
2 answers:
Answer:
see below
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
Answer:
0.0023 moles of H₂A
Explanation:
moles H₂A in soln = moles NaOH used in titration
moles = Molarity x Volume in Liters
moles H₂A = moles NaOH used
Which is = (0.100M)(0.02258L) = 0.0023 mol H₂A
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