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11.During an acid-base titration, 25 mL of NaOH 0.2 M were required to neutralize 20 mL of HCl.
Calculate the pH of the solution for each of the following:
12.Before the titration.
13.After adding 24.9 mL of NaOH.
14.At the equivalence point.
15.After adding 25.1 mL of NaOH.
16.The pH of the equivalence point during a certain titration is 3.5.
17.Which indicator would be adequate for this titration?
18.Which indicator would you suggest to be avoided during this titration? Justify.
19.Calculate the volume of NaOH 0.5 mol/L necessary to neutralize 300 mL of HCl 0.2 M.

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