consider the titration of a 50.00 ml solution of 0.10 m hno2 with 0.10 m koh. determine the ph after 10.00 ml of koh is added

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09-12-2022
Chemistry

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consider the titration of a 50.00 ml solution of 0.10 m hno2 with 0.10 m koh. determine the ph after 10.00 ml of koh is added

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contexto1220 contexto1220 · Answer 1 · 2022-12-15T19:41:43+01:00

The pH is 3.35 after 10.00 ml of koh is added when the convenient formula for determining the pH of a buffer consisting of a weak acid and its conjugate base is the Henderson-Hasselbalch formula.

Titrate 50.00 mL 0.10 M HNO(nitric acid, Ka = 4.5 × 10−4) with 0.10 M KOH solution. What is the pH value in the titration flask after adding 25.00 ml of KOH solution.

The balanced equation for the reaction is shown below.HNO2+KOH →KNO2+H2O

Start by determining the amount needed to reach the equivalence point. 0.050 l × 0.10 mol HNO2 1 l × 1 mol KOH1 mol HNO2 × 1 l 0.10 mol KOH × 1000 ml1 = 50 ml = Veq

Titration is in progress when 25 ml of titrant has been added. pKa at pH = 12 veq = 25 ml. Pka = - log4.5 x 10therefore the pH is 3.35 pH.