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A chemist titrates 90.0 mL of a 0.5705 M carbonic acid (H,CO,) solution with 0.6274 M...


A chemist titrates 90.0 mL of a 0.5705 M carbonic acid (H,CO,) solution with 0.6274 M KOH solution at 25 °C. Calculate the pH
A chemist titrates 90.0 mL of a 0.5705 M carbonic acid (H,CO,) solution with 0.6274 M KOH solution at 25 °C. Calculate the pH at equivalence. The pk of carbonic acid is 3.60. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. DH-
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Given data : Carbonic acid HaCo3 = 0.5705M Chemist titrcut le =90.0 ml KOH 0.627M Carbonicacid = 3.60 H₂CO3 = 90 ml of 0.5705Total volume = 90 + 81.84 =171.80ml Io.AL Concentration - C = number of moles volume 0.5135 0:171 = 3.00 M. AL Ewilance point

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