0.1276 of a monoprotic acid (molar mass 110g/mol) was dissolved in 25ml of water.The pH of the solution was found to be 5.87 after the addition of 10.0ml of 0.0633 M NaOH.The Ka of acid is.......................

Answer 1

HA + NaOH ==> NaA + H2O

Calculate moles HA from the data given. Calculate moles NaOH, determine moles NaA formed and moles HA remaining, plug into Henderson-Hasselbalch equation and solve for pKa, then Ka. Post your work if you get stuck.