a student peforms a titration, titrating 25.00 ml of a weak monoprotic acid, ha, with a 1.26 m solution of naoh. they collect data, plot a titration curve and determine the values given in the below table.ml NaOH added pHHalf-way Point 18.34 4.06Equivalence point 36.68 8.84How many moles of NaOH have been added at the equivalence point?mol. What is the total volume of the solution at the equivalence point?mL During the titration the following reaction occurs
HA + NaOH ⇒ NaA + H2O
What is the concentration of A- (the conjugate base of the weak acid) at the equivalence point?
M
Use [A-] and the pH at the equivalence point to estimate Ka of the weak acid (this is the hard way of estimating Ka)