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 pH Half-way Point 17.99 3.90 Equivalence point 35.98 8.76   How 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)     Use the pH at the half-way point to estimate Ka of the weak acid (this is the easier way)

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Q: point in the titration curve below is a sent? Volume titrant added (mL) nt A nt B B

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.