A laboratory technician titrates 25.00 mL of an aqueous solution of a monoprotic weak…
CHEMISTRY · Multi-part · A Level · Chemistry · Acids and bases · Acids and bases
Problem
A laboratory technician titrates 25.00 mL of an aqueous solution of a monoprotic weak acid HA with 0.150 M NaOH. The equivalence point is reached after 23.80 mL of the base has been delivered.
Answer the following questions about this experiment.
(a) Identify the titrant and the analyte in this procedure.
(b) Describe, in terms of chemical amounts, what is true about the quantities of HA and NaOH present at the equivalence point.
(c) Explain why knowledge of the volume and molarity of the NaOH solution is sufficient to determine the number of moles of HA originally present.
(d) The technician accidentally allows a few excess drops of NaOH to enter the analyte after the equivalence point has been signaled. Explain qualitatively how this mistake would affect the calculated molarity of the acid if the excess base is not accounted for.