Practice AP Chemistry Unit 4.6 questions on reading titration volumes, using equivalence-point mole ratios, calculating unknown concentrations, and evaluating experimental choices.
A student dissolved a 0.139 g sample of oxalic acid, , in water in an Erlenmeyer flask. Then the student titrated the solution in the flask with a solution of , which has a dark purple color. The balanced chemical equation for the reaction that occurred during the titration is shown above.
The student used a 50.0 mL buret to add the to the until a faint lavender color was observed in the flask, an indication that the end point of the titration had been reached. The initial and final volume readings of the solution in the buret are shown below. Write down the initial reading and the final reading and use them to determine the volume of that was added during the titration.
The student proposes to perform another titration using a 0.139 g sample of , but this time using in the buret. Would this titrant concentration be a reasonable choice to use if the student followed the same procedure and used the same equipment as before? Justify your response.