If a strong acid is titrated with a particular weak base, the pH of the equivalence point is known to occur at a pH ~3.7. Using your laboratory manual decide which of the following is the most suitable indicator for this titration.

0.5 mL of 0.014 M salicylic acid is placed in a 50 mL volumetric flask and made up to the mark with distilled water. What is the resulting salicylic acid concentration?

The preparation of standard solutions is a very important skill that requires great care. Which of the following indicates the correct final position of the meniscus (red line) of an aqueous solution in a volumetric flask that has been filled correctly?

What is the molarity of Fe(NO₃)₃ in a 2.14% w/v Fe(NO₃)₃ solution? (Molar Mass of Fe(NO₃)₃ = 241.88).

Hint: X % w/v = Xg/100mL = X x 10 g /L

Molarity = moles / L so divide  X x 10 g by molar mass will give you moles per liter (M).

Where should the plastic pipettes and the gloves be placed during your clean up?

The main reason for preparing the standard solutions containing various concentrations of salicylic acid and Fe(NO₃)₃ is?

When you have finished where do you tip the aqueous solutions in the volumetric flasks?

At what wavelength will you determine the absorption of your standard solutions and your samples?

In Experiment 10, the amount of unreacted salicylic acid present in a prepared sample of Aspirin® is determined. Fe(III) ions are added to a solution of the Aspirin® sample. If salicylic acid is present the solution will turn red/violet in colour. The coloured compound that forms on addition of Fe(III) is called ........?

To measure the absorbance of the standard solutions you must transfer them to a cuvette. Which of the following statements is INCORRECT about this transfer process?