Calculations

1. Determine volume of titrant added. This is determined by subtracting the

final volume of a titration from the initial volume of the titration.

2. Determine moles of titrant added. This is determined by multiplying the

molarity of the titrant by the volume in liters of the titrant found in the

previous calculation.

3. Determine the moles of analyte in the Erlenmeyer flask. This is

determined by using the moles of titrant added in the previous calculation and

multiplying it by the appropriate stoichiometric ratio using the balanced

equation. You need to write the balanced equations to appropriately answer

this question. The products of the reaction in Part 2 are H₂O and NaCl. The

products of the reaction in Part 3 are H₂O and Na₂SO₄.

4. Determine the molarity of the analyte that was titrated. This is

determined by taking the moles of analyte in the previous calculation and

dividing it by the volume in liters of analyte pipetted into the Erlenmeyer flask.

Pre-Lab Questions

1. How do you avoid parallax errors when reading scientific glassware?

2. What is the role of an indicator in a titration?

3. How many decimal places should be included in your reading of the buret?

4. What are the balanced chemical equations for HCl reacting with NaOH and

H₂SO₄ reacting with NaOH?

5. In the part 3 titration if the initial volume reading is 1.25 mL and the final

volume reading is 23.81 mL, what is the concentration of H₂SO₄ in the

solution? Remember that the molarity of NaOH is 0.100 M and that you need

to make sure to consult the balanced equation. 

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