When designing a results table for an acid-base titration, it’s essential to ensure that the table captures all necessary data clearly and systematically.
For example: Given the titration of sulfuric acid with sodium hydroxide, using phenolphthalein, here’s a suggested format for a results table:

Titration Results Table: Sulfuric Acid (analyte) vs. Sodium Hydroxide (titrant).

Key Components:

1. Run: Indicates the number of the trial. Multiple trials are conducted to ensure accuracy and consistency in the results.
   A so-called ‘rough run’ is carried out first. It is done quickly to get a ‘ball-park’ titre. This titre is not used for the average titre!

2. Initial Burette Reading: The starting volume reading on the burette before the titration begins.
   All burette reading should be given to 1 decimal place, including zero, as 0.0.

3. Final Burette Reading: The volume reading on the burette after the endpoint has been reached.

4. Volume of NaOH Used: This is known as the TITRE and is calculated by subtracting the Initial Burette Reading from the Final Burette Reading.
   This gives the exact volume of sodium hydroxide required to neutralize the sulfuric acid in that run.

5. Average Volume of NaOH: After all trials are completed, calculate the average volume of NaOH used in the titrations.
   Only concordant results can be used to work out the average. Runs must be carried out until concordant results are achieved.
   To be concordant, the titres must be within 0.20 cm³.
   This average is often more accurate than any single measurement and is used in calculations.

6. Concentration of H₂SO₄: After determining the average volume of sodium hydroxide required, you can calculate the concentration of the sulfuric acid using the stoichiometric relationship between sodium hydroxide and sulfuric acid.
   2NaOH _(aq)    +   H₂SO_{4 (aq)} →    Na₂SO_{4 (aq)}    +   H₂O _(l)

   The moles of NaOH needed is worked out using the formula n = c.v. That is,  moles = concentration x volume (dm³)
   In the above case: moles of NaOH = 0.871 x (22.75/1000) = 0.01982 mol.
   Moles of sulfuric acid present inthe 25.0 cm3 = half the number of moles of NaOH used (from the balanced equation)
   = 0.01982/2 = 0.00991 mol of H₂SO₄ in 25 cm³.
   Finally the concentration of the sulfuric acid can be determined using the same formula n = c.v
   c = n/v or concentration = moles/volume (dm³ ) = 0.00991/0.025 = 0.396 moldm^-3.

Remember:

• Always record measurements to the appropriate number of decimal places, usually two decimal places for titration volumes.
• It’s important to conduct multiple trials to ensure consistency in your results. Outliers, if any, can be identified and possibly repeated.

Once you have filled the table with your results, you can use the average volume of sodium hydroxide required in the calculations to determine the concentration of the sulfuric acid.