# The purpose of this experiment is to determine the concentration of a solution of sodium hydroxide by titration against a standard solution of potassium hydrogen phthalate.

by crysisfreak69 (student)

Aim

The purpose of this experiment is to determine the concentration of a solution of sodium hydroxide by titration against a standard solution of  potassium hydrogen phthalate.

Qualitative Data

• Sodium hydroxide solution is colorless before titration
• HCL is colorless before titration
• The end result of the solution is slight pink
• When the solution is off-shot the solution has a deep purple color
• before reaching the endpoint the solution turns pink and then fades away as we swirl the conical flask
• the color of phenolphthalein is colorless before titration
• the color of phenolphthalein is slight pink after titration
• a drop of the solution is left behind in the pipette
• ideal color of the solution is fade pink

Quantitative Data

Table below shows the various volumes of chemicals that where used from their respected apparatus

Table below shows the number of trials taken from the NaOH solution from the burette and the intial and final values of the solution titrated

Table below shows the  chemicals used and their concentration

Calculation

Table below shows the number of trials taken from the NaOH solution from the burette and the intial and final values of the solution titrated along with the volumes titrated

Volume of burette solution used for titration = Final reading – Initial Reading

Mean volume of solution = Sum of the values of the volume/number of observations

= 25.61+25.61+25.4/3

=25.54 ml (±0.02ml)

Error calculation

Volume of the acid = (inaccuracy/volume) x100

= (0.06/25)x100

=0.24%

= ± 0.06ml

Concentration of acid = (inaccuracy of moles+ inaccuracy of volume of solution)

= 0.04%+0.24%                     (inaccuracy is obtained from the previous experiment)

= 0.28%

= ± 0.0027286M

Volume of NaOH     ...