Abstract: In this lab, a prepared solution of Potassium Hydroxide will be standardized. The solution we will be standardized by performing multiple calculations to ensure the upmost accuracy. The acid used for this titration will be KHP (C4H5KO4).
Phenolphthalein we be added to the beaker of the dissolved acid before the titration will be added. The titration will stop when the solution turns pink and the color doesn’t go away. Procedure: The procedure is stated in my notebook
Data/Observations:
Observations of all trials|
* The solid KHP dissolved in distilled water * The Solution turned stayed pink after enough KOH was added to the dissolved KHP.|
Trial 1: 1.5316g KHP
50.000 mL KOH in burette
28.000 mL KOH in beaker
Trial 2: 1.5408g KHP
50.000mL KOH in burette
31.500mL KOH in beaker
Trial 3: 1.5380g KHP
50.000mL KOH in burette
31.500mL KOH in beaker
Analysis:
0.025L × .300M1L= .0075mol KOH
KHP (C8H5KO4) molar mass: (12.0101 ×8) + (1.00794×5) + (39.0983) + (15.9994×4) = 204.2156g .0075mol KOH ×1mol KHP1mol KOH ×204.2156g KHP1mol KHP=1.5316g KHP for solid 1.5316g×1mole204.2156g=7.500×10-3moles
7.500×10-3moles.02800L=0.26787M
1.5408g×1mole204.2156g=7.545×10-3moles
7.545×10-3moles.03150L=0.23954M
1.538g×1mole204.2156g=7.532×10-3 7.532×10-3.03150
L=0.23910M .26787+.23954+.23910 =.74651 .746513=0.24884M KOH
Trial 1: 0.26787 M
The Essay on Solution Preparation And Standardization
Generally, there are two ways in preparing a solution, one is by dissolving a weighed amount of solid in a required solvent and the other is by dilution of a concentrated solution into the desired concentration. In diluting concentrated solution, the concentration of the diluted solution can be determined by standardization. To standardize a solution, we will need to perform titration. In this ...
Trial 2: 0.23954 M
Trial 3: 0.23910 M
Accepted value: 0.24884 M
Percent yield: .24884.2583×100%=96.33%
Percent error:.24884-.2583.2583×100%=3.662% Conclusion: In this experiment, a solution of KOH was standardized with titration. The KOH reacted with KHP which was dissolved in distilled water before titration. Phenolphthalein was added to the KHP solution as in indicator of the nature of the solution( acidic or basic).
After all three trials the accepted value of the molarity of KOH was .24884 M. The percent error was 3.662 % where the class accepted value was used as the theoretical value and the group value was used as the actual. The measurement of milliliters limited the amount of sig figs since the burette could only measure to the thousands place. Precision could have been improved by using a burette with more graduations on it. If overtitration had occurred, the molarity of the KOH in the solution since more molecules of KOH would be added to the solution and thus affecting the molarity.
