1.What are the significant regions in the titration curve? Relate the characteristics of each region to the pH results obtained.
-There are four significant regions in each titration curve, namely the initial, pre-equivalence, equivalence, and post-equivalence points. These points are named according to its position relative to the equivalence point. The base titration Chemistry Formal Lab Writeup By A.Mm">equivalence point signifies the volume of titrant at which the solution becomes neutral. This is represented in the graph as the drastic change in pH, first with a sudden increase and a sudden decrease of pH. At the initial point, no titrant has been added yet and the solution’s pH equates to the number of H+ ions originally present in the analyte. At the pre-equivalence point, the titrant is now added. For this experiment, NaOH, a strong base, was added to KHP, a weak acid. With the addition of a strong base to a weak acid, a phenomenon similar to that of buffers occurs, and the solution initially resists drastic pH changes as backed up by the results of the experiment. At the post-equivalence point, since the solution was already neutralized and excess NaOH is still added, the solution’s pH further increases.
The Essay on Solution Preparation And Standardization 2
All chemists must know how to prepare solutions of varying concentrations because many reactions in quantitative analysis take place in an aqueous medium. In this experiment, solutions were made using 2 methods. The first method used was dissolution. A specific mass of solid was dissolved in a specific volume of distilled water. The second method was dilution. A specific volume of a certain ...
2.Why is continuous stirring important in potentiometric titration? -Continuous stirring allows for the formation of incremental hotspots, which allows for a higher concentration of the titrant in a localized area compared to the fluid around it. This allows for faster endpoints.
3.Why should the increments of addition be narrowed down as the titration approaches the equivalence point? -Because as the titration nears the equivalence point, the changes in pH become larger, specifically at the equivalence point. The most drastic change happens at this point and the continuous addition of 1mL increments will not accurately show at which volume the equivalence point occurred at.
4.Why is potentiometry a suitable method in determining pKa of weak acids? -With potentiometric titrations, the potential between the electrodes and the volume of titrant is related. Using this method, the amount of titrant used for weak acids would be the same as that used for strong acids since it is the number of protons or H+ ions, measured through the pH, which determines the equivalence point. With normal titrations of strong acids and bases, since H+ completely dissociates, similar concentrations with a weak acid and strong base titration would not be the same since weak acids do not dissociate completely. Another advantage of potentiometric titration is the fact that indicators are not used, therefore human error due to failure of recognition of color change may be avoided.
5.Discuss possible reasons behind the discrepancies (if any) in the experimental and theoretical pKa values. -Human errors may have affected the results, such as miscalculations, overtitrations and failure of determination of the right pH value since the pH meter tends to fluctuate. Another source of error could be from the pH meter apparatus itself, particularly the electrodes since the classroom’s conditions are not perfect. The failure to rinse the electrodes may result to drastic changes as well. Another error may result from the failure in accuracy of the analytical balance since it has been used for several years prior.
The Term Paper on The Titration Of Acids And Bases
Purpose This experiment will allow you to gain practical experience in the preparing standard solutions, using a pipette and a buret, and performing standard titrations. You will use this experience to experimentally determine the concentration of acetic acid in an unknown solution. There are three parts to this experiment, they are 1. Preparation a standard solution of oxalic acid (~0.07 M) 2. ...
6.What are the possible sources of errors and their effect on the calculated parameters? Rationalize. -One of the members of the group accidentally touched the magnetic stirrer therefore contaminating the whole set-up. Since it cannot be estimated whether the action done would result in the increase/decrease in acidity, the effect is indeterminate. Other possible sources of error include standardization error, such as the failure of correctly measuring the final and initial values which results to drastic changes. Another source of error may be brought out from the preparation of the electrodes, such as failure to recalibrate the electrode once put in a new test solution. This will result in inaccurate results since the previous pH reading still affects the pH meter at the moment it touches the new solution.
