The objective of this experiment were: Titration was used to study acid-base neutralization reaction quantitatively. In acid-base titration experiment, a solution of accurately KHP concentration was added gradually to another solution of NaOH concentration until the chemical reaction between the two solutions were completed. The equivalence point was the point at which the acid was completely reacted with or neutralized by the base.
To determine the molarity of an NaOH solution by titrating it with Oxalic acid a primary standard. Oxalic acid is a primary standard.
It can therefore be used to determine the molarity of an NaOH solution. Oxalic acid is a weak acid. Therefore this is an example of a weak acid-strong alkali titration and the indicator is phenolphthalein.
Ensure that you wash your hands after the experiment and especially before eating anything. In addition oxalic acid is not very soluble and will require the use of a glass rod to dissolve it.
Ensure that you do not add more then the required volume of water in this process. With the aid of an electronic balance weigh out 1.
Dissolve the Oxalic acid in a beaker with distilled water and with the aid of a glass rod. When the Oxalic acid has completely dissolved then transfer the solution into a volumetric flask and make a ml solution using distilled water.
Transfer this solution into the 50ml burette 5. Shake the volumetric flask thoroughly to make sure the solution is homogeneous.
With the aid of a 25ml pipette measure out exactly 25ml of the 0. Add drops of Phenolphthalein indicator. Titrate the solution until the indictor color changes from purple to color less.
Titrate to 1-drop accuracy 9. Repeat to obtain 3 concordant results. The results indicate that the concentration of our solution of NaOH is.
However we know that the value of the NaOH solution is about. Therefore we can work out the error in our results. The concentration of NaOH solution from my results turns out to be 0.
The error analysis indicated that the limitation limitation of this experiment is. There is a good chance that it was contaminated with some other chemicals.
Also the concentration of NaOH solution is very likely not to have been exactly. As this concentration must also have had some errors to it. During the experiment many human errors could have been encountered.
So at times the experiment was titrated to two drops. Also there might have been a systematic error in the apparatus being utilized. This would have led to overall a small difference in the final results. The burette what we were using had an error of.
Also the electronic balance that we were using might have had a systematic error in it. The set up of the experiment was a very straightforward one.
This made the results more accurate. The best way to improve the results would be to minimize the human errors.A student collected their titration data for the standardization of NaOH in the table below.
When they did trial 2, they went past the endpoint of phenolphthalein and had to back- titrate. ion, respectively, the molarity of hydrogen ion is the same as the molarity of the acid, and the molarity of hydroxide ion is the same as the molarity of the base.
PURPOSE: To learn the experimental technique of titration and using this technique, to determine the molarity of three acid solutions of unknown concentration. PROCEDURE: 1. CHM Lab 4 Titration 2: Determination of %KHP Mass in an Impure Sample Purpose: Using the NaOH you standardized, you will determine how much KHP is in an impure Rinse out the buret with your standard NaOH solution and set it up for titrating.
use the molar mass because it is a mixture, not pure KHP. So you’ll need to use the. In the first standardization the molarity of a sodium hydroxide solution (NaOH) will be determined by titrating a sample of potassium acid phthalate (KHP; HKC 8 H 4 O 4) with the NaOH.
In the second procedure the standardized NaOH will be used to determine the molarity of a hydrochloric solution (HCl).
7. Titrate the acid with the base solution until the acid solution turns the slightest shade of pink 8. Record the amount of NaOH solution used 9. Determine the molarity of the NaOH solution Repeat steps , then calculate the a. Average number of moles of KHP b. Average molarity of the NaOH solution NaOH, since you’ll be making a finer determination of the amount of NaOH by titration later in the lab.
Q: But why can’t we just use the analytical balance to determine the exa ct mass of.