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Titration of an Acid with a Base Free essay! Download now

Home > A Level > Chemistry > Titration of an Acid with a Base

Titration of an Acid with a Base

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Downloads to date: N/A | Words: 932 | Submitted: 09-Sep-2012
Spelling accuracy: 98.6% | Number of pages: 8 | Filetype: Word .doc

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Experiment to recognise the end point of titration and the molarity of a base


Titration of an Acid with a Base

The objectives of this experiment are to:
Recognize the endpoint of titration.
Use burets to accurately measure the volumes of solution.
Describe the procedures for standardizing a solution.
Determine the molarity of a base.
Materials and Equipment:
0.500 M HCl
NaOH solution of unknown molarity
50 mL burets, 2
phenolphthalein indicator
100 mL beakers, 3
ring stand
125 mL Erlenmeyer flask
wash bottle filled with distilled water
double buret clamp

Procedures: - Three trials were taken
The titration apparatus was set up by using the buret clamps to clamp the burets on each side of the ring stand. One buret was labeled NaOH and the other was labeled HCl.
Approximately 80 ml of each solution was poured into labeled beakers.
The walls of the NaOH buret were rinsed with approximately 5 ml of NaOH solution. The solution was discarded into the unlabelled beaker. This process was repeated two more times. Rinse solution was then discarded.
The NaOH buret was filled with solution above the zero mark. Solution was drawn out to remove air from the buret tip and to drop the liquid level down to the graduated part of the buret.
Steps 3 and 4 were repeated for the HCl buret, using HCl solution.
The initial readings of the volume levels of each buret were recorded in the data table.
An Erlenmeyer flask was placed under the NaOH buret. About 10 ml of NaOH solution was drawn off from the NaOH buret into the flask. Distilled water was added to increase the volume, and then a couple of drops of phenolphthalein solution were added to the flask. This turned the solution pink.
The titration began by placing the flask under the HCL buret, and slowing adding HCL to the flask. The flask was swirled while HCl was added to mix the contents. Frequent stops were made to wash down the inside of the flask with distilled water from the wash bottle.
When the pink color of the solution began to disappear as the acid was added, the acid was added drop by drop, swirling the flask after each drop. When the color completely disappeared from the entire solution. The titration was stopped.
The flask was then placed under the NaOH buret, and NaOH was added dropwise until the pink color returned. The flask was then returned to the HCL buret, and HCL was added, dropwise until the color disappeared. This process was repeated until just one drop of NaOH cause a slight color change.
The endpoint volume levels of each solution were recorded in the data table.
Steps 6 through 11 were repeated for two more trials for a total of 3 trials. The known concentration of the HCl solution was recorded in the data ...

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