Standardization of acid base
In addition, you should use a black-lined background card to accurately read the meniscus.
Empty the burette out the top and repeat the water washing, this time also opening the stopcock when the burette is inverted to drain most of the water from the tip.
Titrate the sulfuric acid solution in Flask 1 to the lightest pink that your eye can detect and that will not go away with stirring.
Standardization of naoh with hcl lab report
Sheena Resando Experiment No. Then twirl the burette and slowly empty it through the top, being careful to wet the entire interior wall with the new solution. Equivalence point was reached as orange-colored solution was observed. Add 3 to 4 drops of phenolphthalein indicator to the HCl solution in the Erlenmeyer flask. Why is it important? Preparation of Solutions An approximately 0. Dissolve in deionized water and titrate with standard NaOH.
Since the absolute accuracy of the balances can vary slightly, it is important that you use the same balance throughout an experiment. In this activity, the concentration of NaOH analysis is determined by using the NaOH solution to titrate an exactly known mass of primary standard potassium hydrogen phthalate or KHP.
Standardization of naoh with khp conclusion
Then, fill the burette with deionized water and carefully place it in the burette rack. Dissolve in deionized water and titrate with standard HCl. Part III. The beaker was rinsed thoroughly to transfer all the washes to the flask and was filled with water up to the mark. Rinse the buret with three portions about 5 mL of the NaOH solution. Pour the contents of the graduated cylinder into your flask. The concentration of sodium hydroxide is 0. This rinse water can be poured down the drain. It is not necessary to have exactly one gram in each flask but it is necessary to know accurately how much you have in each flask. The point at which the reaction is complete in a titration is referred to as the endpoint. Given that the molecular weight of KHP is The weighing bottle should remain uncapped throughout this operation. Continue this operation until the desired sample size has been obtained. Reweigh the container accurately. Discard the contents of the Erlenmeyer flask into the waste container located under the hood.
Given that the molecular weight of KHP is If it does not, then a measured amount of base must be added to change the color to blue and this volume of added base must be included in the calculations. As the endpoint was approached, the color disappears more slowly, at which time NaOH solution was added drop by drop.
Thus, the data obtained is a precise one but less accurate since its percent error is more than one.
Pour the contents of the graduated cylinder into your flask. The point at which the reaction is complete in a titration is referred to as the endpoint. Weigh three samples of your dry, cooled unknown KHP within the mass range of 0.
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