When Acetic Acid Meets The Criteria Of The Commercial Law

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In this experiment, you measure the acid concentration and determine if the acetic acid meets the criteria of the commercial law. The titration of vinegar has a solution composed of acetic acid (HC2H3O2), water and other substances. When adding sodium hydroxide (basic solution) to acetic acid (acid) it causes a neutralization reaction. The phenolphthalein is colorless in acid, and it will change color when adding the sodium hydroxide. In this experiment, there were four trials to reach the amount of sodium hydroxide needed to reach the end point. When you reach the end point of the experiment, the solution should be pink and if the solution is purple then it is over titrated.
First, you make sure all of the liquid (water) is emptied out of the buret. Next, you fill the buret with sodium hydroxide
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When pouring the NaOH in a flask, a drop of NaOH could be the difference of reaching the accurate measurement to titrate the vinegar sample or you can over titrate the vinegar sample.
4. If the titrated standard NaOH, in the flask against vinegar, in the buret, instead of the way you actually performed the titration, how would you have recognized the end-point with phenolphthalein indicator? Would carrying out the titration in this manner change your calculated results or conclusions?
If the titration uses a phenolphthalein as an indicator, then its end point would always be recognized when the solution is pink.
5. Why is it a good idea to rinse the buret with the NaOH solution, instead of with water, before filling it at start of the titration?
If you rinse the buret with water, there is still plenty of proton remaining and there shouldn’t be any water left in the buret. If so, NaOH solution would be less as stronger than presumed. You wouldn’t get the accurate result because the solution would be diluted. It would hard to determine the correct concentration of the
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