Volume of diluted vinegar added 1000 ML 1000 ML 1000 ML Molarity of NaOH

Volume of diluted vinegar added 1000 ml 1000 ml 1000

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Volume of diluted vinegar added10.00 ML10.00 ML10.00 MLMolarity of NaOH determined in standardization0.04121 MFinal buret reading, NaOH37.79 ML42.17 ML41.70 MLInitial buret reading, NaOH0.10 ML0.72 ML3.31 MLVolume used, NaOH37.69 ML41.45 ML38.39 MLMolarity of acetic acid in thediluted vinegar solution 0.1553 M0.1708 M0.1582 MAverage molarity of acetic acid in the diluted vinegar solution0.1614 M ( 0.1553+0.1708+0.1582/3= 0.1614)
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Molarity of acetic acid in original vinegar1.076 M ( 0.1614 X 100/15= 1.076)Calculations
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DiscussionTitration is a technique for determining ether the concentration solution of unknown molarity or the number of a substance in each sample. A chemical reaction is used for this purpose, and the reaction must be fast, be complete, and have a determinable end point. The reactions of strong acids and bases generallymeet these criteria, and acid-base titrations are among the most important examples of this technique. In this experiment, the sample is hydrochloric acid and sulfuric acid as acid substance and sodium hydroxideas base substance where the concentration of sodium hydroxide unknown. Given that, the concentration of the both acid are 0.1 M.ConclusionAlways make sure that the burette is full to at least 20.00cm3 before beginning titration. Titrating without any indicator. Without the indicator, there will be no color change in the conical flask containing the acid and the base. Ensure to add 2 or 4 drops of the indicator and swirl before beginning to titrate. Limitations and weaknesses This experiment is restricted to an acid base neutralization. A precipitate cannot be used in this experiment. The experiment cannot be stopped at the equivalence point as there are no materials to do that. It can only be stopped at the end point. Leaving the funnel on the tip of the burette while titrating.This could increase the initial volume of the base making the result inaccurate. Forgetting to refill the burette after each titration to avoid running out of the base in the middle of the titration.
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  • Fall '12
  • Mariani
  • Chemistry, Sodium hydroxide

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