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Lab 5: Acid-Base TitrationGeneral Chemistry I – Prof. MartinezI.ObjectivesTo learn about how acid-base titrations are performedTo perform an acid-base titration and determine an unknown acid concentrationII.IntroductionIn this experiment, a technique known as atitrationwill be used to determine theconcentration of hydrochloric acid. A titration involves performing a controlled reactionbetween a solution of known concentration (the titrant) and a solution of unknownconcentration (the analyte). Here, the titrant is an aqueous solution of sodium hydroxide(NaOH) and the analyte is hydrochloric acid (HCl). When mixed, a neutralization reactionoccurs between sodium hydroxide and hydrochloric acid:NaOH (aq) + HCl (aq) à NaCl (aq) + H2O (l)(5.1)The sodium hydroxide will be gradually added to the hydrochloric acid in small amountsfrom aburette. A burette is a device that allows the precise delivery of a specific volumeof a solution. The NaOH will be added to the hydrochloric acid sample until all thehydrochloric acid has been exactly consumed (reacted away). At this point the reaction iscompleted, and no more NaOH is required. This is called theequivalence pointof thetitration.In order to know when the equivalence point is reached, anindicator solutioncalledphenolphthalein is added to the hydrochloric acid at the beginning of the titration.Phenolphthalein is a pH sensitive organic dye. Phenolphthalein is colorless in acidicsolutions like vinegar, and deep pink in basic solutions like sodium hydroxide. At theequivalence point of the titration, just one drop of NaOH will cause the entire solution inthe Erlenmeyer flask to change from colorless to a very pale pink.All labs written using collective resources shared by numerous Lone Star College System Chemistry Faculty. For moreinformation, please contact me at[email protected]

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