Lab Report #4 Titration Of Hydrochloric Acid With Sodium .

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Lab Report #4Titration of Hydrochloric acid with Sodium Hydroxide

SCH3U. 02Thursday, December 19, 2013IntroductionThe following lab was an acid-base neutralizing titration. A titration is a technique, in which a reagent,called a titrant, of known concentration is used to determine the concentration of an analyte orunknown solution. Using a calibrated burette, the initial volume of the titrant is recorded. The exactamount of titrant must be added to the acidic solution for a chemical reaction to occur. This is anindicator that enough of the standard solution was added for an equalization of moles between theanalyte and titrant within the aqueous solution. In the following experiment, the indicator was that thebeginning of the aqueous solution changing from a colorless liquid to a light pink. In order to obtainaccurate results the equivalent point must be attained accurately by slowly adding the titrant to theanalyte for it to reach its end point. The endpoint is the point at which the titration is stopped. The endpoint was when the full solution appeared a light pink. Lastly the final volume of the titrant must berecorded. With this data, the volume of NaOH used can be calculated. Using the formula C1V1 C2V2,where C1 is the molarity of the NaOH, the difference in volume is the V1 and the amount of aqueoussolution that was measured in the Erlenmeyer flask is the V2.PurposeTo determine the concentration of an Unknown Hydrochloric acid solution.MaterialsPlease refer to page 1 of 2 on the lab handoutProcedurePlease refer to page 1 of 2 on the lab handout.

Observations/DataBurette ReadingmLFinal ReadingTrail 1Trail 2Trail 321.6mL38.7mL49.5mL 39.2mL 88.7Initial Reading5.1mL21.6mLVolume of NaOH16.5lmL17.1mLCalculationsAverage of your twoclosest burette readingsGivenAverage V of NaOH;16.81mLMolar concentration ofNaOH; 0.100MWantMolar concentration ofHCLTrail 4(if nec.)50.3mL 41.9mL 92.2mL38.7mL 27.8mL 66.6mL 39.2mL 41.00mL80.2mL22.1mL12mL

Results and DiscussionThis experiment was conducted to determine the analyte. The results showed that three of the fourresults were close and that the outsider of the trails was trail number three because its value is relativelyhigher than the others. This could be due to how the trails were carried out. Trails one, two and fourwere conducted closely in the same fashion. In the first, second and fourth trials, using a calibratedburette the titrant were poured at a reasonable rate into the Erlenmeyer flask, which held the analyte.As the reaction began, occur the nob of the burette was slowly closed, but only after the reaction hadreached its end point. Contrasting to the first, second and fourth trails, the third trail were conducted inwhich the nob was only slightly ajar thus, only a few drops would drip into the Erlenmeyer flask. Therate at which the reaction occurred too longer and thus the nob was opened and closed several times.The reaction took a longer time to occur and used much more base than needed.Volume measurements play a key role in titration. The initial volume and final volume of all three trailswere subtracted to find each amount of titrant delivered. The two closest burette readings conductedwere trail two, where the volume of NaOH calculated was 17.1mL and trail four, where the volume ofthe NaOH calculated is 18ml. These two values were then used to calculate an average volume of17.55mL of NaOH. Using the average concentration of the titrant and the stoichiometry of the titration,with the given molarity of the Sodium hydroxide the number of moles of the reactant in the analytesolution can be calculated. In the calculations for the experiment, the results showed the molarity of theHydrochloric acid to be a value of 0.029mol.Source of experimental errorSome experimental error that could have occurred is that the volume of the hydrochloric acid in theErlenmeyer flask could have a different measurement than that which was used in the calculations dueto different factors, such as the 2 to 3 drops of phenolphthalein indicator. Even though there was a smallamount added, it does have a difference. For, more accurate results the solution should have beenmeasured.As the endpoint was being reached, a partial drop of the titrant was not added, more like a few drops ormore were added, which could cause inaccurate results. Also, the solution wasn’t a light pink. It was alight pink, but a slightly darker light pink.Also when the measurements were being taken, for one of the trails the mincus went below the 50mLmark the mincus had to be estimated, before adding more solution, which could have contributed to

misreading because one’s eye are not at a tangent to the liquid level. This experimental error could haveoccurred with the other values as well.ConclusionIn conclusion, the experiment was a success as the molarity of the Hydrochloric acid solution was foundby stoichiometric methods. By titrating measured volumes with a strong base of known concentration,the unknown molarity of the acid was determined. The process of the experiment involved preparing acalibrated burette and recording the initial ad final NaOH volumes for 4 trials. The data was not asaccurate as it would have been hoped because time was a lack of resource so we could not be as carefulas we wished. However, even with experimental error for a first titration experiment, the experimentwas shown to be a success.Some improvements for this lab could be more trails could be conducted for more accurate results. Theexperiment could have been conducted more carefully.

The following lab was an acid-base neutralizing titration. A titration is a technique, in which a reagent, called a titrant, of known concentration is used to determine the concentration of an analyte or unknown solution. Using a calibrated burette, the initial volume of the titrant is recorded. The exact

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