Help please 3.de33520 m Experiment 12 | TitrationPost-Lab Questions1. If you get to the end point of your titration and wait a few hours, you'll find that the color hasdisappeared. What has happened? Write the chemical equations for the reactions involved inthis delayed color change. (Hint: See the note at the end of Step 12 in the Procedure Section ofthis experiment.)2. Why do we titrate into a flask and not a beaker?Name:aWhat effect would each of the following errors have on the determined concentration of theunknown acid? Would the calculated result be erroneously high, erroneously low, or unaffected?C.You forgot to condition the buret and it contained some deionized water before youadded the NaOH. Circle one: too low / unaffected / too highb. The Erlenmeyer flask was wet with deionized water before you added the acid to it.Circle one: too low / unaffected / too highYou forgot to condition the pipet before using it to transfer the acid to the flask.Circle one: too low / unaffected / too high / dependsd. The final buret reading was mistakenly recorded too high (e.g., recorded as 35.00 mlinstead of the actual 30.00 mL). Circle one: too low / unaffected / too high4. Based on the true molarity of your acetic acid unknown, and assuming that its density of thesolution is 1.01 g/mL, calculate the mass percent of acetic acid in your unknown. 0.00/2540.0100L12.54x0 10omansonTMOTHCLOOL HAI7 Name: Macy huffordData Table and Results Nao C₂30₂ H₂O+NaC₂H₂O₂Molarity of NaOH:.3455 M0.25% FParolaccuc acid0.01000LVolume of acid added toflaskInitial buret readingFinal buret readingVolume of base titrated intoflask*Trial 1Experiment 12 | Titration10.00MLAV=VP-ViTrial 210.0m 10.0m 10.0Calculated molarity of aceticacid in your unknown*Final buret reading - Initial buret reading.Unknown #:True molarity:Trial 30.01 21:19426.0921.07m 42.38m4 47.18ml21.01mL 21.19mL 21.09Trial 4(if needed)Trial 5(if needed)Calculate the molarity of acetic acid in your unknown for each trial and show a sample calculationbelow. (Your instructor may require that you show the calculations for all trials. If so, attach themon a separate piece of paper, if necessary.)trial 1:Choose the three trials that have molarities that agree within 1% of one another and use these threemolarities to calculate your average molarity.Obtain the true molarity for your acetic acid solution from your instructor and record it at the top ofyour data table below the unknown number. Using the average molarity that you calculated above,calculate the percent error for your unknown.

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