2 burets (50 ml) Standard solution of NaOH (0.600 M) Phenolphthalein indicator

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1 Name: \[-[L Percentage of Acetic Acid In Vinegar Lab 4-5 INTRODUCTION: The quality of acid in a sample of vinegar may be found by titrating the sample against a standard basic solution. ost commercial vinegar is labeled as 5% acetic acid, but can have a mass percentage of between 4.0% and 5.5% acetic acid. By determining the volume of sodium hydroxide solution of known molarity necessary to neutralize a measured quantity of vinegar. The molarity and mass percentage can be calculated. Industrial quality control chemists do this to maintain product quality. EQUIPENT AND ATERIALS: Safety goggles Double buret clamp 2 beakers, 100-mL Wash bottle 250-mL beaker (for discards) Sheet of white paper Erlenmeyer flask, 125-mL White vinegar 2 burets (50 ml) Standard solution of NaOH (0.600 ) Ring stand Phenolphthalein indicator PREPARATION OF SOLUTIONS: 1. To prepare a standard sodium hydroxide solution, use a volumetric flask to prepare the NaOH standard solution for accuracy. Add some deionized water to the clean,dry beaker. ass out the NaOH onto a watch glass. Carefully rinse the chemical into the beaker with distilled water (use a rinse bottle) to get all of the chemical into the beaker. ix the flask until the chemical is completely dissolved. Transfer the contents of the beaker into the volumetric flask, and then add distilled water until the bottom of the meniscus is exactly on the etched mark. Stopper the flask and invert to mix. Be sure you make enough solution to do the complete lab. To prepare a solution of sodium hydroxide: For 1000 ml (1 liter) use grams NaOH For 250mL use 6.00 grams NaOH For looml use 2.40 grams NaOH If you do this experiment with several brands of vinegar, you can compare the quality of the brands. Be sure to have enough standard NaOH solution so you can do all the tests with the same solution. 2. If you do not have phenolphthaldn indicator already prepared, dissolve 10 g of powdered phenolphthalein in 500 ml denatured alcohol and add 500 ml deionized water.

2 PROCEDURE: PREPARING FOR TITRATIONS: 1. Obtain approximately 80 ml of the standard NaOH solution in a clean, dry, labeled 100-mL beaker. NOTE ON BURET TECHNIQUE: When filling a buret, check to make sure the stopcock is closed. Hold the buret in your hand with a paper towel wrapped around it to catch any spill, and fill slowly. Wipe the buret up to the top with the paper towel. 2. Pour directly from the beaker into the buret a 5 ml portion of the NaOH solution. Rinse the walls of the buret thoroughly with the NaOH, allow it to drain through the stopcock, and discard it. Rinse the buret two more times times in a similar fashion, using a new 5 ml portion of the NaOH solution each time. Discard all rinse solutions. Fill the buret with the standard NaOH solution above the zero mark. and place the buret in one side of the double buret clamp (see drawing). Withdraw enough solution from the buret to remove the air from the jet tip and bring the liquid level into the graduated region of the buret. Your starting volume does not have to be zero. Discard what you withdrew. Label the buret 3. Follow steps 1 and 2 for the vinegar, and place it on the other side of the double buret clamp. Be sure to label the buret TITRATIONS: ake all buret readings to ml 4. Read the buret with the vinegar as the initial volume and record it in the DATA TABLE for trial 1, as the initial volume for vinegar. Obtain approximately 10 ml of vinegar in the flask. Read the buret and record it in the DATA TABLE for trial 1, as the final volume for vinegar. 5. Add I0 or 15 ml of distilled water to the flask to increase the volume and make reading the equivalence point easier to read. Add 1 or 2 drops of phenolphthalein solution to the flask to serve as an indicator. 6. Read the initial volume of the NaOH solution in the buret and record it in the DATA TABLE for trial 1, as the initial volume for NaOH.

3 7. Place the flask with the vinegar sample, on a sheet of white paper, under the buret. Now begin the titration by adding the hydroxide solution slowly, while swirling the flask. A pink color will appear in the center, but will go away as you swirl. When the pink color begins to linger, add the NaOH one drop at a time, swirling between each drop. When one drop is added, and the faint pink color faint pink color does not disappear, you have reached the equivalence point (the point where all the acid is just neutralized by the base, but no extra base is added). Read the volume in the buret, and record it in the DATA TABLE for trial 1, as the final volume for NaOH. 8. Discard the liquid in the flask and rinse the flask with 4 or 5 rinses of distilled water to be sure it is clean. Repeat steps 4-7 for trials 2 and 3. Record volumes for the burets in the DATA TABLE in the appropriate places. P NOTE: You do not have to refill the buret, if you are sure it will not go past the 50 ml mark in a titration, just read the initial and final volumes. If you do go below the graduations, you will have to re-do that titration, as you will not be able to read a final volume. 0, ~OGC.CCU/,~GC)/-/ tydc) t86/ 2 - A. )wu/ &46(f RESULTS: qlo@ -, =i Trial /a- initial V~~\ec,~cr Vinegar,' i n [C~L? $1- I A+ DATA TABLE Buret Readings (ml) final I t3$ (&I\ initial /'.A- NaOH,r./ I' --- final JoeS / J&O# 60 I & 1n4 S, n J PA C /2*6i 017 ( Ill 90

4 I I t CALCULATIONS TABLE 4-2 Trial volume of volume of mole mole vinegar (ml) NaOH (ml) NaOH acetic acid in vinegar Calculate the volumes of vinegar and NaOH used for each of the three trials. Record j in the CALCULATIONS TABLE, This is simply: initial volume - final volume 10. Record the molarity of the NaOH solution used in the titration. olarity of NaOH solution =. b,w{//, fo) I 1. Determine the moles of NaOH used in each of the three trials. Record in the I I CALCULATIONS TABLE. = A, v, - d&ob(~r.~oj H,(/0~35) molarity = moles solute Liters of solution 4, : OIL 272 A UC, fi c-'~.\\ us~nb the above definition as a conversion factor; mol Liters of solution number of moles = - x L I olarity of NaOH Standard solution Volume of NaOH used in the titrartion -jll1, q,jx less, I i 9/ I 3,603 9J t603 $4 Z ZL *DON'T FORGET You have to convert the ml of solut~on used lnto l~ters for the formula --- L/

5 12. From the balanced equation for the neutralization reaction, it is evident that the molar ratio between acetic acid (vinegar) and sodium hydroxide is 1 : 1. HC2H302 + NaOH -+ H20 + NaC2H302 1 mole 1 mole 1 mole 1 mole Using the molar ratio, you can calculate the moles of acetic acid in each titration. Record in the CALCULATIONS TABLE. mol NaOH x 1 mole acetic acid = moles acetic acid 1 mole NaOH Because the relationship of sodium hydroxide and acetic acid in this reaction is 1 : 1, the moles of acetic acid will be the same as the moles of sodium hydroxide. 13. Given the moles of acetic acid and the volumes of the vinegar sample for each trial, calculate the molarities for the three trials. Record in the spaces provided. Don't forget to convert the volume to liters. moles of acid = molarity of vinegar volume of vinegar olarity of vinegar for trial 1 = olarity of vinegar for trial 2 = olarity of vinegar for trial 3 = 14. Calculate the average molarity of the vinegar samples. Record in the space provided. t Average olarity of vinegar = 5

6 15. The mass of one mole (or the molar mass) of HC2H302 (acetic acid) is 60.0 g. Remembering that molarity is equal to moles / liter, calculate the grams of acetic acid that would be in one liter of your vinegar sample by the following formula: W mol HC2H g HC2H302 = grams HC2H,02 1 L vinegar I mol HC2H,02 1 Liter HC2H302 ass of HC2H302 (in grams) per 1 Liter vinegar = g 16. If we assume the density of vinegar is very close to 1.OO glrnl, then the mass of 1.OO L of vinegar is 1000 g. The percent, by mass, of acetic acid can be expressed as: mass of HC2H g vinegar x 100% = % HC,H302 (by mass) Calculate the percentage of acetic acid in your vinegar sample. Record. % HC2H,02 = %

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