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Acid-Base Titration Experiment

To titrate a hydrochloric acid solution of unknown concentration with standardized 0.50 M sodium hydroxide and to utilize the titration data to calculate the molarity of the hydrochloric acid, and the molarity.
Prepare for lab. Put on apron and goggles. Take 50 mL of the hydrochloric acid solution of unknown concentration and about 100 mL of the standardized NaOH solution. Record the value in Table.
Use suction bulb, pipet 10.0 mL of the HCl solution into a 250 mL Erlenmeyer flask, after rinsing your pipet with small amount of HCLfirst.
Add 3 drops of phenolphthalein solution.
Rinse a clean buret with approximately 15 mL of the standardized NaOH solution. Drain the buret and refill with standardized NaOH solution. Record the initial volume of the NaOH in the buret in your Table.
Gradually dispense some of the standardized NaOH solution into the titration flask. Swirl the flask constantly. Continue adding NaOH, noting any changes in the flask.
As the equivalence point approached, a pinkish color will appear, and the dissipate more slowly as the titration proceeds. Now add NaOH drop by drops. Stop when the addition of a single drop causes the solution to remain pinkish for 30s. Record the volume of NaOH needed to reach the equivalence point in your copy table 1, and repeat the procedure again from getting 10.0 mL sample of HCL and compare the result.
Mix any leftover acids and bases together to neutralize, and pour down the sink with plenty of water.
MOLARITY OF NaOH TRIAL 1 TRAIL 2 TRAIL 3

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