Titrations allow you to calculate the concentration of a solute in an unknown solution, based on a standard solution, where the concentration is known. Acids and bases combine in solution to form water and a salt, essentially neutralizing each other. For example, sodium hydroxide, which is a base, neutralizes acetic acid, forming the product sodium acetate and water.1 The chemical reaction reaches the equivalence point when the two solutions are stoichiometrically identical. For acid-base titrations, indicators may change color due to a change in pH, which can help determine where the equivalence point is. Say no to plagiarism. Get a tailor-made essay on “Why violent video games should not be banned”?Get the original essayA burette is cleaned with distilled water and rinsed with about 5 ml of NaOH solution, then filled to 0 .00 ml of NaOH. The NaOH level was recorded. A volumetric pipette was used to fill a 125 mL Erlenmeyer flask with 5.00 mL of vinegar (also known as acetic acid) and 3 drops of phenolphthalein were also added to the flask. The flask was placed under the burette and NaOH was added slowly to the flask while swirling it. Once a slight color change from clear to pink began, no more NaOH was added to the flask and the burette volume was recorded. The burette was refilled with NaOH and this entire process was repeated 3 more times for a total of 4 trials. The liquid volumes in this experiment were critical because 1 drop of NaOH had the potential to change the color of phenolphthalein in solution. from clear to purple. A modified version of the dilution rule was used to calculate the molarity of acetic acid. The concentration of acetic acid declared by the producer was calculated by converting g/mL to mol/L or M, in order to compare it to the calculated value of acetic acid concentration. The two values ​​were very close and the percentage error was well below 5%, so the experimental procedure did not need to be changed. Keep in mind: this is just a sample. Get a personalized article from our expert writers now. Get Custom Test This experiment demonstrated how the molarity of an unknown solution in an acid-base titration can be determined using the known volumes of solution and a standard solution. The rapid color change of phenolphthalein indicates how the equivalence point can be very difficult to reach once the pH approaches that of the equivalence point. A single drop of NaOH when the solution is near the equivalence point can drastically change the pH. The percent error for the calculated molarity of acetic acid was 0.120%, so the experiment is valid..