Acid-Base Titration Lab

4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

To begin, three sets ofabout 0.3000g of KHP are weighed out on an analytical balance. Put the three sets of KHP into three separate, labeled flasks. All three sets of the KHP is then dissolved with approximately 50mL of deionized water. Next, a buret is used to start the actual titration. Buret is initially filled to 0.00mL mark with the NaOH solution, this is recorded as initial volume. Next, add 2-3 drops of phenolphthalein indicator into each of the three flasks containing KHP. A magnetic stir bar is then added to the first flask, and placed above a stir plate. Everything is positioned under the buret. Stirrer is put on medium speed and the titration can start. Slowly release the NaOH into the KHP flask. As the end point is reached, a pink color will be seen in the flask. When the lightest pink possible remains in the solution for more than 30 seconds titration is complete. The final volume is recorded, and the same steps are taken for the other two sets of KHP solution. Finally, blank titration is completed to determine deviation.

The purpose of the experiment was to determine how a buffer works and how to use an acid-base indicator. The way a buffer works was determined by observing the changes in pH of solutions of different concentrations weak acids and their conjugate bases to determine how a buffer affects the pH change. The solution of 10 mL of 0.20 M CH3COOH and 10 mL of 0.20 M CH3COONa had slighter changes in pH than the solution of 10 mL of 0.0020 M CH3COOH and 10 mL of 0.0020 M CH3COONa. Both of these solutions were buffers, shown because they had slighter changes in pH than the solutions with only the weak acid or conjugate base and water. The determination of how buffers work was also tested with observing that the solution of NaC4H3O4 and Na2C4H2O4 had smaller

The purpose of this experiment was to determine the pKa of the bromothymol blue (indicator) through absorption spectroscopy. Bromothymol blue being a monoprotic acid base indicator, displays different colors at different pH because of the differences in the ratio of the conjugated acid and base form. The fraction of conjugate acid and base was interpolated for the solutions through the acquired absorbance spectrum of the bromothymol blue at various pH. The rearranged form of Henderson Hasselbalch equation was graphed as a function of pH to determine the pKa of the indicator.

A weakness of using red cabbage indicator to check the pH of an unknown solution or buffer is the subjectivity of determining color. What one individual sees as pink. another person would see as light purple. Color blind individuals would be at a significant disadvantage. Accuracy of pH is another consideration, since in addition to the variability in shades of color the pH shown by the red cabbage indicator is more of a ballpark estimate and limited to whole numbers. Using a pH meter, we can get a significantly more accurate reading that is objective and not dependent on an individual's interpretation of color or visible hue.

Introduction The inspiration for this experiment came from a book called Counting by Sevens by Holly Sloan. The main character in the book has a garden and she regularly checks the pH value of the soil in her garden. From this came the idea to do this science fair experiment on pH values. Through the years people have found out the different ideal soil pH values of plants, herbs, vegetables, as well as the pH value of cow’s milk and blood.

Acid-base balance in the body is important to maintain our normal functions. The regulation of hydrogen ions is essential for the body to perform normally and to achieve homeostasis. Our bodies maintain a pH level between a small margin of 7.35 to 7.45. If the pH level becomes too low, the body goes into a state called acidosis. On the contrary, if it elevates too far, the body enters into a state called alkalosis.

While the goal of this lab was mainly to be able to perform an acid-base titration. Complete a traditional titration and then and a pH electrode titration. Calculate the molarity of citric acid from the titration volume of NaOH. Calculations should be fairly close in average and the ending point should coincide with the equivalence point. All while effectively being able to compare and contrast the two methods to detect the endpoints of an acid-base titration.

First, three titration curves and three second derivative curves were created to determine the average pH at the half-equivalence point from the acetic acid titrations. Titration curves were used as visuals to portray buffer capacity. The graphs and a table, Table 1, that showcased the values collected were created and included below. The flat region, the middle part, of Figures 1, 2 and 3, showed the zone at which the addition of a base or acid did not cause changes in pH. Once surpassed, the pH increased rapidly when a small amount of base, NaOH, was added to the buffer solution. Using the figures below and

In this lab, the pH scale was used to determine which waters are most healthy to drink. The term ph means potential hydrogen. It is a measure of the hydrogen ion concentration when talking about a solution. If a solution has a high concentration of hydrogen ions, it will have a low pH and solutions with a low concentrations of H+ ions will result in a high pH. pH is a very well known water test to ensure that the water is healthy to drink. pH reveals the water’s acidity and it is a measurement of the potential activity of hydrogen ions. The pH scale is from 0 to 14. If one has a pH of 7.0 that is considered neutral. Solutions with a pH below 7.0, are considered acids. Solutions above 7.0 are considered basic. The purpose of this lab is to conduct

Phenolphthalein is an indicator commonly used in acid-base titration. Explain how the equivalence point of acid-base reaction can be determined using this indicator. State relevant reactions, pH ranges and qualitative

Purpose: The motive of this experiment is to determine the pH with potentiometric measurement using a pH meter and electrode.

The purpose of this experiment was to determine how much KMnO4 was needed to titrate approximately 1 mL of an Unknow X101 concentrated solution of Oxalic Acid. A standardized KMnO4 solution was used on a known solution of Oxalic acid to help determine the unknown percent oxalic acid in unknown X101. The unknown sample for this experiment was sample x101 which theoretically was a % Oxalic Acid dehydrate sample but, the average of all three trials determined it to be a 6.7% percent Oxalic acid.

For the determination of acidity, 10g samples of three fish sample from each treatment will randomly selected, crushed and homogenized with 200 mL of distilled water in an Ultra-Turrax homogenizer for 1 min. This solution will be transferred to a 250 mL volumetric flask, and the volume will be completed with distilled water. This solution will be filtered, and 25 mL of the filtrate will be added to 75 mL of distilled water and three drops of 1 % phenolphthalein alcohol