Acid-Base Titration Lab

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.

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.

In this essay I will be discussing four conditions: respiratory acidosis, respiratory alkalosis, metabolic acidosis and metabolic alkalosis. I will be defining each condition by including the levels of PCO2 or HCO3- and the pH levels, common causes for each condition, the compensatory mechanism for each condition, treatment mechanisms for each condition, and how older age may compromise the acid-base balance processes.

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.

b) The graph will be mirrored, so that the PH levels go from low to high rather than high to low, because the sample is now an acid becoming more basic not a base becoming more acidic..

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.

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.

4. It would be difficult to measure the concentration of acid in red wine or coca-cola because the colour of the drink is too dark for us to see when the phenolphthalein indicator changes colour. You could overcome this difficulty by using a pH meter.

According to Le Chatelier's principle, the equilibrium shifts to the left, making Phenolphthalein colorless. At a high ph level where the H3O- concentration is low, the equilibrium shifts to the right, showing the pink color of Phenolphthalein. This allows it to be used in both weak acid-strong base and strong acid-strong base titration. In a weak acid and strong base titration, the equivalence point would be above 7 due to the reaction occur between the conjugated base and water. This often makes the pH value detectable by Phenolphthalein. In a strong acid and strong base titration where the equivalence point is 7, the spike of pH around equivalence point is huge and all indicators at this range change color at the same volume of acid or base. Therefore, using Phenolphthalein in this case won’t cause major

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

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.

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

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

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