Determination Of Total Acidity Lab Report

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.

Herbal remedies-aromatic plants that may be used by people from all ethno cultural traditional backgrounds as one method of restoring physical health. (Africa)

The pH was tested by adding acid (HCl), base () and neutral (water) to the enzyme. When the enzyme samples were tested using the hydrogen peroxide and O2 sensor test it was determined that any

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 standardized concentration of NaOH was used to identify the unknown acids, this value is shown is experiment 16.1. This mean standardized concentration was 0.0784 M. By titrating a known amount and concentration of this standardized base to the unknown acid, a titration curve and its derivative could be plotted in order to find the molar mass and acid dissociation constant. The first unknown acid titrated, BGYW, was identified to be Maleic acid, C4H4O4.

The use of natural products as medicine has initiated the isolation of active compounds. The first commercial pure natural product introduced for therapeutic use is generally considered to be

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

“Traditional pharmacologic therapies although widely used must be assessed for a favorable risk-benefit ratio. One such plant that has

In this Lab report we will be using Red Cabbage extract as an indicator to determine the pH of substances. The purpose of this experiment is to see if and how base and acids react. Indicators are chemicals that change color depending on the pH solution that they are dissolved in. This experiment will determine which items we use to determine ph. The pH of a solution indicates its acidity or alkalinity. There is a ph. scale that determines if the items such as lemons or bleach are an acid or a base. I have chosen to use red cabbage in this experiment so that I can know the range of the item that

Summary A standardized vinegar solution was prepared, to test how much sodium hydroxide is needed to turn the solution pink. In order to know when the equivalence point is reached, an indicator solution called phenolphthalein was added to the vinegar at the start of the titration. Phenolphthalein is an organic dye which is colorless in acidic solutions

The results were compared to the calculated pH. The unbuffered solutions were: 30 mL DI H2O, 30 mL DI H2O with 2 mL 3.0 M HCL, and 30 mL DI H2O with 2 mL 3.0 M NaOH. The buffered solutions were divided into three categories, carbonate, phosphate, and acetate. The carbonate buffered solutions were 30 mL 0.4 M sodium carbonate with 30 mL 0.4 M sodium bicarbonate , 30 mL of the previous buffer with 2 mL 3.0 M HCl, and 30 mL of the previous buffer with 2 mL 3.0 M NaOH. Next, the phosphate buffered solutions were 30 mL 0.8 M sodium phosphate monobasic with 40 mL 0.8 M sodium phosphate dibasic, 30 mL of the previous buffer with 2 mL 3.0 M HCl, and 30 mL of the previous buffer with 2 mL 3.0 M NaOH. Lastly, the acetate buffered solutions were 25 mL 1.6 M sodium acetate with 10 mL 1.6 M acetic acid (Buffer A), 15 mL 1.6 M sodium acetate with 20 mL 1.6 M acetic acid (Buffer B), Buffer A with 2 mL 3.0 M HCl, and Buffer B with 2 mL 3.0 M NaOH.

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 a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.

Herbal medicines are great alternative for commercially manufactured medicines available in the market. The major reason why herbal medicine differ from modern medicine is because they are produced with 100% natural content. Therefore the plant extract has all the medicinal values that are as effective as modern medicine. Commercially prepared drugs show results quickly but have numerous side effects. However herbal medicines don’t show any side

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.