The Amount Of Ascorbic Acid In A Saving Of Country Time Pen

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.

Table 2 came from the Coca-Cola experiment. The information above is the data that should have been recorded throughout the experiment.

In this experiment I will be finding out which fruit juice contains the most vitamin C. I will be using a method similar to titration but I will be using a syringe instead of a burette.

An experiment was done to determine the concentration of Allura Red in a commercially available beverage, Gatorade. This was done by using the colorimeter, the absorbance of five Allura Red solutions were measured. The graph obtained demonstrated a linear relationship and the equation obtained yielded a concentration of 1.9910-6M.

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.

Introduction: The goal or purpose of this experiment was to determine the concentration of Allura Red in red commercially available beverage- Gatorade. Colorimeter are used to shine a LED light through the solution and hit a photocell: it will detect an absorbance or a percent transmittance value. These “value” can be charted and examined as a calibration curve. Calibration curve is a method for determining a substance concentration in an unknown sample

We obtained a composition of 58 (±5.1) wt% Na2CO3 and 42 (±8.3) wt% NaHCO3 for the unknown solid analyzed in this experiment. Although the accuracy of these results cannot be fully evaluated, since we do not have a known composition concentration to compare, we must assume that there was some contribution of error, especially given the somewhat large errors observed. One possible source is a miscalculation of the volumes or concentrations obtained from the results due to exposure of CO2 in our titrants and solutions which, as discussed in the previous lab report, can make our solution more acidic than what the nature of the experiment requires.2 Therefore, different volumes of standard HCl would be necessary for titration. A simple solution for this issue would have been boiling the distilled water to expel carbon dioxide from the stock solutions. Additionally, the stock solutions may also be responsible for some of this error. Besides having stock solutions available for the entire class, which may cause cross contamination and mishandling of the stock solutions, the stock solution needed to be replenished multiple times, thus providing the possibility of preparing a solution with a different molarity. Moreover, at one point all 0.1 M NaOH had been expended, and the only option available was to use a solution of 0.08 M NaOH for further experiments. This was

To calculate the concentration of the sucrose and glucose after the first reaction, and the final concentration of glucose of the samples of Powerade and Gatorade, the Beer-Lambert equation was used.

The objective of the lab was to measure the % of NaCO3 in an Alka-Seltzer tablet in different measures of an acidic solution (Vinegar). Through understanding of stoichiometric relationships and limiting reactants, quantities of substances yielded or consumed in a reaction

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

This is an experimental lab that tested how well an antacid acid tablet will dissolve in excess stomach acid. The lab can help the creators and consumers of the drug with know how efficient the drug is. Each group got a certain antacid acid tablet to test. The lab utilizes back titration to help with figuring out the amount of hydrochloric acid(HCl) that is dissolved by an antacid acid by introducing a base with a known molar concentration. The tablet effectiveness was tested by seeing how much strong base (Sodium Hydroxide-NaOH) is needed to be added to a strong acid solution (HCl and antacid acid tablet) for a color change. A color change means that the acid solution became basic, so enough base was added to neutralize the acid. The results

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

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

pH meteric titration were carried out with jenway 3020 pH meter, Varian UV–Vis spectrophotometer and All chemicals were analytical grade supplied by BDH and Fluka.

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.