Lab Report On Titration

Introduction: This experiment is going to test the ability of antacids and how they absorb acid to see which is a better buffer. An antacid neutralizes acid, and this helps the most with heartburn. Heartburn is where stomach acid is regurgitated back into the esophagus, and this causes a burning feeling in the chest (Oxford University Press, 2017). A buffer is a source of hydroxide ions that can absorb hydrogen ions, which in turn keeps the pH stable (Mader, 2017). In this experiment, the different antacids that are being tested to absorb the hydrogen ions from stomach acid are the buffers. The pH scale helps determine how acidic or basic a solution

In this laboratory exercise, we used the single celled ciliated protist Tetrahymena to be a model organism for the formation of vacuoles. For this lab, you should be able to see Tetrahymena vacuole formation through phagocytosis, and be able to calculate the rate of formation. The cilia of the organisms sweep food particles into the "mouth" of the cell, and get enclosed within the vacuoles through the process of phagocytosis. You can visualize that process through a microscope and feeding Tetrahymena India Ink, stained yeast cells, and observe vacuole formation. In order to test whether or not the concentration of India ink affects the rate of

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.

To start off the experiment 25mL of water was placed into a labeled beaker and tested for the pH using pH test strips. Next the antacid tablet was placed in the solution and timed for how long it took to dissolve the tablet. Finally the temperature was measured. This same process was repeated for the acidic solution, and finally for the basic solution. After each experiment the pH, the reaction time, and the temperature of the beaker were recorded into a table. For this experiment the independent variable was the substance used (acid, neutral or base), and the dependent variable was the reaction time of each substance. The constant conditions of this experiment included the amount of substance being used, and the placing of one antacid tablet into each beaker. The experimental group was the acidic and basic solution, and the control group was the neutral

Upon the addition of water, it was noted that a layer separation occurred and the water layer remained on top, with the 2-methylphenol layer on the bottom layer. Then, conversion calculations were performed to determine the appropriate amount of 3M NaOH to be added to the 2-methylphenol solution. From the calculations, it was determined that 1.08 mL were to be added. 3M NaOH itself was a cloudy solution in appearance and upon the addition of 3M NaOH to the 2-methylphenol solution, it was noted a color change occurred and it became a yellow-green solution. Following this, the same calculations used previously, were used to determine the appropriate amount of sodium chloroacetate, which was found to be 0.38 g (3.26 mmol). Sodium choloroacetate was a white, crushed solid that was then combined with 1 mL of water and was swirled until the sodium chloroacetate completely dissolved. This sodium choloracetate solution was then transferred to the 2-methylphenol solution by the use of a medicine

In order to test the rate of phagocytosis in tetrahymena, the tetrahymena need to ingest particles that are visible under a light microscope. The substance used in this experiment was India ink. India ink is deep black colored ink containing dispersed carbon particles. The trethymena treat the India ink as if it were food and ingest it. There were three concentrations of India ink that were fed to the eukaryotes The percent’s that were used are: 1%, 5% and 10% of India ink. After certain time intervals, the tetrahymena were fixed with a compound called 3% paraformaldehyde (PFA).On the first day six different mixtures of tetrahymena and ink concentrations were made to test which conditions would express the best rate of phagocytosis. The well fed tetrahymena were fed with 1% India ink, the another group was fed 5% India ink, the last group was fed 10% India ink. Then the starved tetrahymena were fed in the same manner as the well-fed tetrahymena. After adding the ink to the microcentrifuge, we prepared a slide for each mixture at the following time intervals 2 minutes, 5 minutes, 10 minutes, 20

The antacid each group added to their HCl solutions all increased the pH of the HCl to a certain degree. In order to determine the best antacid, the trial/antacid where the least amount of NaOH was added in order to turn the HCl solution pink needs to be identified. This tells which solution was the most basic before the addition of NaOH, and consequently tells which antacid increased the pH the most, making it the

2. (5 pts) List and explain the names and affiliations of the various characters/stakeholders in this story – I’m looking for us to use the story to map out the complexities that are generally associated with solving public health puzzles – the stakeholders you list and explain here should apply to many of the cases we consider going forward.

In a test tube, 0.5mL of the sample will be added with 0.5 mL of water and shaken vigorously. Take note for its solubility by parts (0.5mL is one part). Keep adding parts of the solvent until the sample is soluble. If not, add until ten parts of the solvent and determine its solubility. To separate test tubes, water will be replaced with ethanol, chloroform, ether, and acetone as solvents. Same procedures were

Its concentration was found through a quantitative and qualitative titration testing. Because HCl is acidic, a 1.07M NaOH solution was used to titrate an aqueous solution of HCl (the unknown solution). The PASCO program gave the final results shown in Figure 1. A typical titration curve can be described as starting at the initial pH of the solution, then some acid/base is added, until a sharp curve either up or down takes the pH past a neutral of 7, and towards the pH level of whatever the added acid’s/base’s pH is (Clark6). The stronger the acid or base being titrated, the faster the change occurs, which means a sharper slope of the titration graph. Also, it is important to note the equivalence point on this titration graph. At the equivalence point “the correct amount of standard solution must be added to fully react with the unknown concentration” (Xavier3). In Figure 1, this equivalence point is shown by where the sharpest slope occurs in the curve, which is seen at about a pH of 5.0

October 17, 18, and 19, samples were collected from multiple sites along the BSR. The class was split into groups, and samples were collected from seven separate locations along the river and WWTP. There was also a sample collected by the S which is located between sites four and five. For each of these sites, there were ten groups from other labs that also collected a sample from the BSR. At site two of the river, the location included multiple sources of possible contamination. A drainage site was located 200 yards upstream, along with a small PVC drainage pipe next to the collection site. Not only was there drainage running into the river, the site was under a bridge, and contained other trash scattered throughout the area. The

The purpose of the experiment was to compare antacids by the amounts acid they neutralize to find the most effective antacid. Finding the most effective antacid is important because it will help others by allowing them to choose the best product for their heartburn. Titration is the process of which the unknown solutions concentration reacts with a known solution concentration. During the experiment, titration was used to calculate the moles of HCl neutralized by the antacid in this case was gelusil, by knowing the moles of HCl initially added to the flask and moles of HCl neutralized by the NaOH.

For this experiment, titrations on a weak acid, acetic acid, and a buffer were performed. Acetic acid was titrated with NaOH in order to observe the half-equivalence point as well as the equivalence point. Then, the buffer and the buffered acetic acid solution prepared faced additional titration with NaOH and HCl to evaluate the differing buffering effects following the addition of a strong acid and strong base. Finally, the buffer’s buffering capacity was calculated. If the experiment were to be repeated, it would be interesting to observe the buffering effects following a titration between a weak base and a buffer instead with greater concentrations. The change in the concentration following the preparation of buffer with a weak base and its conjugate acid would pose for an interesting experiment to observe an increase in the buffering capacity.

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.

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.