Naoh Dispensed Lab Report

increasing the waste of HCl. Water was also used to wash the vial to remove all solids

Germination is affected by many factors including pH. The pH scale is a logarithmic scale that runs from 1 to 14. If the substance ranges from 1-6 it is considered to be on the acidic side, however, if the substance ranges from 8-14 it is considered to be on the basic side. A pH of 7 is neutral, which is typically the pH of pure water. Plants typically have a specific tolerance for pH ranges in which they can flourish.

The main possible source of errors on this experiment is based on the measurement of mass and volume for the experiment, which could affect moles of NaOH and HCl, could as well affect the antacid titration. One question I have after this experiment is that, how the increasing of mole of the tablet would affect the titration? This experimental work can be related to lecture on how acid and acid bases interact to each other, and also this experiment give a better understanding on term pH. A real life application for acid base titration is that is use in medicine and most food

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

The initial goal of this experiment was to investigate the properties of an unknown acid or base. These properties include pH, concentration, and how the solution behaves once titrated. In order to accomplish these goals, the initial pH of the unknown compound needed to be found through the use of pH strips and/or a PASCO probe. It was also necessary to titrate the unknown compound to find the equivalence point, which would allow the calculation of the initial concentration of the unknown chemicals. In order to see how dilution affected the pH of the unknown compound, it was necessary to dilute the unknown compounds over a series of steps and observe the trend. Finally, it was helpful to test the household chemicals for their acidic or basic properties and compare how they reacted to the reactions of the unknown compounds.

Purpose: As there were four different parts, each one had a specific goal. Part 1 was to identify over-the-counter drugs that are easy for the average person to obtain. Drugs like aspirin, acetaminophen, sodium bicarbonate, and effervescent antacid were tested with H2O, pH, HCl, and FN to see if there was a reaction. This helped to determine the unknowns.

The second data table provides the results of all the brand antacids, including Medique Alcalak and Alka Seltzer, and the average of Gelusil. The results also include the initial moles of HCl used, average volume of NaOH used, moles of NaOH used, and moles of HCl neutralized by antacid. In the experiment, according to the data, the Medique Alcalak neutralized the most moles of HCl while the generic antacid followed suit. Then, the Alka-Seltzer neutralized the second least amount of HCl followed by Gelucil. As a note, because two groups were assigned to the Gelusil brand antacid to run their own trials and calculations, the class was instructed to calculate the average of their results. Furthermore, there was a substantial difference between the two results and the difference can be attributed to the differing amount of mL NaOH they may have used to titrate with. Additionally, a rough trial was performed during our experiment which ended up providing an opportunity to see how much NaOH was needed for titration before it became purple and too basic. The group named this the rough trial as we recorded the largest possible amount of NaOH used to make the solution to basic, 6 mL, and used that as a benchmark for the future so that the rest of the trials will be successful. Likewise, the trials recorded were more precise as the titration method was performed much more

A suitable indicator for determining the endpoint in the neutralization of a weak acid with a strong base is phenolphthalein. Phenolphthalein has a pH range of 8-10. It is colorless in acidic and neutral solutions. According to the titration curve of a weak acid-strong base titration, the pH at the end point is basic. Phenolphthalein only changes color when the solution becomes basic. Hence, it is an ideal indicator for this lab because it will change color when the end point is reached.

able to neutralize the greatest amount of HCl, I will compare it to the others to determine/prove

It occurs when enough base is added for a neutralisation reaction to occur. The equivalence point between a weak acid and a strong base is pH 8.72. It must be attained precisely to produce accurate results. This is done by slowly adding the titrant to the analyte. The end point of the experiment refers to the point at which the indicator changes colour because of an indicator. The indicator phenolphthalein has a pH range of 8.2 to 10.0 and is used to determine the endpoint as it shows when enough of the base has been added to fully react with the acid. It remains colourless in an acid and when neutral, however, when the solution becomes basic, it turns pink. When it turns a pale pink, the endpoint has been reached and the amount of base can be determined, and the concentration of acid can be found. However, if the solution is overly titrated, it will turn a bright pink. This means that the results are no longer precise nor accurate. When the endpoint has been reached, the amount of base used can be determined, and thus the concentration of the acid can be found using

The purpose of this experiment was to find the molarity of a concentration and the acid-base titration. In part A of this experiment, the molarity of an assigned concentration which was 0.040, was found using formulas that represent molarity. Part B of this experiment, which was titration of an acid and base, was found by a series of steps that involved dropping Sodium Hydroxide from a buret into vinegar, until the perfect shade of pale pink occurred. With the Phenolphthalein, too much acid causes the base to turn a dark pink. The molarity was then found of the titration. So the end results will determine M HCH3O2.

In a chemical reaction with an acid and base combination, the base neutralizes the acid. Antacids follow this process once entered your body to soothe an upset stomach during heartburn. The scientist’s hypothesis is if a brand uses the least amount of average drops to neutralize the acid, then it is most potent. In order to test the hypothesis in the scientist’s experiment, they will test different brands of liquid antacid against each other to find out which is most potent in neutralizing lemon juice (acid). They will do this by having 3 different graduated cylinders, each filled with 10 drops of non-sugar grape juice (a natural acid-base indicator which changes color based upon what the pH of another liquid is when it makes contact with it) and 10 drops of lemon juice (acid). Each brand will have its own graduated cylinder. For

Diluted essence (10ml, 100 times diluted) was pipetted into a 100ml separating funnel. 20ml of dichloromethane was added to the diluted essence. The funnel was then shaken vigorously for 2 minutes with gas being release occasionally. The organic phase (lower layer) was released into a 100ml beaker and another 20 ml of dichloromethane was added to the funnel and shaken vigorously for another 2 minutes. The organic phase (lower layer) was again released into the 100 ml beaker. The contents of the funnel were disposed of. The organic phase was then added back into the separating funnel with 40ml of 0.1M sodium hydroxide solution and shaken well for 2 minutes. The organic phase was released and disposed of and the aqueous phase was kept and transferred to a 250ml volumetric flask and the volume was made up with 0.1M sodium hydroxide. Standards were then made using the 50mg/L standard provided and mixing with 0.1M sodium hydroxide to create standards with 1,2,3,4,5 mg/L concentrations. Each solution was run through the UV – Visible spectrometer to find the absorbance and then the concentration.

In a titration, an exact volume of one substance(NaOH) was reacted with a known amount of another substance (HCl). The point at which the reaction was complete in a titration is referred to as the endpoint. We recognized a solution which reached the endpoint: when we saw a solution completely turned into pink color. A chemical substance known as an indicator was used to indicate the endpoint. An indicator is a substance that undergoes a distinct observable change (pink color) when conditions in its solution change. The indicator we used in this experiment was phenolphthalein because Phenolphthalein is a weak acid. The weak acid is colourless and its ion is bright pink. And the solution turned pink when we added a basic solution (NaOH) into the solution because adding hydroxide ions removes the hydrogen ions from the equilibrium which replace them turning the indicator

which would have only surface-seeded cells. The well plate was wrapped in Parafilm to prevent