Tom Nguyen Mike Noah University of Central Florida 07/03/17 Analysis of Antacids to Determine Which is the Most Effective at Neutralizing Stomach Acid Abstract: This experiment was performed to determine the factors of an antacid that lead to stomach acid neutralization. Multiple over the counter antacids were tested for each lab group along with Sodium Hydroxide (NaOH) being identified as the titrant and Hydrochloric acid (HCl) being identified as the analyte for the reactants. Each antacid was crushed and mixed into 120 mL of HCl using a pestle and mortar with a graduated cylinder followed by heating up the solution to remove carbon dioxide. The initial and final volumes of NaOH were compared after the solution was titrated in five different …show more content…
This was due to the indicator changing color as the solution approached its end point. The solutions that turned dark pink passed their end points, meaning that the number of moles of acid and base were surpassed and not at equality. The solutions that turned light pink were near the end points, meaning that the number of moles of acid and base were very close to equality. The first step in determining which antacid has the best at neutralizing the hydrochloric acid was to calculate the average amount of moles of acid left in the Erlenmeyer flasks after titration. Since at the equivalence point the number of moles of base is equal to the number of moles of acid, the known moles of base used can also be used as the known moles of acid left in the flasks. There are further steps that have to be taken to find the amount of moles neutralized by the antacid. First, the average was calculated by adding all of the number of moles of NaOH from each of the trials then dividing it by 5 (which represents how much trials there were) to get a total of 0.00129 moles. After receiving the average, you multiply the 0.00129 moles by 6 (which was the total number of antacids available for the experiment) and then subtract that total from the original amount for the moles of HCl used in the beginning of the experiment (which was 0.0180) to determine exactly how many moles of acid were neutralized by the sodium hydroxide which calculated to be 0.0103 moles. As Table 2 shows, the antacid, which neutralized the most number of moles of HCl was Alcalak with 0.0103 moles
barbier reaction: In a 50 mL round bottom flask that had a reflux condenser attachment, saturated ammonium chloride (5 mL), THF (1 mL), zinc powder (0.4 g), benzaldehyde (0.500 mL, 0.5225 g, 4.92 mmol), and allyl bromide (0.470 mL, 0.6533 g, 5.40 mmol) were charged with stir bar and stirred at room temperature for 45 minutes. Diethyl ether (10 mL) was added to the reaction mixture and stirred. The mixture was gravity filtered into a beaker that was topped with a watchglass. The filtrate was transferred to a separatory funnel and the organic layer was extracted with deionized water (10 mL) and diethyl ether (15 mL). The organic layer was placed into an Erlenmeyer flask and the aqueous layer was placed into a beaker, which was extracted with
Cu (aq) + 2NO3 (aq) + 2Na+ (aq) + 2OH- (aq) → Cu(OH)2 (s) + 2Na+ (aq) + 2NO3(aq)
We were then to make a base solution of 0.7 M NaOH. In order to standardize
Apparatus: * 1 measuring cylinder * 1 test tube * 1 stop clock * A large gelatine cube containing indicator and NaOH * Hydrochloric acid ranging from 1-3 molars * A scalpel Diagram: Method: * Take the large gelatine cube and cut into 15 equal pieces * Place on piece of the cube into the test tube * Measure out 10mls of HCl in the measuring cylinder * Pour the HCl into the test tube with the gelatine cube and start the clock * Time how long it takes for the pink colour inside the gelatine cube to completely disappear * You will also notice that the cube dissolves slightly * Record your results and repeat this same process 3 times for each molar of acid: § 1 molar § 1.5 molar § 2 molar
Purpose/Introduction: In this experiment, four elimination reactions were compared and contrasted under acidic (H2SO4) and basic (KOC(CO3)3) conditions. Acid-catalyzed dehydration was done on 2-butanol and 1-butanol; a 2o and 1o alcohol, respectively. The base-induced dehydrobromination was performed on 2-bromobutane and 1-bromobutane isomeric halides. The stereochemistry and regiochemistry of the four reactions were analyzed by gas chromatography (GC) to determine product distribution (assuming that the amount of each product in the gas mixture is proportional to the area under its complementary GC peak).
The above equation tells us that 1 mole of calcium hydroxide reacts with exactly 2 moles of hydrochloric acid, so we should try to make the solution of HCl about twice as concentrated as the Ca(OH)2, so that when we measure out, shall we say, 10 cm3 of the calcium hydroxide solution into the flask we should need to add approximately 10 cm3 of hydrochloric acid from the burette.
Text Box: The results collected in the experiment have been shown on a graph. The graph shows a temperature increase up to 26.9oC. This was taken when 28cm3 of HCL was added to the solution. This is where neutralisation has occurred. After this point the temperature slowly decreased.
The same procedure was done using 10ml of CV and 20ml of sodium hydroxide, both separately diluted to 50ml and added in a large beaker. The absorbance was recorded. In the last trial, 10ml of CV, 10ml of NaOH were diluted to 50ml. Before adding the two mixtures, 1ml of soap was added to the NaOH solution and then poured into a large beaker, along with the CV. Absorbance was recorded and the materials
The concentration of calcium hydroxide at the beginning will be: 1.5 / 74 = 0.02 So, the concentration is 0.02 mol/dm3 In the experiment I will be using 25cm3 of the solution from the volumetric flask, so the mass of the calcium hydroxide in one titration will be: 0.375 / 10 = 0.0375g Therefore the number of moles of calcium hydroxide: 0.0375 / 74 = 0.0005 moles Ca(OH)2(aq) + 2HCl à CaCl2(aq) + 2H20(l)
In 1957, two sociologists, Gresham Sykes and David Matza, developed a theory in regards to people neutralizing deviance. This theory represents as the five Techniques of Neutralization. “Through the use of these neutralizations social and internal controls that serve to check or inhibit deviant motivational patterns are blocked, thereby allowing individuals to engage freely in delinquency without serious damage to their self-image” (Copes). Sykes and Matza outlined five neutralization techniques: denial of responsibility, denial of injury, denial of the victims, condemnation of the condemners, and appeal to higher loyalties. Sykes and Matza studied juvenile delinquents’ behavior to understand the denial process and explain that their improper behavior can extremely benefit amongst other social groups.
Areia Falahpour University of Central Florida CHM2046L 29 June 2017 Antacids Abstract The purpose of this experiment was to answer the question of which antacid is more readily or in other words the best at neutralizing stomach acid. This experiment is insightful and the importance of this experiment is that humans have a strong acid within the epigastric region or stomach known as hydrochloric acid (HCl). HCl is essential as the body uses it to digest the food that comes through the epigastrium.
Analysis of Aspirin Tablets Aim --- To discover the percentage of acetylsalicylic acid in a sample of aspirin tablets. ----------------------------------------------------------------- In order to do this, the amount of moles that react with the sodium hydroxide must be known. This is achieved by using the method of back titration.
Titration is a technological process in which a solution, known as a titrant, is slowly and carefully added from a burrette into a fixed volume of another solution (known as the sample). In an acid-base titration an acid neutralizes a base or vice versa. This process is maintained untill the reaction between the titrant and the sample (acid and the base) is judged to be complete. The reaction is judged to be complete when the endpoint is reached. An endpoint in a titration analysis is referred to as the point at which no more titrant is added due to an observable colour change of an indicator. Indicators can be used to find an endpoint because they change colour when the pH of a solution changes and an endpoint in a titration is an empirical approximation of the equivalence point, which is the point of major pH change in the titration sample due to the fact that equal chemical amounts of reactants have been combined at that point. All indicators have a pH range, which is the range of pH values at which the colour of the indicator changes. Thus
The question that was proposed for investigation was: Can the exact concentration of 0.1M sodium hydroxide solution be determined by titration (Lab Guide pg. 141)?
Antacids reduces the amount of acid produced by the stomach. They can help relieve heartburn. There are many different types of nonprescription acid reducers in stores. Different ingredients can have different effects. Sodium bicarbonate antacids ( such as Alka-Seltzer) contain baking soda. People who have high blood pressure or on a salt restricted diet may want to avoid these because sodium bicarbonate antacids contain aspirin which is linked to Reye syndrome. Calcium carbonate antacids can be used as calcium supplements. Aluminum-based antacids are less potent and work slower than other antacids and can cause calcium loss. Antacids with alginic acid ( such as Gaviscon) contain a foaming agent that floated on the top of the stomach which helps keep stomach juices from coming in contact with the esophagus. ("Antacids and acid," 2010). Each antacid is slightly different from the next. Different ingredients can have different effects and defects, such as Gaviscon and Alka-Seltzer.