The purpose of this experiment was to mix Alka-Seltzer with Hydrochloric acid in order to analyze Sodium Bicarbonate as an active ingredient in the Alka-Seltzer. The mixture will contain hydrochloric acid to only see the composition of Sodium Bicarbonate in the tablet once it reacts. The amount that reacted allowed
Amount of Water Colin Lee Dr.Cooper Chemistry 12 Introduction: Alka-seltzer contains three active ingredients, aspirin, sodium hydrogen carbonate and citric acid. It is used for headaches, migraines, and cold and flu symptoms. Alka-Seltzer is usually taken when dissolved in a glass of water. When placed in water a series of chemical reactions result into Sodium citrate and Sodium acetylsalicylate. The sodium citrate would act as the antacid for stomach pains, and the sodium acetylsalicylate would act as the pain reliever.
Alka Seltzer is a medicine that acts as a pain reliever and an antacid. Antacids are used to help neutralize the acids in the stomach and help treat acid reflux, heartburn, indigestion, and gastritis. The tablets contain sodium bicarbonate (NaHCO3) and citric acid (C6H8O7). The sodium bicarbonate is a base that helps neutralize the acids in the stomach, mainly hydrochloric acid (HCl). It does this by the following reaction: Na3C3H5O7(aq) + 3HCl(aq) H3C3H5O7(aq) + 3NaCl(aq). When the tablets are dropped into the water, a reaction occurs in which water (H2O), sodium citrate (Na3C6H5O7), and carbon dioxide (CO2) are formed.
An Alka Seltzer is a white, solid, odorless tablet that is used in our daily life. For the most part it is mainly used for temporary relief on heart burns, acid indigestion, upset stomachs, headaches and pain in general. The purpose of the lab conducted was to show the fastest way on can dissolve an alka seltzer tablet using different liquids. The liquids used were regular tap water, Sprite and Minute-Maid Apple Juice. So, if we use different types of liquids to see which will dissolve the alka seltzer the fastest, then out of the three liquids water will take the least amount of time to fully dissolve the tablet because it is the most recommended liquid to take with any
The mass of the small beaker/flask and solution for each trial was found and recorded by using 50 mL graduated cylinders to add increasing 5 mL increments of vinegar, from 0 to 35 mL, and decreasing 5 mL increments of water, from 35 to 0 mL to the eight small beakers or flasks and weighed on an analytical balance. Accordingly, the mass of each of the eight Alka-Seltzer Tablets was determined and recorded. Moreover, the tablets were each dropped in their respective beakers/flasks, and allowed to fizz, without spilling over. The loss of mass of CO2 was furthermore ascertained by finding change in mass of each of the solutions after the fizzing stopped from the value of the mass of the Alka-Seltzer tablet plus the mass of the solution and beaker/flask. Further, using the loss of mass of CO2 for each trial and the balanced equation, the amount of NaHCO3 reacted and percent by mass in the tablet were identified. After determining the class average and the standard deviation for each trial, and plugging it into a scatter plot, the change of slope showed the true percent by mass of NaHCO3 in Alka-Seltzer tablets.
he experimental variable in this experiment was the changing number of Alka Seltzer tablets that were put into the 250mL beaker of vinegar. Some of the control variables in this experiment were that the same beaker and thermometer were used for each trial, the same type of vinegar and Alka Seltzer were used for each trial, and the same amount of vinegar. The original Hypothesis was that more Alka Seltzer would increase the temperature of the vinegar was not correct. After analyzing the data it can be seen that for the first trial the temperature did not change as it stayed at 24 degrees Celsius before and during the reaction with 1 tablet, also for trial two with two tablets the temperature stayed the same at 23 degrees Celsius and did
Subsequently, HCl was added, drop-wise, to the labeled NaHCO3 extract. Once the solution had a pH of 2, additional HCl was not needed: 3-chlorobenzoic acid was precipitated. An ice-water bath beaker (250 mL) was made to cool the acidified solution. Eventually, a Buchner filtration apparatus was assembled with a pre-weighed filter paper; not to mention, wetted in the apparatus. Then the apparatus was attached to a water aspirator and the water valve was opened.
Stoichiometry and Determining the Limiting Reagent Abstract: Four chemical reactions will be done using different ratios of mixture between calcium chloride and sodium carbonate. The mixture of these two substances produces the precipitate calcium carbonate, which will be separated using filtration. After observing the tubes and collecting data, the limiting reagents were deduced from observing which amount of substance had the least amount of moles. It was found that in trials one through three, the limiting reagent was calcium chloride and in trial four, the limiting reagent was sodium carbonate. The actual yield in grams were compared to the theoretical yield in grams of product to provide percent yields of 63.89 %, 88.67 %, 89.6%, and
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
Experiment to investigate the amount of sodium hydroxide needed to neutralize the solution of vinegar CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l) (Reaction between sodium hydroxide and solution of vinegar, which produces an aqueous solution of sodium acetate and water) Hypothesis: Approximately 8.8ml of sodium hydroxide will be
Discovering the Concentration of Sodium Hydroxide and Citric Acid Introduction: This laboratory experiment focuses on determining the quantity of a substance that is existing in a certain solution, by using titration in the experiment, (French et al. 2014). A hypothesis for this experiment is that the unknown concentration of a solution will be identified. The objectives are to identify the concentration of citric acid and the concentration of sodium hydroxide in solutions of unknown concentration. In order to discover the concentration of a solution, acid-base titration must be executed during the experiment, (French et al. 2014). The standard solution (known concentration) is reacted entirely during titration due to stoichiometry located in the equation, and because the chemical reaction is between a base and an acid, the products formed from the reaction will be salt and water, (French et al. 2014). The equivalence point occurring in an acid-base titration will have the same amount of moles in H+ as in OH-. The equations that are used for this acid-base titration are as follows:
Another source of error that was present in the investigation was rinsing the flasks between use. For example, the team members will rinse out the flask after testing it into the sink and then rinsing the insides with distilled water. However, it was difficult to dry the insides, so when reusing the flask, there may be extra residue of distilled water