Purpose: The purpose of our experiment was to precipitate Copper (II) Phosphate Trihydrate and determine percent yield, also to react an aqueous solution of Copper (II) Chloride with aqueous Sodium Phosphate and describe the reaction. Procedure: To conduct our experiment 10 milliliters of CuCL2 and 8 milliliters NaPO4 was added to its own 50 milliliter beaker. These solutions were then combined in a 150 milliliter beaker and mixed for 1 minute. The PH of the mixed solution was checked to see if it was accurate enough to go on with the experiment. The solution was then filtered using the vacuum filtration technique.…
A possible chemical reason that this experiment yielded less than 100% cyclohexanone was due to the spontaneous decomposition of sodium hypochlorite, 2NaOCl = 2NaCl + O2, which decreased the amount of reactant present in the initial reaction when hypochlorous acid was formed, which was the oxidizing agent required to oxidize cyclohexanol into cyclohexanone. Sodium hypochlorite decomposed into O2 and NaCl due to a multitude of factors such as exposure to high temperatures, prolonged storage time or sunlight exposure. If a large enough quantity of the sodium hypochlorite was decomposed to limit the reaction that produced hypochlorous acid, the quantity of cyclohexanone produced may be affected. This would have resulted in a decrease in the production…
This lab makes use of the reaction excess powdered calcium carbonate and different concentrations limiting hydrochloric acid in order to determine the effect of changing concentration on the rate of the reaction. Students will carry out 3 trials of 5 experiments each trial. The five different experiments are for the various concentrations of hydrochloric acid (0.2, 0.4, 0.6, 0.8, 1.0 mol/L). First measure out approximately 2 grams of powdered calcium carbonate using a weighing boat and analytical balance. Then, measure out 30 mL of 0.2 M hydrochloric acid into a volumetric flask.…
A graduated cylinder was used to measure 200mL of distilled water into an Erlenmeyer flask and then 40mL of 0.6 M NaOH was added to the distilled water in the flask. The flask was then plugged with a rubber stopper and shook in order to mix the solution. A buret was then washed, rinsed with distilled water, and then 5 mL of the NaOH diluted solution. After the cleansing of the buret, it was then filled up with the NaOH diluted solution. The dilution of the solution was calculated to find the molarity of the NaOH.…
Hypothesis: If different concentrations of aqueous 〖"NaHCO" 〗_"3 " are tested, then a 2.0 M concentration of 〖"NaHCO" 〗_"3 " will reduce the tarnish on sterling silver the…
The iodide’s position is opposite of the –OH group. Salicylamide and sodium iodide are dissolved in ethanol, and stirred and cooled to 0. After that household bleach was added while stirring vigorously, solution changed from colorless to pale yellow. Sodium thiosulphate and hydrochloric acid were added aswell.…
Visual comparison of the available solid and aqueous compounds to the unknown was done first so as to eliminate unnecessary testing. A 30.0 g/mL solution of the unknown was made in a beaker by dissolving 1.000 g of the unknown in 30.0 mL of distilled water. Before weighing out 1.000 g of the unknown, the scale was zeroed out with a piece of weighing paper (square cut-out of normal paper) on it. Using a scoopula, 1.000 g was the compound was carefully placed on the weighing paper and measured to exactly 1.000 g. These same measurements and procedures were used when solutions of calcium chloride and nitric acid were created using separate beakers. Portions of each solution were then poured into test tubes (exact measurements were not necessary for this step).…
When hydrochloric acid was added to the unknown and known solutions, both resulted in no reaction. This also occurred when potassium hydroxide was added to both of the solutions. Barium chloride was then added to the two solutions, which resulted in a cloudy white precipitate from both of the solutions. A cloudy white precipitate also formed when calcium nitrate and ammonium nitrate were added to both the unknown and known solutions. These reactivity tests were conducted in order to establish how the unknown compound would react with acids, bases, and salts.…
A Hydrate’s Empirical Formula Aaron Meehan Ethan 11/06/17 Kotiba 09J I have read and agree to the terms of the Academic Honesty Statement. _ Aaron Meehan____________11/06/2017 _____________________ Student Signature…
Do mole ratios affect the amount of reactant that is produced? This experiment tested why mixing reactants in different mole ratios affected the amount of the product and the amount of each reactant that is left over. To solve the problem, the lab contained reacting sodium bicarbonate(baking soda) and acetic acid(vinegar) in different ratios and seeing if the product changed. The data suggests that the higher ratio of baking soda to vinegar creates the most product. For the ratio 3:1, the final grams of sodium acetate(product) was 0.09, the product of 1:2 was 0.52, while for the ratio 1:3, the final grams of the sodium acetate was 1.65.…
There have been many great articles that have been published over the years . There are also many great authors such and Pam Munoz Ryan and Jennifer L. Holm. These two magnificent writers have produced many great articles. These authors have produced two very good articles such as “Freddie in the Shade” and Follow the Water”. Jennifer L. Holm is an American children's writer , and a person who won three Newbery Medals for her writing.…
b. Add two drops of 6.0M HCl(aq), 0.5mL 10% Hydroxylamine-HCl, six drops 2.0M Sodium Acetate, and 1.0mL 0.1% 2,2-Dipyridyl solution to the test tube. c. Fill the test tube to the 10mL mark with DI water and the color will fully develop in 15 minutes d. Prepare the four other standard solutions with appropriate amounts of the solutions. 9. The sample uses 2.0mL from the volumetric flask with the dissolved Fe and add the appropriate reagents. 10.…
Reaction Scheme: Procedure: The procedure for this experiment was drawn from Wissinger laboratory manual.1 The only deviation from this procedure was that the Variac outlet for the Reflux condenser was set at sixty for fifty minutes rather than at forty-five to fifty for sixty to seventy-five minutes. For the sodium bicarbonate washes, four washes were completed before the solution was deemed no longer acidic. As well, for the NaCl wash, 10mL of aqueous NaCl solution was used.…
Racheal A. Krasner Professor Garfield Beckford CHEM 1211 L 25 September 2015 Lab Report Concerning Acid-Base Titrations The purpose of this experiment was to recognize the procedures for conducting acid-base titrations. Each acid-base titration used one solution to analyze another; it also involved the use of an indicator, which denoted the endpoint of the titration. The indicator used was phenolphthalein; it produced a pink hue when the titrations reached their endpoints – between pH 8 and pH 10.…
Experiment Summary The purpose of this experiment was to determine the copper content of brass using iodometry. This was accomplished by creating a thiosulfate solution and standardizing it by titrating using a known amount of KIO3. The second part of the experiment involved preparing a brass sample and allowing copper to react with excess iodide to form I2. The resulting I2 was then titrated with the thiosulfate standard.…