The compound that was assigned to be tested and the identity to be discovered was blue in color. Once 0.5028 grams of the blue compound was weighed out it was combined with 5 mL of distilled water. initially the unknown compound didn’t seem to dissolve in water. However, after a few minutes of constant stirring the substance dissolved completely. Thus indicating that the cation in the unknown compound was Cu2+. The identity of the cation had to be confirmed therefore a flame test had to be preformed. Once the solution was placed over the Bunsen burner the flame turned green confirming that the cation was Cu2+. To determine the character of the anion 0.1087 grams of the unknown compound, and 0.5109 grams of Na2CO3 was measured. Both solids were
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
The purpose of the Unknown White Compound Lab was to identify the unknown compound by performing several experiments. Conducting a solubility test, flame test, pH paper test, ion test, pH probe test, conductivity probe test, and synthesizing the compound will accurately identified the unknown compound. In order to narrow down the possible compounds, the solubility test was used to determine that the compound was soluble in water. Next, the flame test was used to compare the unknown compound to other known compounds such as potassium chloride, sodium chloride, and calcium carbonate. The flame test concluded that the cation in the unknown compound was potassium. Following, pH paper was used to determine the compound to be neutral and slightly
The primary goal of this laboratory project was to identify an unknown compound and determine its chemical and physical properties. First the appearance, odor, solubility, and conductivity of the compound were observed and measured so that they could be compared to those of known compounds. Then the cation present in the compound was identified using the flame test. The identity of the anion present in the compound was deduced through a series of chemical tests (Cooper, 2009).
Hypothesis: If the mystery powder is compared with the five known compounds, the mystery powder should match the one with the same physical and chemical properties. Also their reaction with water, universal indicator, vinegar and Iodine solution should match if an accurate experiment is conducted.
The purpose of conducting experiment was to determine the identity of white compound. Based on the 5 gram of unknown white compound several experiment conducted including solubility test, pH test, flame test, and ion test. Several materials including chemicals used throughout experiment and will be described through paragraphs.
Catching Fire: How Coooking Made us Human by Richard Wrangham is a fresh perspective on the evolution of humankind. Wrangham has made a concentrated effort to prove that humans have evolved particular adaptations, like bipedalism, due to the introduction of cooked foods into their diet. In his book, he is legitimately arguing that humans are the way they are because early on in human evolution, early man discovered fire, discovered the joys of cooked foods, and developed all sorts of fascinating traits still being utilized today.
This smoke bomb lab helped me understand chemical bonding and reactions by starting from the very beginning with mixing the nitrate, sugar, and melted crayon. Mixing them formed a texture almost like powdery peanut butter with some liquid which was actually pretty interesting. The second chemical bonding I seen was that, once putting the solution in the tin-can and it started solidifying due to all the stuff we mixed together. It didn’t take long at all for it to start forming into a solid. When we went outside and lit the wick on fire showed the main chemical reaction throughout the whole experiment. The nitrate reacting with the lighted wick started a big fire in one of the groups cans but some of the other groups bombs didn’t get to light like it was supposed to and the wick just burned out. I was one of the groups whose bombs didn’t work properly. I think it’s because we didn’t put the wick in deep enough to our solution so when we lit it the fire just burned out before going into the solution.
The experiment we did was Copper Cycle. We reverted the copper to its elemental form after a chain of reactions. We performed a series of reactions, starting with copper metal and nitric acid to form copper (ii) nitrate. Then we reacted copper with sodium hydroxide, sulfuric acid, nitric acid and zinc to form precipitates. In conclusion our percent recovery was 40.38%.
== = == Hypothesis for the experiment: After I conduct this experiment, I expect and suppose I can recognize and physical changes, identifying the difference these two kinds of changes. Also, I will be able to know some physical and chemical properties of copper (II) sulfate, water, iron, sodium carbonate, hydrochloric acid and magnesium and identify if it is a chemical change or physical change in each part of the experiment.
By doing this experiment, I can know the physical and chemical properties of these samples. After I get my results about the physical and chemical properties of these samples, I can compare my results with the information given by the past student and identify the 5 unknown samples, finding out which sample is which substance. Hypothesis = ==
The materials used in the previous were cleaned and dried. 10ml of CV was obtained along with 10ml of sodium hydroxide. These solutions were separately diluted to 50ml. A stopwatch was set up to record in 30second increments and the Spectrophotometer prepped for the cuvette. The following steps were done within 30seconds. The two solutions (CV and sodium hydroxide) were mixed in a large beaker. A pipette was used to deliver the solution into a test tube serving as the cuvette. The absorbance was recorded every 30second until 15minutes had passed and entered into a spreadsheet. All used materials were cleaned for the next trial.
... 45.5%, and a melting point of 92-98oC. The purified amount of acid was 0.124g,a percent recovery of 37.6%, and a melting point of 154-165oC. The purified amount of base was 0.206g,a percent recovery of 62.4%, and a melting point of 130-141oC. The purified amount of neutral was 0.023g,a percent recovery of 6.97%, and a melting point of 94-99oC. Percent recovery is based on fact that we have a 1:1:1 ratio. The percent recovery was established by dividing the purified or crude amount by the initial amount times 100. Since the percent recovery was high before recrystallization and low after recrystallization, some product must had been lost during recrystallization. After comparing the melting points of the acid, base, and neutral compounds I think that the acid was Salicylic acid, the base was 2-methyl-4-nitroanaline and the neutral was 9-fluorene.
With regards to Part B, once the initial two steps of this step were conducted, K2CrO4 was added. This reagent served to help identify whether Ca2+ or Ba2+ was present based on solubility and the presence of precipitate. On the principle of solubility, since the anion CrO42- forms mostly insoluble ionic compounds in water with most cations, Ca2+, could be identified due to that specific cation being one of the few exceptions.9 As a
No modification were made to this procedure as outlined in lab packets pages 17-18. The purpose of this advanced inquiry was to analyze the amount of copper in a brass sample using visible spectra. The percent copper in brass calculated was 84.2%. Finding the percent of copper was found by creating a calibration curve of various copper (II) nitrate solutions. This was used to create a possible range of copper ions when dissolving copper with nitric acid extending from 0.05 M to 0.4 M (Lab Packet). 10 mL samples of 0.05M, 0.1M, 0.2M, and 0.4M were created for the calibration curve. The ratio between Copper(II)Nitrate and H2O were found by using the following formula: M1V1=M2V2. This equation is utilized for dilutions and was used to find the volume of water and Copper(II)Nitrate. These solutions were then placed into the spectrometer to measure their absorbance of orange light (610nm). The 0.05 M solution had an absorbance of 0.063. The 0.1 M solution had an absorbance of 0.144 and the 0.2 M had an absorbance of 0.302. The last solution with a 0.4 M had a 0.598 absorbance. These data points created a line of best fit that showed the linear relationship between absorbance and concentration. The equation yielded was
The chemicals used were a metal oxide, in this case, copper oxide and a dilute acid, sulphuric acid, aiming to separate the copper and oxygen to collect the pure copper (II) ions, which is a soluble salt. The colour should be a very characteristic blue.