Lab Experiment to Identify Unknown Compound

Lab Experiment to Identify Unknown CompoundAbstract.The design of this experiment was to severalise the chartless conflate. The proves that were done to determine the identity of the mix include qualitative solubility try ons, quantitative solubility canvass, measuring stem conductivity, anion and cation adjudicate, ardour test, and formation of diminish. It was found that the mingled had no smell, was soluble in irrigate supply, and non soluble in toluene and acetone. The ions dissociated in the weewee, creating conductivity. When the ammonia test was per make no ammonia smell was pleadd. The blast test yielded a chroma that matched that of atomic number 11 bicarbonate indicating that the extraterrestrial blend contained atomic number 11. The anion test for chloride proved to be official, resulting in the summation that the unbeknown(predicate) merge was atomic number 11 chloride.IntroductionThe radical is employed by an Environmental Protection Agency to indentify a change in the landfill in your home town. The group must also tell on as m any(prenominal) chemical and physical properties of the commingle as we can. We get hold of to devise cardinal syntheses of the compound, and comp be them for cost effectiveness, safety, and potential yield of the compound. To identify the compound, the physical properties (smell, color, and state) need to be established. Next, the qualitative solubility of the compound was well-tried in water, toluene, and acetone, which would determine whether the compound would dissolve from rain water or other chemicals that may be place in the landfill and create runoff. conduction was also tested with a voltmeter in order to determine whether or not the compound would be dangerous when dissolved in water. If the compound was semiconducting it would dissolve in water and recruit an electric current. The ignite test was performed to specify one of the particles. A effect of water and the elemen t was utilise to place the nichrome wire in, and and then(prenominal) the nichrome wire is pose into the flame. If the flame produces a color it is indicative of a certain alloyloid ion or metal. A color is produced in the flame when the heat of the flame changes the metal ions into atoms which then become excited and produce light that can be seen with the naked eye. It is also important to analyze the presence of certain cations and anions use tests that identify the presence of the anions chloride and convert, and the presence of the cation ammonium ion. The anion tests for chloride and sulfate prove to be positive degree when a white go down forms and the ammonium test proves to be positive when an ammonium smell is produced. aft(prenominal) all of the physical and chemical tests were performed, a solution of the unusual region compound and a solution of what was deduced to be mystic compound were reacted with an erosive (nitric acid), a base ( kilobyte hydroxide) , notes nitrate, potassium sulfate, and potassium nitrate in order to determine if they produce the same results. gravimetric filtration was then performed with the known and unknown substance. A fall down was formed employ silver nitrate, which could then be weighed. After the filtration process, the unknown compound was then synthesized to produce a per centum yield.Results tabularise 1 Physical Properties shewColorWhiteState of MatterSolid looknoneSolubility in WaterSolubleConductivity0.35 voltsTABLE 2 Anion quizsTests PerformedResultsTest for ChlorideWhite Precipitate FormedTest for SulfateNo ReactionTest for NitrateNo Brown RingTest for CarbonateClearTest for AcetateClear, OdorlessTABLE 3 Cation TestsTests PerformedReactionResultsTest for AmmoniumNH4Cl + NaOH Ammonium SmellNo OdorFlame TestBright Orange/Yellow FlamesodiumTABLE 4 Reaction TestsType of ReactionBalanced parReactionAcidNaCl(aq) + HNO3(aq) - NaNO3(aq) + HCl (aq)NoneBaseNaCl(aq) + KOH(aq) - NaOH(aq) + KCl(aq )None treble transmutationNaCl (aq)+ AgNO3 (aq)- AgCl (aq)+ NaO3(aq)Precipitate formedDouble DisplacementNaCl(aq) + K2SO4(aq) - Na2SO4(aq) + 2 KCl(aq)NoneDouble DisplacementNaCl (aq) + KNO3(aq) - NaNO3(aq) + KCl(aq)NoneTABLE 5 Gravimetric AnalysisNaCl (aq) + AgNO3 (aq) - AgCl (s) + NaNO3 (aq) make clean Filtration audition Amount of Precipitate Produced (grams)Percent expectKnown Trial 11.08188.18 %Known Trial 21.19697.56%Unknown Trial 11.21198.78%Unknown Trial 21.18596.66%Unknown Trial 31.17095.44%TABLE 6 Synthesis ReactionReactionAmount Produced (grams)Theoretical Yield (grams)Percent YieldHCl (aq) + NaOH (aq) NaCl (s) + H2O (l)1.971298.55%DiscussionFirst, the physical properties of the unknown compound were observed and recorded. It was found that the compound was crystalline in structure, a solid, white, with no odor (Table 1). All of these properties suggest that the compound was bonce because loft compounds do not have a distinct odor and ar solid at room temperature bec ause of their high melting points. The unknown compound was then tested for solubility in water, toluene and acetone. The compound was soluble in water, indicating the compound was a charged or ionic compound, and not soluble in toluene or acetone which eliminates it being polar or nonpolar. Therefore, this points to the compound being ionic. After the compound was dissolved in water, the conductivity was tested with a voltmeter, which produced a voltage of 0.35 volts proving that the substance is conductive since it is over 0.1 volts. This further proves that the unknown compound was ionic since only ionic compounds dissociate in water and create an electric current.The flame test was performed to determine one of the elements in the compound. Four known compounds, sodium bicarbonate, atomic number 12 nitrate, calcium sulfate, and potassium nitrate were put under the flame test to compargon the unknown to. When the unknown compound was put under the flame test it produced the same color as sodium bicarbonate, bright orangeness/yellow, indicating the presence of sodium (Table 3). The ammonium test was also performed to verify that the compound did not contain ammonia. No smell was produced when the unknown solution and sodium hydroxide were abstruse, and a smell would indicate the presence of ammonia. Therefore, the compound was proved to contain sodium. When the anion tests for chloride and sulfate were performed, a white precipitate was produced from the chloride test, indicating the presence of chloride art object the sulfate reception created no precipitate indicating the absence of sulfate (Table 2).In addition, the unknown compound was put by means of a series of reactions along with what was believed to be the compound in order to compare the reactions to determine if they produce the same reactions. First sodium chloride, what is believed to be the unknown compound, and the unknown compound were reacted with silver nitrate, which produced a prec ipitate because it was a double displacement that produced AgCl which is not soluble in water. Sodium chloride and the unknown compound were reacted with potassium sulfate just now produced no reaction because the products sodium sulfate and potassium chloride are both soluble in water. Sodium chloride and the unknown compound were then also reacted with potassium nitrate, creating a double displacement reaction which produces sodium nitrate and potassium chloride, which are also both soluble in water, at that placefore producing no reaction. When sodium chloride and the unknown compound were reacted with an acid, nitric acid, but the presence of the sodium chloride did not affect the pH of the nitric acid because it was an ionic compound. When the sodium chloride and the unknown compound were reacted with a base, potassium hydroxide, there was also no reaction or change in the pH of the potassium hydroxide because the sodium chloride is an ionic compound. Both the sodium chloride and the unknown compound produced the same results in every reaction further proving that they are one in the same (Table 4). at a time it was found that sodium chloride and silver nitrate produce a precipitate when reacted, the reaction was used to produce a certain sum total of precipitate which was then used in gravimetric analysis to see if both the known and unknown compound would produce the same make out of precipitate. The reaction that was filtrated was NaCl(aq) + AgNO3 (aq) - AgCl (s) + NaO3(aq). The results from the known reaction were 1.77 grams of click paper and 1.081 grams of precipitate alone, while the theoretical yield was 1.225 grams. The unknown reaction has yet to be found. The percent yield for the reaction was 97.56% (Table 5).A deduction reaction was the final test preformed. The following chemical reaction occurred HCl(aq) + NaOH(aq) NaCl(s) + H2O(l). Once all of the water was evaporated out with the use of a hot central office, the precipitate was ab le to be weighed and the percent yield could be calculated. The reaction had a percent yield of 98.55% (Table 6).ConclusionAfter being employed by the Environmental Protection Agency, the group was able to identify the compound in the landfill. After all of the tests and reactions were performed, it was found that the unknown compound was sodium chloride. Its solubility in water, conductivity, and crystalline structure points to the fact that the compound is ionic. The positive flame test for sodium indicates that sodium is one of the elements in the compound because it produced a bright orange flame. The positive chloride test, when a white precipitate was formed, indicates that chloride is the due south element in the compound. The unknown compound and sodium chloride were put through the same reactions and consistently produced the same results, further indicating that the unknown compound is sodium chloride. The gravitational analysis of the known and unknown substances provide d similar results, backing up that the unknown substance was sodium chloride. The synthesis reaction produced a percent yield of 95.05%.Experimental ProcedurePhysical Properties Tests1. The physical state of the unknown compound was observed. This included the state of matter, smell (using the wafting technique), color, and structure.2. A low-pitched number of the unknown compound was determined in approximately 50mL of water and stirred to see if it would dissolve.3. The same solution was used for the voltmeter and the conductivity was recorded.Anion TestsChloride Ion Test nigh 1 mL of the unknown solution was pose in a test tube and 1 mL of 6 M HNO3 was added. After that another 1 mL of AgNO3 was added. Whether a white precipitate was formed or not was recorded. If a white precipitate is observed, a chloride ion is present in the solution.Sulfate Ion Test near 1 mL of the unknown solution was placed into a test tube and 1 mL of 6 M HCl was added. After that another 1 mL of Ba Cl2 solution was added to the same test tube. Whether or not a white precipitate formed was recorded. If a white precipitate is formed, sulfate is present in the solution.Cation TestFlame Test1. The heat from the Bunsen flame was used to cleanse the nichrome wire.2. A wasted inwardness of the unknown compound was placed onto the nichrome wire and held over the flame. The color of the flame was observed.Ammonium Test almost 1 mL of 6 M NaOH was added to 1 mL of the unknown compound solution. The waft technique was used to detect if there was any odor. If the smell of ammonia was present, there were ammonium ions present in the solution. reactivity TestsReaction with an AcidA solution with a lessened heart of unknown compound was mixed in 50 mL of water and a assort solution of a small amount of ammonium chloride and 50 mL of water. A small amount of the two solutions were placed in to two know apart test tubes and a small amount of HNO3.Double Displacement ReactionA solution of a small amount of unknown compound was placed into 50 mL of water and a separate solution containing a small amount of sodium chloride and 50 mL of water. A small amount of the two solutions was placed into two separate test tubes and a small amount of K2SO4 was added into severally test tube. The test tubes were then swirled and mixed.Double Displacement ReactionA solution of a small amount of unknown compound was mixed with a solution of 50 mL of water and a separate solution of a small amount of sodium chloride and 50 mL of water. A small amount of the two solutions were placed into two separate test tubes and a small amount of AgNO3 was added into each of the test tubes. The test tubes were then swirled and mixed.Double Displacement ReactionA solution of a small amount of unknown compound was mixed in 50 mL of water and a separate solution of a small amount of sodium chloride and 50 mL of water. A small amount of the two solutions were then placed into two separate test tubes and a small amount of KNO3 was added to each test tube. The test tubes were then swirled and mixed, and whether or not a reaction occurred was recorded.Reaction with a BaseA small amount of unknown compound was mixed with 50 mL of water and a separate solution of a small amount of ammonium chloride and 50 mL of water. A small amount of these two solutions were then placed into two separate test tubes and a small amount of KOH was added.Gravimetric Analysis1. A Buchner flask was used with a funnel placed over the top.2. The filter paper was weighed and then wetted with water slightly.3. The solution containing the precipitate was poured onto the filter paper and left until most of the tranquil had seeped through.4. The filter was then take from the funnel and placed into an oven for 10 transactions until the precipitate and paper had completely dried.5. The filter paper was then weighed with the precipitate still on top. The exercising weight of the filer paper was subtracted fro m the new weight to obtain the most accurate result.6. The procedure was completed three measure with the unknown substances and twice with a known substance.Synthesis Reaction1. Approximately 12.3 mL of ammonium hydroxide was mixed with 6.2 mL of hydrochloric acid in a beaker.2. The solution was placed on a hot plate (under a hood) and allowed to boil until all of the liquid evaporated.3. The remaining precipitate was removed from the beaker and weighed.ReferencesCooper, M. M., Cooperative Chemistry Laboratories, McGraw- Hill New York, NY, 2008.