Development of an Equation Essay

Purpose Investigate a chemic reply using lab procedures and observations. Then, find a pattern of reactivity and exempt the findings using a chemical equation and snap officle diagram. Procedure evoke to De situationment of Chemistry, The Ohio State University. Development of an Equation. General Chemistry 1210 Laboratory Manual. Vol. 2013-2014. Plymouth Hayden-McNeil. 32-35. info/ResultsPart A In the honey oil iodide dissolver, I think thither were super acid atoms as well as iodin atoms. In the chip in nitrate dissolver, I think there were go away and nitrate ions. The cat valium atoms and the sensation atoms can be classified as cations, since they are metals. The iodine atoms and the nitrate ion can be classified as anions since they are nonmetals. Upon mixing, the ancestor rancid into a deep colour deform. Evidence that a chemical reaction occur personnel casualty was that the two solutions created a new color because the two solutions were primarily colorl ess. in that respect was no gas make. Part B(Testing the Anions)Iodide reaction with enthalpy peroxide observations- The precipitous at the bottom turned into a florid solid and the liquid solution was a dirty yellow color. treat reaction with hydrogen peroxide observations- A colorless pass create at the bottom and looked like a bubble. It was a relatively tumescent bubble. The liquid solution was colorless and cloudy/fizzy. Since the reaction resulted in rough fizzing and bubbles, this is indication that a gas was form. (Testing the Cations)Potassium reaction with thioacetamide observations No reaction occurred. Lead reaction with thioacetamide observations A violet-black sicken formed at the bottom of the footrace underground and the liquid solution was a cloudy grey color. It was about the identical size come down as the nitrate reaction with hydrogen peroxide. Strong smell from the thioacetamide.Part C identification of ions in the precipitate that forms when continue nitrate solution is added to yard iodide solution. (Testing for Anions)chemical reaction with hydrogen peroxide observations- A dark red precipitate formed at the bottom of the strain supply and the liquid solution was colorless. There was not a large amount of precipitate formed and it classification of smeared along the inside of the try on tube. Inferences What anions are in the precipitate? -iodine (I-) When compared with results from type B to test anions, similar results were plunge. A dark red precipitate was formed in two.(Testing for cations)Reaction with hydrogen sulfide observations- A small, violet-black precipitate formed at the bottom of the test tube and the liquid solution was grey and cloudy. Inferences What cations are in the precipitate? lead (Pb2+) When compared with results from fall apart B to test cations, similar results were form, A violet-black precipitate was formed in both tests. Exchange reaction- Positive potassium started off with n egative iodine, and positive lead started off with negative nitrate. Potassium switched to desegregate with nitrate and lead switched to combine with iodine. Part DTesting of accrue Observations on Initial Precipitate Formed (relative amount, etc.) Lead Nitrate Potassium Iodide Ratio Tube 1 Powdery, yellow precipitate formed at the bottom. Not very oft precipitate. Little to no streaking. Clear liquid solution to a higher place precipitate. 31 Tube 2 Powdery, yellow precipitate formed at the bottom. Equal to tube 1. Little to no streaking. Clear liquid solution higher up precipitate. 21 Tube 3 Powdery, yellow precipitate formed at the bottom. A undersize more precipitate than tube 1 and 2. Little to no streaking. Clear liquid solution above precipitate. 11 Tube 4 Powdery, yellow precipitate formed at the bottom. Much more than tube 3. Noticeable streaking of precipitate along sides of test tube. Clear liquid solution above precipitate. 12 Tube 5 Powdery, yellow precipitate fo rmed at the bottom. more or less precipitate formed out of all test tubes. A deal out of streaking of the precipitate along sides of the test tube. Clear liquid solution above precipitate. 13Testing of Supernatant Observations Inferences Which ions were in the supernatant? appoint cations and anions. Tube 1 The solution was illuminate with lead nitrate, but turned a yellow cloudy color with the potassium iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 2 The solution was clear with lead nitrate, but turned a yellow cloudy color with the potassium iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 3 The solution was clear with lead nitrate, but turned a yellow cloudy color with the potassium iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 4 The solution was clear with both the lead nitrate and the potassium iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 5 The solution was a little yellow with the lead nitrate, and a little less yellow with the potassium iod ide. K+ (potassium)I- (iodine)Discussion/Conclusion In part A, the first metre was to obtain 5 drops of potassium iodine and 5 drops of lead nitrate and put them into a test tube and record observations. Then, to test the anions in part B, 5 drops of potassium iodine, 5 drops of nitric, 10 drops of dichloroethane, and 5 drops hydrogen peroxide to a new test tube. Then to a bring out test tube, 5 drops of potassium nitrate, 5 drops of nitric acid, 10 drops of dichloroethane, and 5 hydrogen peroxide to a new test tube. Both should be stoppered and shook to produce two distinct stages. To test the cations, 2 test tubes would each get 20 drops of thioacetamide and 2 drops of nitric acid. angiotensin-converting enzyme would get 5 drops of lead nitrate and the other 5 drops of potassium nitrite. Both test tubes were heated for 5 minutes and observations were recorded. In part C, the sample was used from part A and the test tube was centrifuged, thus the clear aqueous layer was remove d and discarded and the precipitate was washed with distilled water. This process was repeated once more. To test the anions, 5 drops of nitric acid, 10 drops of dichloroethane, and 5 drops of hydrogen peroxide were added to the solid precipitate and the test tube was stoppered and shook.These results were compared to the results from part B. To test for cations, the less colored aqueous layer was transferred to a clean test tube and the leftover layer was discarded. The solution was heated in a water bath until clear. 20 drops of thioacetamide were added, wound up then heated in a water bath and compared to the results from part B. In part D, to determine the proportionality of ions in the precipitate, 5 test tubes were labelled 1-5 and were filled according to table 3.1 on page 34 of the lab manual. The same medicine dropper was used for all drops and the test tubes were stoppered and shook, then centrifuged. The relative amounts and appearance of each precipitate were reco rded. To test for potassium of iodide ions in the supernatant, 5 drops of lead nitrate were added to 5 disjoint test tubes with along with 5 drops from the appropriate test tube solution. The same was done to test for lead or nitrate ions, but potassium iodide was added instead. The perfect ratio for this lab was 2 potassium iodides for every lead nitrate. This ratio was found from balance the equation and from comparing the results from part C to part B to match the observations of the precipitates.The ratio is the molar mass ratio of the balanced equation. The balanced equation was 2KI(aq)+Pb(NO3)2(aq) 2KNO3(aq)+PbI2(s) and the formula of the precipitate was PbI2(s) based on the observations. In part B, the test for anions resulted in a dark red precipitate which was the iodide solution with hydrogen peroxide. In part C, the same results were found when lead nitrate and potassium iodide were added to hydrogen peroxide, therefore the anions found were iodide ions because it has a negative 1 charge. In part B to test cations, the precipitate was a violet-black color for the lead solution reaction with thioacetamide. In part C, the same results were found when lead nitrate and potassium iodide were added to hydrogen sulfide.The cations found were lead ions since they view a positive 2 charge. just about intrinsic errors could have been while extracting the clear aqueous solution, some of the precipitate could have been extracted with the solution and transferred into another test tube. Upon heating, not all of the precipitate dissolved. Some of the drops with the micropipet varied also. The medicine dropper was more precise with the drops. Through this lab, a chemical reaction was used to find the pattern of reactivity which was an commutation reaction. This is known by finding the chemical equation and properly balancing it which is seen above. This lead to the ability to create a particle diagram and the findings of a perfect ratio of lead nitrate to po tassium iodide.