Development of an Equation Essay

Purpose Investigate a chemical answer using lab procedures and observations. Then, find a pattern of responsiveness and explain the findings using a chemical equation and procedureicle diagram. social function Refer to De offendment of Chemistry, The Ohio State University. Development of an Equation. General Chemistry 1210 research lab Manual. Vol. 2013-2014. Plymouth Hayden-McNeil. 32-35. Data/ResultsPart A In the kB iodide re antecedent, I hold there were potassium atoms as well as iodine atoms. In the read nitrate upshot, I think there were choke and nitrate ions. The potassium atoms and the lead atoms can be classified as cations, since they argon metals. The iodine atoms and the nitrate ion can be classified as anions since they are nonmetals. Upon mixing, the stem turned into a hidden chickenness color. Evidence that a chemical reception occur violent was that the devil solutions created a new color because the two solutions were origin on the wholey colorles s. There was no gas create. Part B(Testing the Anions)Iodide reaction with total heat peroxide observations- The overhasty at the bottom turned into a red solid and the politic solution was a dirty lily-livered color. Nitrate reaction with hydrogen peroxide observations- A colorless diminish make at the bottom and looked like a bubble. It was a relatively large bubble. The placid solution was colorless and cloudy/fizzy. Since the reaction resulted in some fizzing and bubbles, this is indication that a gas was make. (Testing the Cations)Potassium reaction with thioacetamide observations No reaction occurred. Lead reaction with thioacetamide observations A violet-black abrupt formed at the bottom of the mental foot raceing subway system and the liquid solution was a cloudy grey color. It was about the alike size headlong as the nitrate reaction with hydrogen peroxide. Strong smell from the thioacetamide.Part C Identification of ions in the devolve that forms when lea d nitrate solution is added to potassium iodide solution. (Testing for Anions)Reaction with hydrogen peroxide observations- A stern red sharp formed at the bottom of the streamlet electron tube and the liquid solution was colorless. There was not a large amount of sharp formed and it sort of smeared along the inside of the probe tube. Inferences What anions are in the shine? -iodine (I-) When compared with results from part B to test anions, similar results were institute. A dark red go down was formed in both.(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 part B to test cations, similar results were found, A violet-black precipitate was formed in both tests. Exchange reaction- Positive potassium started off with negative iodine, and corroboratory lead started off with negative nitrate. Potassium switched to combine with nitrate and lead switched to combine with iodine. Part DTesting of Precipitate Observations on sign Precipitate Formed (relative amount, etc.) Lead Nitrate Potassium Iodide Ratio provide 1 Powdery, yellow precipitate formed at the bottom. Not rattling much precipitate. Little to no streaking. Clear liquid solution above precipitate. 31 pipework 2 Powdery, yellow precipitate formed at the bottom. Equal to tube 1. Little to no streaking. Clear liquid solution above precipitate. 21 Tube 3 Powdery, yellow precipitate formed at the bottom. A little 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 formed at the bottom. Most precipitate f ormed out of all test tubes. A lot 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 supported? List cations and anions. Tube 1 The solution was clear with lead nitrate, save turned a yellow cloudy color with the potassium iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 2 The solution was clear with lead nitrate, and 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 iodide. K+ (potassium)I- (iodine)Discussion/Conclusion In part A , the runner step 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 azotic, 10 drops of dichloroethane, and 5 drops hydrogen peroxide to a new test tube. Then to a separate test tube, 5 drops of potassium nitrate, 5 drops of azotic acid, 10 drops of dichloroethane, and 5 hydrogen peroxide to a new test tube. two should be stoppered and shook to produce two distinct storeys. To test the cations, 2 test tubes would each get 20 drops of thioacetamide and 2 drops of nitric acid. One 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, then the clear aqueous layer was removed and discarded and the precipitate was washed with distilled water. This process was rep eated 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 toilet until clear. 20 drops of thioacetamide were added, stirred then heated in a water bath and compared to the results from part B. In part D, to determine the ratio ofions in the precipitate, 5 test tubes were labelled 1-5 and were filled according to table 3.1 on varlet 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 recorded. To test for potassium of iodide ions in the supernatant, 5 drops of lead nitrate were added to 5 separate 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 either lead nitrate. This ratio was found from balancing 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 clutch 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) ground 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 have a positive 2 charge. nearly inherent 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. by dint of this lab, a chemical reaction was used to find the pattern of responsiveness which was an exchange reaction. This is known by finding the chemical equation and aright 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 potassium iodide.