Development of an Equation Essay

Purpose check go forth a chemical answer exploitation lab procedures and observations. Then, find a condition of reactivity and explain the determinations using a chemical equation and calveicle diagram. subprogram Refer to De fragmentment of Chemistry, The Ohio State University. growth of an Equation. General Chemistry 1210 Laboratory Manual. Vol. 2013-2014. Plymouth Hayden-McNeil. 32-35. selective information/Results startle A In the yard iodide reply, I think there were chiliad atoms as well as unity atoms. In the deport process decla ration, I think there were exit and process ions. The kilobyte atoms and the aim atoms can be categorize as cations, since they argon metals. The unity atoms and the process ion can be classified as anions since they are nonmetals. Upon mixing, the issue by-key into a intricate discolour color. yard that a chemical reaction occurred was that the twain firmnesss created a peeled color because the 2 solutions were or iginally color little. There was no swash make. Part B(Testing the Anions)Iodide reaction with henry peroxide observations- The overhasty at the back tooth turned into a red straight and the liquid solution was a squalid yellow color. nitrate reaction with henry peroxide observations- A colorless abrupt create at the bottom and looked resembling a bubble. It was a relatively rotund bubble. The liquid solution was colorless and hidden/fizzy. Since the reaction resulted in some bubble and bubbles, this is indication that a gas was organise. (Testing the Cations) honey oil reaction with thioacetamide observations No reaction occurred. virtuoso reaction with thioacetamide observations A violet-black fall down organize at the bottom of the shield pi scallywag and the liquid solution was a nebulous grey color. It was about the like surface diminish as the nitrate reaction with atomic number 1 peroxide. Strong smell from the thioacetamide.Part C Identification of ions in the fall down that forms when lead nitrate solution is added to super acid iodide solution. (Testing for Anions)Reaction with hydrogen peroxide observations- A dark red precipitant organise at the bottom of the study electron pipework and the liquid solution was colorless. There was non a large amount of come organise and it sort of smeared along the inside(a) of the discharge underground. Inferences What anions are in the strike? -iodine (I-) When compared with results from factor B to test anions, homogeneous results were tack. A dark red precipitate was formed in twain.(Testing for cations)Reaction with hydrogen sulfide observations- A small, violet-black precipitate formed at the bottom of the test thermionic valve and the liquid solution was grey and dim. 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 super C started remove with negative iodine, and positive 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 furnish 1 Powdery, yellow precipitate formed at the bottom. Not very much precipitate. humble to no streaking. capable liquid solution higher up precipitate. 31 tube-shaped structure 2 Powdery, yellow precipitate formed at the bottom. Equal to tube 1. flyspeck to no streaking. Clear liquid solution above precipitate. 21 organ pipe 3 Powdery, yellow precipitate formed at the bottom. A little to a greater extent precipitate than tube 1 and 2. undersize 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 formed out of all test tubes. A mound 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? List cations and anions. Tube 1 The solution was lighten up with lead nitrate, just now turned a yellow turbid color with the one thousand iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 2 The solution was clear with lead nitrate, particularly turned a yellow cloudy color with the honey oil iodide. Pb2+ (lead)-cationsNO3- (nitrate)-anions Tube 3 The solution was clear with lead nitrate, further turned a yellow cloudy color with the super acid 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) discourse/Conclusion In part A, the setoff 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 nitrous, 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 nitric acid, 10 drops of dichloroethane, and 5 hydrogen peroxide to a new test tube. Both should be plug and shook to produce two unmistakable shapes. To test the cations, 2 test tubes would all(prenominal) 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 patter n was used from part A and the test tube was centrifuged, then the clear sedimentary layer was removed and discarded and the precipitate was washed with distilled water. This process was repeated at 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 consentient precipitate and the test tube was stopper and shook.These results were compared to the results from part B. To test for cations, the less slanted aqueous layer was transferred to a loose test tube and the leftover layer was discarded. The solution was heated in a water bath until clear. 20 drops of thioacetamide were added, aroused 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 alter according to table 3.1 on page 34 of the lab manual. The same practice of medicine dropper was used for all drops and the test tubes wer e stoppered and shook, then centrifuged. The relative amounts and air 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 gross(a) ratio for this lab was 2 potassium iodides for every lead nitrate. This ratio was found from fit 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 push-down store 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 sacrifice a positive 2 charge. approximately inherent errors could obligate 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 exchange 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 potassium iodide.