Chemistry: Displacement Reactions Essay

Objectives1. Learn how to determinate the percent report card2. Learn how to withdraw the percent utilize oxidation reduction and prototype fight backions3. To become more familiar with the use titration techniques4. To learn how to get the salinity out of an quimicalBackgroundTo develop and utilize procedures to sterilise the percent composition, of ZnCI2. As well titrating with NaOH resultant role. After all in all the experiment we got hta flavour witch we dull and we got our results.Experiment moveions.33w of Zn(OH)2 x counterspyes Zn(OH)2/m. moles Zn(OH2) x 1molZnCI2/1 mol Zn(OH)2 x g molZnCI2/1 mol of ZnCL2 = .4531 grams of ZnCI2 .4531g of ZnCl2 x 1 moles ZnCI2/m. moles ZnCI2 x 1molZn/1 mol of ZnCI2 x 65.39 of Zn/1 mol Zn = .2174g ZnMaterials inevitableScaleBuretteBeakerSpatulaErlenmeyer flaskPrenolpthen ( saturation indicator)ZnCL2NaOHTubeVacuumPaper filters natural rubber baseQuestions1. What is the weight of a grade 1982 centime?2.5 grams2. What is the percen t blur and surface in a post 1982 penny?97.5% of zinc and 2.5% of bull3. How many grams of copper and zinc ar in a post 1982 penny?2.44grams of copper and 0.0625gramss of zinc4. How many moles of copper and zinc are in post 1982 pennies?0.0383moles of cooper and 0.000955moles of zinc5. Write a balance reaction of zinc with HCl.Zn (s) + 2 HCl(aq) ==== Zn+2(aq) + 2 Cl-(aq) + H2(g) answerZn(s) + 2 H+(aq) ==== Zn+2(aq) + H2(g)6. How many moles of HCl are infallible to react get alongly with all of the zinc in a post 1982 penny?7.46 x 10-2 mol HCl7. In a procedure developed to make up the percent zinc in post 1982 pennies, 50 ml of an HCl root was used to react (dissolve) all of the zinc in the penny. To contain complete reaction, the solution contains twice as many moles of HCl that is actually needed. What niggardness of HCl should be used?M=2.9847.4610-2 mol x 2 = .1492mol H8. In the scenario described in problem 7, what is the amount (in moles) of supernumerary (unreacted) HCl in solution?.1492 moles used.0746 needed.0746 moles HCI unreacted9. How many moles of NaOH would be needed to completely react with all of the excess HCl posed in problem 8?.0746 moles HCI reacts with.0746 moles of NaOH10. As described in problem 7, a procedure was developed to determine the percent zinc in post 1982 pennies. In that procedure 50 ml of an HCl was used to react (dissolve) all of the zinc in the penny. To ensure complete reaction, the solution contains twice as many moles of HCl that is actuallyneeded. To determine the percent zinc in the penny, the excess (unreacted) HCl was titrated with NaOH. Determine the concentration of NaOH needed if you want to use approximately 25 mL of NaOH to titrate the excess HCl. M = .0746 moles of NaOH/.025L NaOHM = 2.98411. Write the balanced chemical reaction of zinc with HCl (same as problem 5). Is the yield of this reaction soluble in sedimentary solution? Yes soluble Zn(s) + 2HCI (aq) = ZnCI2(aq) + H2(g)12. Write the balance d chemical reaction of the product of the reaction described above (problem 11) with NaOH. Is the product of this reaction soluble in aqueous solution? ZnCI2 + 2NaOH = Zn(OH)2+ 2NaCIZn(OH)2 = low solubilityExpected resultsOur expected results are to obtain the wiretap cluster in the solution while titrating. This course after taken more steps we while maybe be able to find rough salt.Steps to do*In the offset printing part of this experiment we are going to dissolve the zinc total of a penny *After that we leave the copper covering total*We also by putting four notches in the coin using a triangular file and placing the penny in 50ml of a determine concentration of HCI overnight*After that we are going to determinate the concentration needed to add 2 times the number of moles of HCI needed in the 50ml of solution *We are going to determinate the percent of copper from the can of copper and the percent zinc by two methods1. The titration experiment2. The hastiness experimen t*Now we first got 10 ml of ZnCI2*To that we added 6 drops of our color indicator (Prenolpthen) *After that we got 50 ml NaOH solution*Than we titrate the ZnCl2 with NaOH*Until we got pink cluster*Now we put the clusters in a paper filter that was dripping the solution living only the clusters *With a tube we affiliated a vacuum so this way wewere left with only the salt*After this we put the salt in like an oven so that this could wry the salt and this wont be wet*When we took it out all we had was dry salt and we weight it and started our formulasResultsI calculated the percent % of salt of Zn(OH)2. First I determinate the formulas for both, follow by calculating the atomic mass of Zn. First I had to have the weight of the salt, so I did all the procedures on top. My result for the weight of the salt was .33g and the result of the Zn was .2174. To be able to get percent I calculated by dividing 2.174 witch is the grams of Zn and 2.5 grams multiplying the result by 100 = 86.994% Conclusion and discussionDuring Experiment 8 conducted April 16 2014. I noticed the difference in the % for the reaction, when titrating ZnCI2 with NaOH solution. For this experiment we did 2 trials since in the first one we did not get any clusters, but on the second trial we did get some and we got more salt than anyone else.