(2pts) Le Châtelier's Principle How will you collect data for this experiment? virtually Report Sheet Iron Thiocyanate R
Posted: Mon Jul 11, 2022 1:54 pm
(2pts) Le Châtelier's Principle How will you collect data forthis experiment? virtually
Report Sheet Iron Thiocyanate Reaction From the procedureMeasure 50 mL of 0.002 M KSCN solution in a 100 mL graduatedcylinder and pour it in a clean 100 or 150 mL beaker. Observe anycolor in the solution. If there is no color, write "colorless". Usea Pasteur pipet, add 4 drops of 0.2 M Fe(NO3)3 to the solution andmix with a glass stirrer. Observe any color in the solution. Thisis your equilibrium mixture.
KSCN (step 2) After addition of Fe(NO3)3 (step 3) colorlessturned orange immediately Enter your observations for: KSCN(procedure step 2) Addition of Fe(NO3)3 (procedure step 3) KSCN iscolorless, after the addition of Fe(NO3)3 the solution turnedorange. From the procedure Put the 6 clean, dry test tubes in atest tube rack. Label them "1" thru "6" with a permanent marker.Use a 10 mL graduated cylinder to divide the equilibrium mixtureequally among the 6 test tubes, placing roughly ~8.3 mL in each.Remember the "roughly" part, don't spend time getting precisely theright amount of solution, just get close to it. Test tube #1 isyour reference test tube. Do not add anything to it. Add 2 drops of0.2 M KSCN solution (in dropper bottle) to test tube 2 and mix witha glass stirrer. Compare it to the reference tube and observe anycolor changes (including the intensity of the color). Add 2 dropsof 0.2 M Fe(NO3)3 solution to test tube 3 and mix with a glassstirrer. Compare it to the reference tube and observe any colorchanges. Use a spatula to add a few grains of solid NaF to testtube 4 and mix well. Compare it to the reference tube and observeany color changes. Fluoride ion reacts with Fe3+(aq) to form thecomplex ion [FeF6]3- which effectively removes Fe3+(aq) fromparticipating in the FeSCN2+ reaction. Place test tube 5 in the hotwater bath and place test tube 6 in the ice bath. After about 5minutes, compare it to the reference tube and observe any colorchanges. Pour all solutions into the FeSCN2+ waste bottle and recapthe bottle. Wash out and dry your glassware for the next step.
For your reference tube (tube 1), select the color option thatbest matches your observation for the solution, then include anyadditional descriptions or details about your observation in the"Description" entry.
For tubes 2-6, compare each tube to the reference tube andselect the option that most closely describes the color of thatsolution relative to the reference solution. Then, include anyadditional descriptions or details about your observation in the"Description" entry.
For each solution, both the "Observation" and "Description"entries are required.
Table LC.1: Observations for Iron Thiocyanate Reaction Colorchange after the addition of various stressors Color observationDescription Test tube 1: Reference orange there is a red ring atthe top of the solution Test tube 2: Added KSCN(aq) more red/brownthan reference there is still a red ring at top of solution Testtube 3: Added Fe(NO3)3(aq) more red/brown than reference there is adark ring at top of solution Test tube 4: Added NaF(s) lessred/brown than reference the solution is clear Test tube 5: Hotwater bath less red/brown than reference the color is lighter butthere is a red ring at top of solution Test tube 6: Ice bath morered/brown than reference the color is orange with red ring attop
Tetrachlorocobaltate(II) Ion Reaction
From the procedure Transfer 40.0 mL of 0.01 M [CoCl4]2- inalcohol solution to a clean, dry 100 or 150 mL beaker using a 100mL graduate cylinder. Observe the color of soluton. Using a Pasteurpipette, add 30 drops of deionized water to the beaker and mixwell. Observe the color of the solution. This is your equilibriummixture.
[CoCl4]2- (step 1) After addition of DI water (step 2) lightblue light purple Enter your observations for: [CoCl4]2- (procedurestep 1) Addition of DI water (procedure step 2) [CoCl4]2- is alight blue color, after DI is added the color turned purple Fromthe procedure Prepare 6 clean, dry test tubes. Label them 1 thru 6.Divide the equilibrium mixture equally among the 6 test tubes. Yourfirst test tube is the reference test tube. Add one drop ofconcentrated HCl to test tube 2 and mix well. Compare it to thereference tube and observe color changes. Add 3-4 drops ofdeionized water to test tube 3 and mix well. Compare it to thereference tube and observe color changes. Remember the solvent inthis part is ethanol. Water is considered to be a reactant. Add onedrop of 0.02 M AgNO3 to test tube 4 and mix well. Ag+ reacts withCl- to form solid AgCl effectively removing Cl- from solution. Letthe solid settle, compare it to the reference tube and observe thecolor changes. Place test tube 5 in the hot water bath and testtube 6 in the ice water bath. After at least 5 minutes, take thetest tubes out, compare it to the reference tube and observe colorchanges. Place all solutions in the test tube in the cobalt wastebottle and clean up.
For your reference tube (tube 1), select the color option thatbest matches your observation for the solution, then include anyadditional descriptions or details about your observation in the"Description" entry. For tubes 2-6, compare each tube to thereference tube and select the option that most closely describesthe color of that solution relative to the reference solution.Then, include any additional descriptions or details about yourobservation in the "Description" entry. For each solution, both the"Observation" and "Description" entries are required. Table LC.2:EObservations for Tetrachlorocobaltate(II) Ion Reaction Colorchange after the addition of various stressors Color observationDescription Test tube 1: Reference purple light purple with a darkring a top Test tube 2: Added HCl (aq) more blue than referencelight blue with a blue ring at top Test tube 3: Added DI water morepink than reference light pink with a dark pink ring at rop Testtube 4: Added AgNO3(aq) more pink than reference precipitate formedat the bottom Test tube 5: Hot water bath more blue than referencelight blue in color Test tube 6: Ice bath more pink than referencepink ring at the top Your results will be graded based on theobservations you have entered above. Once you leave this part ofthis report, you will not be able to change these observations somake sure you double check them before proceeding. I have confirmedmy observations
(25pts) Iron Thiocyanate Reaction Analysis Fe 3 + ( a q ) + SCN− ( a q ) ⇌ FeSCN 2 + ( a q ) colorless blood-red color Table LC.3:Equilibrium Response for Iron Thiocyanate Reaction Table view Listview Analysis of equilibrium response to various stressors Colorobservation Reaction response Test tube 1: Reference orange Testtube 2: Added KSCN(aq) more red/brown than reference Towardsproducts Choose... Test tube 3: Added Fe(NO3)3(aq) more red/brownthan reference Towards products Choose... Test tube 4: Added NaF(s)less red/brown than reference Towards reactants Choose... Test tube5: Hot water bath less red/brown than reference Towards reactantsChoose... Test tube 6: Ice bath more red/brown than referenceTowards products Choose...
(10pts) 1. For test tubes 2 through 6, explain how each changeaffected the equilibrium in terms how each change affected thevalue of Qc or Kc and how this is consistent with your observation.For Tubes 2, 3 and 4 include in your analysis what happenschemically when each reagent is added. State the direction in whichthe equilibrium shifts and relate how the change in solution colorsupports your conclusions. Saved →attachment
(3pts) 2. Based on your results from test tubes 5 and 6, is thisreaction exothermic or endothermic? Exothermic Saved
(2pts) Give a reason for your choice. Saved →attachment
(25pts) Tetrachlorocobaltate(II) Ion Reaction Analysis [ CoCl 4] − ( a l c ) + 6 H 2 O ( a l c ) ⇌ [ Co(H 2 O) 6 ] 2 + ( a l c ) +4 Cl − ( a l c ) deep blue rose pink Table LC.4: EquilibriumResponse for Tetrachlorocobaltate(II) Ion Reaction Table view Listview Analysis of equilibrium response to various stressors Colorobservation Reaction response Test tube 1: Reference purple Testtube 2: Added HCl (aq) more blue than reference Choose... Choose...Test tube 3: Added DI water more pink than reference Choose...Choose... Test tube 4: Added AgNO3(aq) more pink than referenceChoose... Choose... Test tube 5: Hot water bath more blue thanreference Choose... Choose... Test tube 6: Ice bath more pink thanreference Choose... Choose...
(10pts) 3. For test tubes 2 through 6, explain how each changeaffected the equilibrium in terms how each change affected thevalue of Qc or Kc and how this is consistent with your observation.For Tubes 2, 3 and 4 include in your analysis what happenschemically when each reagent is added. State the direction in whichthe equilibrium shifts and relate how the change in solution colorsupports your conclusions. Saved →attachment
(3pts) 4. Based on your results from test tubes 5 and 6, is thisreaction exothermic or endothermic? Choose...
(2pts) Give a reason for your choice. Saved →attachment
(7pts) Post-Laboratory Questions
(2pts) 1. In Step 1 of of the tetrachlorocobaltate(II) ionreaction, there is a warning that all glassware must be dry whenpreparing the equilibrium solution. Explain why this warning wasincluded. Saved →attachment
(3pts) 2. Write the balanced net ionic equation for the reactionof Fe3+ and NaF. Explain, in your own words, how this secondreaction affects the equilibrium of the iron thiocyanate reactionand what this indicates about the stability of the iron(III)fluoride complex compared to the iron(III) thiocyanate complex.Saved →attachment
(2pts) 3. Write the balanced net ionic equation for the reactionof Cl- and AgNO3. Explain, in your own words, how this secondreaction affects the equilibrium of the tetrachlorocobaltate(II)ion reaction. Be sure to mention what specific property of theproduct drives this shift in equilibrium. Saved →attachment
Report Sheet Iron Thiocyanate Reaction From the procedureMeasure 50 mL of 0.002 M KSCN solution in a 100 mL graduatedcylinder and pour it in a clean 100 or 150 mL beaker. Observe anycolor in the solution. If there is no color, write "colorless". Usea Pasteur pipet, add 4 drops of 0.2 M Fe(NO3)3 to the solution andmix with a glass stirrer. Observe any color in the solution. Thisis your equilibrium mixture.
KSCN (step 2) After addition of Fe(NO3)3 (step 3) colorlessturned orange immediately Enter your observations for: KSCN(procedure step 2) Addition of Fe(NO3)3 (procedure step 3) KSCN iscolorless, after the addition of Fe(NO3)3 the solution turnedorange. From the procedure Put the 6 clean, dry test tubes in atest tube rack. Label them "1" thru "6" with a permanent marker.Use a 10 mL graduated cylinder to divide the equilibrium mixtureequally among the 6 test tubes, placing roughly ~8.3 mL in each.Remember the "roughly" part, don't spend time getting precisely theright amount of solution, just get close to it. Test tube #1 isyour reference test tube. Do not add anything to it. Add 2 drops of0.2 M KSCN solution (in dropper bottle) to test tube 2 and mix witha glass stirrer. Compare it to the reference tube and observe anycolor changes (including the intensity of the color). Add 2 dropsof 0.2 M Fe(NO3)3 solution to test tube 3 and mix with a glassstirrer. Compare it to the reference tube and observe any colorchanges. Use a spatula to add a few grains of solid NaF to testtube 4 and mix well. Compare it to the reference tube and observeany color changes. Fluoride ion reacts with Fe3+(aq) to form thecomplex ion [FeF6]3- which effectively removes Fe3+(aq) fromparticipating in the FeSCN2+ reaction. Place test tube 5 in the hotwater bath and place test tube 6 in the ice bath. After about 5minutes, compare it to the reference tube and observe any colorchanges. Pour all solutions into the FeSCN2+ waste bottle and recapthe bottle. Wash out and dry your glassware for the next step.
For your reference tube (tube 1), select the color option thatbest matches your observation for the solution, then include anyadditional descriptions or details about your observation in the"Description" entry.
For tubes 2-6, compare each tube to the reference tube andselect the option that most closely describes the color of thatsolution relative to the reference solution. Then, include anyadditional descriptions or details about your observation in the"Description" entry.
For each solution, both the "Observation" and "Description"entries are required.
Table LC.1: Observations for Iron Thiocyanate Reaction Colorchange after the addition of various stressors Color observationDescription Test tube 1: Reference orange there is a red ring atthe top of the solution Test tube 2: Added KSCN(aq) more red/brownthan reference there is still a red ring at top of solution Testtube 3: Added Fe(NO3)3(aq) more red/brown than reference there is adark ring at top of solution Test tube 4: Added NaF(s) lessred/brown than reference the solution is clear Test tube 5: Hotwater bath less red/brown than reference the color is lighter butthere is a red ring at top of solution Test tube 6: Ice bath morered/brown than reference the color is orange with red ring attop
Tetrachlorocobaltate(II) Ion Reaction
From the procedure Transfer 40.0 mL of 0.01 M [CoCl4]2- inalcohol solution to a clean, dry 100 or 150 mL beaker using a 100mL graduate cylinder. Observe the color of soluton. Using a Pasteurpipette, add 30 drops of deionized water to the beaker and mixwell. Observe the color of the solution. This is your equilibriummixture.
[CoCl4]2- (step 1) After addition of DI water (step 2) lightblue light purple Enter your observations for: [CoCl4]2- (procedurestep 1) Addition of DI water (procedure step 2) [CoCl4]2- is alight blue color, after DI is added the color turned purple Fromthe procedure Prepare 6 clean, dry test tubes. Label them 1 thru 6.Divide the equilibrium mixture equally among the 6 test tubes. Yourfirst test tube is the reference test tube. Add one drop ofconcentrated HCl to test tube 2 and mix well. Compare it to thereference tube and observe color changes. Add 3-4 drops ofdeionized water to test tube 3 and mix well. Compare it to thereference tube and observe color changes. Remember the solvent inthis part is ethanol. Water is considered to be a reactant. Add onedrop of 0.02 M AgNO3 to test tube 4 and mix well. Ag+ reacts withCl- to form solid AgCl effectively removing Cl- from solution. Letthe solid settle, compare it to the reference tube and observe thecolor changes. Place test tube 5 in the hot water bath and testtube 6 in the ice water bath. After at least 5 minutes, take thetest tubes out, compare it to the reference tube and observe colorchanges. Place all solutions in the test tube in the cobalt wastebottle and clean up.
For your reference tube (tube 1), select the color option thatbest matches your observation for the solution, then include anyadditional descriptions or details about your observation in the"Description" entry. For tubes 2-6, compare each tube to thereference tube and select the option that most closely describesthe color of that solution relative to the reference solution.Then, include any additional descriptions or details about yourobservation in the "Description" entry. For each solution, both the"Observation" and "Description" entries are required. Table LC.2:EObservations for Tetrachlorocobaltate(II) Ion Reaction Colorchange after the addition of various stressors Color observationDescription Test tube 1: Reference purple light purple with a darkring a top Test tube 2: Added HCl (aq) more blue than referencelight blue with a blue ring at top Test tube 3: Added DI water morepink than reference light pink with a dark pink ring at rop Testtube 4: Added AgNO3(aq) more pink than reference precipitate formedat the bottom Test tube 5: Hot water bath more blue than referencelight blue in color Test tube 6: Ice bath more pink than referencepink ring at the top Your results will be graded based on theobservations you have entered above. Once you leave this part ofthis report, you will not be able to change these observations somake sure you double check them before proceeding. I have confirmedmy observations
(25pts) Iron Thiocyanate Reaction Analysis Fe 3 + ( a q ) + SCN− ( a q ) ⇌ FeSCN 2 + ( a q ) colorless blood-red color Table LC.3:Equilibrium Response for Iron Thiocyanate Reaction Table view Listview Analysis of equilibrium response to various stressors Colorobservation Reaction response Test tube 1: Reference orange Testtube 2: Added KSCN(aq) more red/brown than reference Towardsproducts Choose... Test tube 3: Added Fe(NO3)3(aq) more red/brownthan reference Towards products Choose... Test tube 4: Added NaF(s)less red/brown than reference Towards reactants Choose... Test tube5: Hot water bath less red/brown than reference Towards reactantsChoose... Test tube 6: Ice bath more red/brown than referenceTowards products Choose...
(10pts) 1. For test tubes 2 through 6, explain how each changeaffected the equilibrium in terms how each change affected thevalue of Qc or Kc and how this is consistent with your observation.For Tubes 2, 3 and 4 include in your analysis what happenschemically when each reagent is added. State the direction in whichthe equilibrium shifts and relate how the change in solution colorsupports your conclusions. Saved →attachment
(3pts) 2. Based on your results from test tubes 5 and 6, is thisreaction exothermic or endothermic? Exothermic Saved
(2pts) Give a reason for your choice. Saved →attachment
(25pts) Tetrachlorocobaltate(II) Ion Reaction Analysis [ CoCl 4] − ( a l c ) + 6 H 2 O ( a l c ) ⇌ [ Co(H 2 O) 6 ] 2 + ( a l c ) +4 Cl − ( a l c ) deep blue rose pink Table LC.4: EquilibriumResponse for Tetrachlorocobaltate(II) Ion Reaction Table view Listview Analysis of equilibrium response to various stressors Colorobservation Reaction response Test tube 1: Reference purple Testtube 2: Added HCl (aq) more blue than reference Choose... Choose...Test tube 3: Added DI water more pink than reference Choose...Choose... Test tube 4: Added AgNO3(aq) more pink than referenceChoose... Choose... Test tube 5: Hot water bath more blue thanreference Choose... Choose... Test tube 6: Ice bath more pink thanreference Choose... Choose...
(10pts) 3. For test tubes 2 through 6, explain how each changeaffected the equilibrium in terms how each change affected thevalue of Qc or Kc and how this is consistent with your observation.For Tubes 2, 3 and 4 include in your analysis what happenschemically when each reagent is added. State the direction in whichthe equilibrium shifts and relate how the change in solution colorsupports your conclusions. Saved →attachment
(3pts) 4. Based on your results from test tubes 5 and 6, is thisreaction exothermic or endothermic? Choose...
(2pts) Give a reason for your choice. Saved →attachment
(7pts) Post-Laboratory Questions
(2pts) 1. In Step 1 of of the tetrachlorocobaltate(II) ionreaction, there is a warning that all glassware must be dry whenpreparing the equilibrium solution. Explain why this warning wasincluded. Saved →attachment
(3pts) 2. Write the balanced net ionic equation for the reactionof Fe3+ and NaF. Explain, in your own words, how this secondreaction affects the equilibrium of the iron thiocyanate reactionand what this indicates about the stability of the iron(III)fluoride complex compared to the iron(III) thiocyanate complex.Saved →attachment
(2pts) 3. Write the balanced net ionic equation for the reactionof Cl- and AgNO3. Explain, in your own words, how this secondreaction affects the equilibrium of the tetrachlorocobaltate(II)ion reaction. Be sure to mention what specific property of theproduct drives this shift in equilibrium. Saved →attachment