Add FeCl3 to the second tube Add kSCN to test tube 3 Add AgNO3 to test tube 4 an

Question

Add FeCl3 to the second tube Add kSCN to test tube 3 Add AgNO3 to test tube 4 and till allthe color disapears Answer the following questions: Fofmat Painter D Clipboard Font Alignment A19 40 Part 5: Fe3++SCN- 41 1.Observations: 42 Tube 2: 43 Tube 3: 44 Tube 4: 45 2 Write the reaction equilibrium we are investigating 46 47 3. In which direction did the stress cause the equilibrium to shift? Tube 2: Tube 3: Tube 4: 4. Explain why the reaction shifted using phrases such as (Added/Removed reactants or Tube 2: 48 49 50 51 Added/Removed products) 52 Tube 3: 53 Tube 4: 54 55 Post Lab Questions 1. Imagine you have a saturated solution of Ca(OH)2, at equilibrium, that has some undissolved Ca(OH)2 solid on the bottom of the test tube. If you add an additional scope of Ca(OH)2 to this solution will the concentration of [OH-1 in the solution increase, decrease, of be unchanged? (Briefly explain and assume we let the solution reach equilibrium again) s6 60 61

Explanation / Answer

40.      Fe3+ + SCN– <------------à FeSCN2+

Given-

Full 4 test tubes with stock

Iron(111)thiocyanate solution and the use the first one as control

Add FeCl3 to the second tube

Add kSCN to test tube 3

Add AgNO3 to test tube 4 and till all the color disappears

41. Observations- If [SCN] is added to a solution containing Fe3+, a blood red solution is formed due to the formation of [Fe(SCN)(H2O)5]2+.

42. When we add FeCl3 to the second tube,   red color became deeper.

43. When we add KSCN to the third tube,   red color became deeper.

44. When we add AgNO3 to the forth tube, solution turned milky white.

45. The reaction equilibrium-

      Fe3+ + SCN– <--------à FeSCN2+

47. Tube 2-

Adding FeCl3 (Fe3+) removes the equilibrium from the solution by adding more product (left side). The reaction will shift to the right in order to convert some SCN- to FeSCN2+

48.

Adding KSCN to test tube 3 mean that adding K+ and SCN- to the system since they dissociate The K+ doesn't matter for the above equation, however the SCN- does. Adding a product (SCN-) will drive the equilibrium to the right turning the solution red.

49.

When AgNO3 is added to test tube 4 and till all the color disappears

Fe3+ (aq) + 3SCN- + 3AgNO3 (aq) ----> 3AgSCN(s) + Fe(NO3)3 (aq)

So, the equilibrium shifts toward the reactants side as the concentration of the reactants decreases the color disappears.

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