ProcedureFe3+ (aq) + SCN . (ay-FeSCN2+ (aq)light brown coessEq. 11.8)red1. Put 1 drop of 0.1 M iron (II) nitrate solution (Fe(NO,) into a clean10-cm test tube. Add 1 drop of 0.1 M potassium thiocyanate solution(KSCN) to the test tube. Add 5 mL of distilled water to the test tubeand mix well.2. Put 20 drops of the solution prepared in Step 1 into each of five clean10-cm test tubes.3. Use one of the test tubes as a color reference that represents the initialequilibrium condition Note its orange color that results from theequilibrium mixture containing both the light-brown-colored Fe ionsand red-colored FeSCNons in solution. Set the reference tube asideso you can compare other tube colors to it4. The remaining four samples in the test tubes will be used in the fourtests described below. Perform one test on each test tube. In each test,make sure the test tube contents are mixed well during heating orcooling and after test reagents are added. Then note and record inTable 11.7 any differences in the color intensity of the solution comparedto the reference solution (lighter or darker orange than the reference)a. Add 2 drops of 0.1 M iron (III nitrate solution (Fe(NO to one testb. Add 2 drops of 0.1 M potassium thiocyanate solution (KSCN) to onec. Add 1 drop of 0.1 M silver nitrate solution (AgNO,) to one testd. Cool one test tube in a small beaker of ice and water for 10 minutes.tube.test tube.tube.5. Put 20 drops of a saturated solution of calcium acetate (Ca(C2HO22)into a clean, dry 10-cm test tube. Note that this solution contains theequilibrium concentration of both Ca and C2H3O ons that are in-volved in the equilibrium represented by Equation 11.9. Note that thisis an equilibrium between undissolved solid and dissolved solid. Focuson the amount of undissolved solid present.Eq 11.9)6. Record the initial appearance of the original solution in Table 11.9Then put the test tube into a boiling water bath for 3 minutes. Agitatethe test tube to mix the contents after heating for 3 minutes, then noteand record the appearance of the sample in the test tube7. Cool the sample in a small beaker of ice and water for 3 minutes.Agitate the test tube two or three times during the cooling. When thecooling is completed, note and record the appearance of the sample.

Question
Asked Apr 9, 2019
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10. In Part D, what property will you observe that will allow you to determine the direction of equilibrium shift for the reaction Fe3+(aq) + SCN-(aq) = FeSCN2+(aq)

Procedure
Fe3+ (aq) + SCN . (ay-FeSCN2+ (aq)
light brown coess
Eq. 11.8)
red
1. Put 1 drop of 0.1 M iron (II) nitrate solution (Fe(NO,) into a clean
10-cm test tube. Add 1 drop of 0.1 M potassium thiocyanate solution
(KSCN) to the test tube. Add 5 mL of distilled water to the test tube
and mix well.
2. Put 20 drops of the solution prepared in Step 1 into each of five clean
10-cm test tubes.
3. Use one of the test tubes as a color reference that represents the initial
equilibrium condition Note its orange color that results from the
equilibrium mixture containing both the light-brown-colored Fe ions
and red-colored FeSCNons in solution. Set the reference tube aside
so you can compare other tube colors to it
4. The remaining four samples in the test tubes will be used in the four
tests described below. Perform one test on each test tube. In each test,
make sure the test tube contents are mixed well during heating or
cooling and after test reagents are added. Then note and record in
Table 11.7 any differences in the color intensity of the solution compared
to the reference solution (lighter or darker orange than the reference)
a. Add 2 drops of 0.1 M iron (III nitrate solution (Fe(NO to one test
b. Add 2 drops of 0.1 M potassium thiocyanate solution (KSCN) to one
c. Add 1 drop of 0.1 M silver nitrate solution (AgNO,) to one test
d. Cool one test tube in a small beaker of ice and water for 10 minutes.
tube.
test tube.
tube.
5. Put 20 drops of a saturated solution of calcium acetate (Ca(C2HO22)
into a clean, dry 10-cm test tube. Note that this solution contains the
equilibrium concentration of both Ca and C2H3O ons that are in-
volved in the equilibrium represented by Equation 11.9. Note that this
is an equilibrium between undissolved solid and dissolved solid. Focus
on the amount of undissolved solid present.
Eq 11.9)
6. Record the initial appearance of the original solution in Table 11.9
Then put the test tube into a boiling water bath for 3 minutes. Agitate
the test tube to mix the contents after heating for 3 minutes, then note
and record the appearance of the sample in the test tube
7. Cool the sample in a small beaker of ice and water for 3 minutes.
Agitate the test tube two or three times during the cooling. When the
cooling is completed, note and record the appearance of the sample.
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Procedure Fe3+ (aq) + SCN . (ay-FeSCN2+ (aq) light brown coess Eq. 11.8) red 1. Put 1 drop of 0.1 M iron (II) nitrate solution (Fe(NO,) into a clean 10-cm test tube. Add 1 drop of 0.1 M potassium thiocyanate solution (KSCN) to the test tube. Add 5 mL of distilled water to the test tube and mix well. 2. Put 20 drops of the solution prepared in Step 1 into each of five clean 10-cm test tubes. 3. Use one of the test tubes as a color reference that represents the initial equilibrium condition Note its orange color that results from the equilibrium mixture containing both the light-brown-colored Fe ions and red-colored FeSCNons in solution. Set the reference tube aside so you can compare other tube colors to it 4. The remaining four samples in the test tubes will be used in the four tests described below. Perform one test on each test tube. In each test, make sure the test tube contents are mixed well during heating or cooling and after test reagents are added. Then note and record in Table 11.7 any differences in the color intensity of the solution compared to the reference solution (lighter or darker orange than the reference) a. Add 2 drops of 0.1 M iron (III nitrate solution (Fe(NO to one test b. Add 2 drops of 0.1 M potassium thiocyanate solution (KSCN) to one c. Add 1 drop of 0.1 M silver nitrate solution (AgNO,) to one test d. Cool one test tube in a small beaker of ice and water for 10 minutes. tube. test tube. tube. 5. Put 20 drops of a saturated solution of calcium acetate (Ca(C2HO22) into a clean, dry 10-cm test tube. Note that this solution contains the equilibrium concentration of both Ca and C2H3O ons that are in- volved in the equilibrium represented by Equation 11.9. Note that this is an equilibrium between undissolved solid and dissolved solid. Focus on the amount of undissolved solid present. Eq 11.9) 6. Record the initial appearance of the original solution in Table 11.9 Then put the test tube into a boiling water bath for 3 minutes. Agitate the test tube to mix the contents after heating for 3 minutes, then note and record the appearance of the sample in the test tube 7. Cool the sample in a small beaker of ice and water for 3 minutes. Agitate the test tube two or three times during the cooling. When the cooling is completed, note and record the appearance of the sample.

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Expert Answer

Step 1

Given reaction is,

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Step 2

The reaction of Fe3+ (aq) + SCN- (aq) = [FeSCN]2+(aq) is a reversible reaction.

 

 The color of iron (from Fe(NO3)3) and KSCN are colorless (or have a slightly yellow tinge).

 

 While forming the product, [FeSCN]2+, the color changes to reddish brown. 

Step 3

To observe the equilibrium shift of Fe3+ + SCN-  =  Fe(SCN)2+ , one can observe the color change. Fe(SCN)2+ has a very reddish brown color which is very different fro...

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