Pre-Laboratory Assignment: Determination of K, for a Complex lon Formation Name Section A student mixes 5.0 ml of 0.00200 M Fe(NO,), with 5.0 mL 0.00200 KSCN. She finds that the concentration of FESCN in the equilibrium mixture is 0.000125 M. Follow these steps to determine the corresponding experimental value of K, for the reaction of Fe" and SCN to produce this complex ion. Show your calculations for each step below and then place the appropriate value(s) in the equilibrium (or 'ICE') table near the bottom of the page. Step 1. Calculate the molarity of Fe", SCN, and FESCN" initially present after mixing the two solutions, but prior to any reaction taking place. (M,V, = M,V3) Step 2. Determine the expression and initial value for Q. Then give the appropriate signs of the concentration changes for each species in terms of the reaction's shift, or x, into the ICE table. Step 3. Fill in the equilibrium value for the molarity of FeSCN". From this, you can determine the value of x. Step 4. Given the value of x, determine the equilibrium molarities of Fe" and SCN". "ICE' Table Fe" (ag) SCN (aq) = FeSCN" (aq) Step 5. Give the correct expression for K. for this equation. Then calculate the value of K. for the reaction from the equilibrium concentrations. Use correct significant figures. Step 6. On the reverse side, complete an 'ICE' table using this same procedure, but using a different reaction stoichiometry: Fe" + 2 SCN S FESCN". Assume that the equilibrium concentration of FeSCN" is 0.0000625 M, or one-half its previous value. Remember how the reaction stoichiometry affects the expression for K Page 1 of t K, Determination
Pre-Laboratory Assignment: Determination of K, for a Complex lon Formation Name Section A student mixes 5.0 ml of 0.00200 M Fe(NO,), with 5.0 mL 0.00200 KSCN. She finds that the concentration of FESCN in the equilibrium mixture is 0.000125 M. Follow these steps to determine the corresponding experimental value of K, for the reaction of Fe" and SCN to produce this complex ion. Show your calculations for each step below and then place the appropriate value(s) in the equilibrium (or 'ICE') table near the bottom of the page. Step 1. Calculate the molarity of Fe", SCN, and FESCN" initially present after mixing the two solutions, but prior to any reaction taking place. (M,V, = M,V3) Step 2. Determine the expression and initial value for Q. Then give the appropriate signs of the concentration changes for each species in terms of the reaction's shift, or x, into the ICE table. Step 3. Fill in the equilibrium value for the molarity of FeSCN". From this, you can determine the value of x. Step 4. Given the value of x, determine the equilibrium molarities of Fe" and SCN". "ICE' Table Fe" (ag) SCN (aq) = FeSCN" (aq) Step 5. Give the correct expression for K. for this equation. Then calculate the value of K. for the reaction from the equilibrium concentrations. Use correct significant figures. Step 6. On the reverse side, complete an 'ICE' table using this same procedure, but using a different reaction stoichiometry: Fe" + 2 SCN S FESCN". Assume that the equilibrium concentration of FeSCN" is 0.0000625 M, or one-half its previous value. Remember how the reaction stoichiometry affects the expression for K Page 1 of t K, Determination
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 37P
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Transcribed Image Text:Pre-Laboratory Assignment:
Determination of K, for a Complex lon Formation
Name
Section
A student mixes 5.0 ml of 0.00200 M Fe(NO,), with 5.0 mL 0.00200 KSCN. She finds that the
concentration of FESCN in the equilibrium mixture is 0.000125 M. Follow these steps to
determine the corresponding experimental value of K, for the reaction of Fe" and SCN to produce
this complex ion. Show your calculations for each step below and then place the appropriate
value(s) in the equilibrium (or 'ICE') table near the bottom of the page.
Step 1. Calculate the molarity of Fe", SCN, and FeSCN" initially present after mixing the two
solutions, but prior to any reaction taking place. (M,V, = M,V3)
Step 2. Determine the expression and initial value for Q. Then give the appropriate signs of the
concentration changes for each species in terms of the reaction's shift, or x, into the ICE table.
Step 3. Fill in the equilibrium value for the molarity of FESCN". From this, you can determine the
value of x.
Step 4. Given the value of x, determine the equilibrium molarities of Fe" and SCN".
"ICE' Table
Fe" (aq)
SCN (aq) = FeSCN" (aq)
E
Step 5. Give the correct expression for K. for this equation. Then calculate the value of K. for the
reaction from the equilibrium concentrations. Use correct significant figures.
Step 6. On the reverse side, complete an 'ICE' table using this same procedure, but using a
different reaction stoichiometry: Fe" + 2 SCN S FESCN". Assume that the equilibrium
concentration of FeSCN" is 0.0000625 M, or one-half its previous value. Remember how the
reaction stoichiometry affects the expression for K
Page 1 of 1
K, Determination
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