Question

45 Determination of Equilibrium Constant pre-lab Assignment 1. What is the chemical equation and equilibrium equation ($K_{eq}$=) that will be measured in this lab? $Fe^{3+}_{(aq)} + SCN^-_{(aq)} \leftrightharpoons FeSCN^{2+}_{(aq)}$ 2. Give the equilibrium equation ($K_{eq}$=) for this reaction. $K_{eq} = \frac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^-]}$ 3. Why is a massive excess of iron ion ($Fe^{3+}$) added to the reaction in part I? 4) Why is nitric acid added to the reaction? 4. Pt. 1: Each solution is measured by a mixture of three solutions, causing the concentration of every ion to be diluted. For the solution below determine what the concentration of $Fe^{3+}$ and $SCN^-$ will be AFTER dilution ($M_f$) ($M_1V_1 = M_2V_2$) Test Tube 0.100 M $Fe^{3+}$ 0.0010 M SCN $H_2O$ total volume (mL) (mL) (mL) (mL) 1 2.0 2.0 6.0 10.0 2 2.0 3.0 5.0 10.0 Test tube $Fe^{3+}$ Conc (M) SCN Conc (M) After dilution After dilution 1 2 Note: These concentrations after dilution are considered to be the "Initial" concentrations for the equilibrium ICE tables.

          45
Determination of Equilibrium Constant pre-lab Assignment
1. What is the chemical equation and equilibrium equation ($K_{eq}$=) that will be measured in this
lab?
$Fe^{3+}_{(aq)} + SCN^-_{(aq)} \leftrightharpoons FeSCN^{2+}_{(aq)}$
2. Give the equilibrium equation ($K_{eq}$=) for this reaction.
$K_{eq} = \frac{[FeSCN^{2+}]}{[Fe^{3+}][SCN^-]}$
3. Why is a massive excess of iron ion ($Fe^{3+}$) added to the reaction in part I?
4) Why is nitric acid added to the reaction?
4. Pt. 1: Each solution is measured by a mixture of three solutions, causing the concentration of
every ion to be diluted. For the solution below determine what the concentration of $Fe^{3+}$ and
$SCN^-$ will be AFTER dilution ($M_f$) ($M_1V_1 = M_2V_2$)
Test Tube
0.100 M $Fe^{3+}$
0.0010 M SCN
$H_2O$
total volume (mL)
(mL)
(mL)
(mL)
1
2.0
2.0
6.0
10.0
2
2.0
3.0
5.0
10.0
Test tube
$Fe^{3+}$ Conc (M)
SCN Conc (M)
After dilution
After dilution
1
2
Note: These concentrations after dilution are considered to be the "Initial" concentrations for the
equilibrium ICE tables.

45
Determination of Equilibrium Constant pre-lab Assignment
1. What is the chemical equation and equilibrium equation (Keq=) that will be measured in this
lab?
Fe^3+(aq) + SCN^-(aq)⇋ FeSCN^2+(aq)
2. Give the equilibrium equation (Keq=) for this reaction.
Keq = ([FeSCN^2+])/([Fe^3+][SCN^-])
3. Why is a massive excess of iron ion (Fe^3+) added to the reaction in part I?
4) Why is nitric acid added to the reaction?
4. Pt. 1: Each solution is measured by a mixture of three solutions, causing the concentration of
every ion to be diluted. For the solution below determine what the concentration of Fe^3+ and
SCN^- will be AFTER dilution (Mf) (M1V1 = M2V2)
Test Tube
0.100 M Fe^3+
0.0010 M SCN
H2O
total volume (mL)
(mL)
(mL)
(mL)
1
2.0
2.0
6.0
10.0
2
2.0
3.0
5.0
10.0
Test tube
Fe^3+ Conc (M)
SCN Conc (M)
After dilution
After dilution
1
2
Note: These concentrations after dilution are considered to be the "Initial" concentrations for the
equilibrium ICE tables.

Added by Juan Jos- H.

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