Equilibrium: ICE Tables
Learning Target: I can solve equilibrium problems using ICE tables.
ICE tables are used to calculate equilibrium concentrations of the reactants
and products from the initial concentrations.
Steps to use “ICE” table:
1.“I” = Tabulate known ___________ concentrations (and equilibrium concentrations if
known) of all species in equilibrium expression
2.“C” = Determine the concentration ______________ for the species where initial are
known
•Use stoichiometry to calculate concentration changes for all other species
involved in equilibrium
3.“E” = Calculate the _________________ concentrations
Sample Problem 1:
Enough ammonia is dissolved in 5.00 L of water at 25ºC to produce a solution that is
0.0124 M ammonia. The solution is then allowed to come to equilibrium. Analysis
of the equilibrium mixture shows that [OH1-] is 4.64 x 10-4 M. Calculate Keq at 25ºC
for the reaction:
NH3 (aq) + H2O (l) ↔ NH41+ (aq) + OH1- (aq)
Sample Problem 2:
When hydrogen iodide (HI) is placed in a closed container it will decompose into its
elements hydrogen and iodine and an equilibrium will be established:
2 HI (g)  H2(g) + I2(g)
Initial concentration of HI: 0.025 mol/L
Kc=2.2x10-3
Sample Problem 3:
A 5.000-L flask is filled with 5.000 x 10-3 mol of H2 and 1.000 x 10-2 mol of I2 at
448ºC. The value of Keq is 1.33. What are the concentrations of each substance at
equilibrium?
H2 (g) + I2 (g) ↔ 2 HI (g)
** Calculate concentrations