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SQUARE ROOT SIMPLIFY EQUATIONS CALCULATOR
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Initial Conc. (M) 



Change in Conc. (M) 



Equilibirum Conc. (M) 



The change is only 0.03% of the initial value and is negligible.
[HA] = 0.500  1.5 x 10^{4} = 0.500 M
K and Q Lie on Opposite Sides of One (K>>Q or K<<Q)
When K is much larger than Q, or K is much smaller than Q, the change in amount of each species will be very large as the system moves towards a state of equilibirum. When this occurs, finding the change in concentration can often be facilitated by doing the following:
 When K>>Q and K > 1, assume 100% conversion into products, followed by the back reaction to establish equilibrium. When K<<Q and K < 1, assume 100% conversion into reactants, followed by the forward reaction to establish equilibrium.
 Make an ICE chart to determine change and equilibrium quantities starting with those resulting from the 100% conversion.
 Substitute quantities into the equilibrium expression.
 Assume the change is near zero such that "[A]  x" is equal to "[A]."
 Solve for the variable.
 Check to see if the change is less than 5% of the maximum amount, or within the limits set by your instructor. If not, use the method of approximations, a programmable calculator, or other method to solve.
 Solve for the equilibrium concentrations if asked to do so.
 Check your work.
H_{2}(g) + I_{2}(g) 2 HI(g) K_{c} = 794 @ 298 K
 Initially the [HI] = 0, so K >>Q and K is > 1. The change in the concentration of each species will be large so we calculate the quantity of product formed assuming 100% conversion.
 Make an ICE chart starting with the concentrations after the 100% conversion.
100% conversion will result in the formation of 1.24 M HI (1 to 1 to 2 proporation) with neither reactant remaining.




Initial Concentration (M) 



Change in Concentration (M) 



Equilibrium Concentration (M) 


