When you set up the ICE chart, are you supposed to bring the 0.05 to the product side to give you an equation of x^2 / x - 0.05?
Thomas, with the equation I gave you before you really don't need an ICE chart.
I think I had
Kb = (Kw/Ka) = (HC2H3O2)(OH^-)/(0.05)
1 x 10^014/1.8 x 10^-5) = 5.55 x 10^-10
so
5.55 x 10^-10 = (X^2)/0.05
Then X^2 = 5.55 x 10^-10 x 0.05
X = sqrt(5.55 x 10^-10 x 0.05)
This is the OH^-, convert to pOH, then to pH.
Thank You, i got it. The answer was 8.7
When setting up an ICE (Initial-Change-Equilibrium) chart, it is important to follow the principles of stoichiometry and consider the balanced chemical equation.
Let's take the example of a generic chemical reaction:
a A + b B ⇌ c C + d D
In the ICE chart, we typically write the initial amounts or concentrations of the reactants (A and B) on the left-hand side and products (C and D) on the right-hand side. The "I" in ICE stands for "Initial."
Next, we determine the "change" in concentration or amount for each species. This change is usually represented by variables such as "x," which represents the change in concentration or amount after reaching equilibrium.
Finally, we write the "Equilibrium" concentrations or amounts, which include both the initial amounts and the changes. This allows us to calculate the equilibrium concentrations or amounts of each species using the initial conditions and changes.
In regards to your specific equation, x^2 / (x - 0.05), it seems like you are describing the expression for calculating the equilibrium concentration using the quadratic formula. However, it is impossible to determine the correct calculation without knowing the specific reaction and its balanced chemical equation.
To correctly set up an ICE chart, you need to start with a balanced chemical equation and then determine the initial amounts/concentrations, changes, and equilibrium amounts/concentrations based on the given conditions.