Math Problem Statement
Solution
The image you've uploaded contains a problem about calculating equilibrium concentrations for the reaction involving ammonia () and water, where the equilibrium constant . You need to use the ICE (Initial, Change, Equilibrium) table method to find the equilibrium concentrations for this reaction.
Here's the general approach:
1. Write the balanced chemical equation:
2. Set up the ICE table:
- I (Initial): You start with 0.25 M of and no or .
- C (Change): As the reaction proceeds to equilibrium, some of the will dissociate, producing and .
- E (Equilibrium): At equilibrium, you'll have the concentrations of , , and .
The equilibrium expression based on the reaction is:
[ K_c = \frac{[NH_4^+][OH^-]}{[NH_3]} ]
Now, let's go step-by-step to fill the table.
-
I (Initial):
-
C (Change):
- Let represent the concentration of that dissociates. Hence:
- The change for will be .
- The change for both and will be .
- Let represent the concentration of that dissociates. Hence:
-
E (Equilibrium):
Substitute these into the equilibrium expression:
Now, you can solve this equation to find , and then determine the equilibrium concentrations for each species.
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Math Problem Analysis
Mathematical Concepts
Equilibrium Chemistry
ICE Tables
Quadratic Equations
Formulas
Kc = [NH₄⁺][OH⁻] / [NH₃]
x (concentration change)
Theorems
Le Chatelier's Principle
Suitable Grade Level
Grades 10-12
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