Math Problem Statement
- Calculate the [HIn], [In−], and [H+] for each of Solution 1—5 and the Unknown Solution, U.
[HIn] (M)
[In−] (M)
[H+] (M)
K at lab temp
Solution 1
Solution 2
Solution 3
Solution 4
Solution 5
Solution U
Solution
To calculate the concentrations of , , and in each of the solutions, I need to know the following:
- The pH of each solution (or the concentration of ).
- The acid dissociation constant () of the indicator in question.
- The concentration of the indicator () in each solution.
The indicator dissociates in water as follows:
The equilibrium expression for the dissociation is:
[ K_a = \frac{[H^+][In^-]}{[HIn]} ]
We can rearrange the equation to solve for the unknown concentrations.
If you provide these values for each solution (the pH or , the total concentration of the indicator, and ), I can help calculate the concentrations of , , and for each case.
Let me know if you have this information or if you'd like help in another way!
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Math Problem Analysis
Mathematical Concepts
Equilibrium Chemistry
Acid-Base Chemistry
Indicator Dissociation
Formulas
K_a = [H+][In^-] / [HIn]
Theorems
Le Chatelier's Principle
Henderson-Hasselbalch Equation
Suitable Grade Level
Grades 11-12
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