Math Problem Statement

  1. 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 [HIn][HIn], [In][In^-], and [H+][H^+] in each of the solutions, I need to know the following:

  1. The pH of each solution (or the concentration of [H+][H^+]).
  2. The acid dissociation constant (KaK_a) of the indicator in question.
  3. The concentration of the indicator ([HIn]+[In][HIn] + [In^-]) in each solution.

The indicator dissociates in water as follows:

HInH++InHIn \rightleftharpoons H^+ + In^-

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 [H+][H^+], the total concentration of the indicator, and KaK_a), I can help calculate the concentrations of [HIn][HIn], [In][In^-], and [H+][H^+] 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