A monoprotic weak acid (HA) has a \( pK_a \) value of 4.435. Calculate the fraction of HA in each of its forms (HA, \( A^- \)) at pH 5.659.\[\alpha_{HA} = \quad \quad \alpha_{A^-} =\]What is the quotient \(\frac{[A^-]}{[HA]}\) at pH 5.659?\[\frac{[A^-]}{[HA]} = \] **Exercise: Calculating Ion Concentrations****Task:**Calculate the concentrations of hydronium ions, \( \text{H}_3\text{O}^+ \), and hydroxide ions, \( \text{OH}^- \), for a 0.0285 M HCl solution.**Inputs:**- [\( \text{H}_3\text{O}^+ \)] = **1.545 M** (Incorrect)- [\( \text{OH}^- \)] = **12.45 M** (Incorrect)**Instructions:**Enter the correct numeric values for each ion concentration in the provided fields. The current entries are incorrect; reassess the calculations based on the given HCl concentration.Understanding the dissociation of HCl in water and the resulting impact on ion concentrations is crucial:- Remember that in a solution, \( \text{HCl} \) completely dissociates to produce equal concentrations of \( \text{H}_3\text{O}^+ \).- Utilize the water dissociation constant, \( K_w \), to calculate \( \text{OH}^- \).**Note:** This exercise helps to reinforce the concept of pH and equilibria in aqueous solutions.

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Answered: 20 A monoprotic weak acid (HA) has a pK…

20 A monoprotic weak acid (HA) has a pK value of 4.435. Calculate the fraction of HA in each of its forms (HA, A¯) at pH 5.659. αHA = What is the quotient [A-] = [HA] [A-] at pH 5.659? [HA] αA- =

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

A monoprotic weak acid (HA) has a \( pK_a \) value of 4.435. Calculate the fraction of HA in each of its forms (HA, \( A^- \)) at pH 5.659.

\[
\alpha_{HA} = \quad \quad \alpha_{A^-} =
\]

What is the quotient \(\frac{[A^-]}{[HA]}\) at pH 5.659?

\[
\frac{[A^-]}{[HA]} =
\]

**Exercise: Calculating Ion Concentrations**

**Task:**
Calculate the concentrations of hydronium ions, \( \text{H}_3\text{O}^+ \), and hydroxide ions, \( \text{OH}^- \), for a 0.0285 M HCl solution.

**Inputs:**
- [\( \text{H}_3\text{O}^+ \)] = **1.545 M** (Incorrect)
- [\( \text{OH}^- \)] = **12.45 M** (Incorrect)

**Instructions:**
Enter the correct numeric values for each ion concentration in the provided fields. The current entries are incorrect; reassess the calculations based on the given HCl concentration.

Understanding the dissociation of HCl in water and the resulting impact on ion concentrations is crucial:
- Remember that in a solution, \( \text{HCl} \) completely dissociates to produce equal concentrations of \( \text{H}_3\text{O}^+ \).
- Utilize the water dissociation constant, \( K_w \), to calculate \( \text{OH}^- \).

**Note:** This exercise helps to reinforce the concept of pH and equilibria in aqueous solutions.

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