---
title: "A student prepares an aqueous solution of a weak monoprotic acid, \\(\\text{HA}\\), by dissolving \\(0.010 \\text{ mol}\\) of pure \\(\\text{HA(s)}\\) in distilled water to give a total volume of \\(250 \\text{ mL}\\). The acid dissociation constant, \\(K_a\\), for \\(\\text{HA}\\) is \\(6.4 \\times 10^{-5}\\) at \\(25^\\circ\\text{C}\\). What is the percent ionization of \\(\\text{HA}\\) in this solution?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/121484/"
date_modified: "2026-08-23T05:04:49+00:00"
---

# A student prepares an aqueous solution of a weak monoprotic acid, \(\text{HA}\), by dissolving \(0.010 \text{ mol}\) of pure \(\text{HA(s)}\) in distilled water to give a total volume of \(250 \text{ mL}\). The acid dissociation constant, \(K_a\), for \(\text{HA}\) is \(6.4 \times 10^{-5}\) at \(25^\circ\text{C}\). What is the percent ionization of \(\text{HA}\) in this solution?

A student prepares an aqueous solution of a weak monoprotic acid, \(\text{HA}\), by dissolving \(0.010 \text{ mol}\) of pure \(\text{HA(s)}\) in distilled water to give a total volume of \(250 \text{ mL}\). The acid dissociation constant, \(K_a\), for \(\text{HA}\) is \(6.4 \times 10^{-5}\) at \(25^\circ\text{C}\). What is the percent ionization of \(\text{HA}\) in this solution?

- **A.** \(0.16\%\)
- **B.** \(2.0\%\)
- **C.** \(4.0\%\)
- **D.** \(8.0\%\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121484/*