---
title: "The graph below shows the percent ionization as a function of initial acid concentration for aqueous solutions of two weak monoprotic acids, \\(\\text{HA}\\) and \\(\\text{HB}\\), at \\(298\\text{ K}\\).  Based on the graph and principles of chemical equilibrium, which of the following claims is correct?"
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url: "https://nerd-notes.com/ubq/123851/"
date_modified: "2026-09-28T12:30:33+00:00"
---

# The graph below shows the percent ionization as a function of initial acid concentration for aqueous solutions of two weak monoprotic acids, \(\text{HA}\) and \(\text{HB}\), at \(298\text{ K}\).

Based on the graph and principles of chemical equilibrium, which of the following claims is correct?

The graph below shows the percent ionization as a function of initial acid concentration for aqueous solutions of two weak monoprotic acids, \(\text{HA}\) and \(\text{HB}\), at \(298\text{ K}\).

Based on the graph and principles of chemical equilibrium, which of the following claims is correct?

![A 2D line graph with labeled axes and a legend in the upper-right corner. The horizontal axis is labeled 'Initial Concentration (M)' and ranges from 0.00 to 0.20 with tick marks at 0.00, 0.05, 0.10, 0.15, and 0.20. The vertical axis is labeled 'Percent Ionization (%)' and ranges from 0 to 100 with tick marks at 0, 20, 40, 60, 80, and 100. Bare axes without internal gridlines. Two smooth curves start near the top-left at very low concentration and decay downward asymptotically toward the horizontal axis as concentration increases. Curve 1 is drawn as a solid line labeled in the legend as 'HA(aq)'; it starts near 90% at 0.005 M, falls steeply, and levels off to approximately 10% at 0.20 M. Curve 2 is drawn as a dashed line labeled in the legend as 'HB(aq)'; it starts near 50% at 0.005 M, falls steeply, and levels off to approximately 2% at 0.20 M. Curve 1 remains strictly above Curve 2 across all concentrations. No other particles, labels, text, or annotations appear.](https://nerd-notes.com/wp-content/uploads/ubq-frq-generated/stem-fig-1-1790598633-CNGXSp.jpg)

- **A.** \(\text{HB}\) is a stronger acid than \(\text{HA}\) because its percent ionization changes more rapidly at low concentrations, and a strong acid like \(\text{HCl}\) would display a horizontal line at \(0\%\) ionization.
- **B.** \(\text{HB}\) is a stronger acid than \(\text{HA}\) because it has a lower percent ionization at every concentration, and adding water shifts the dissociation equilibrium toward the undissociated acid molecules.
- **C.** \(\text{HA}\) is a stronger acid than \(\text{HB}\) because it ionizes to a greater extent at any given concentration, and for both acids, dilution causes \(Q < K_a\), shifting the equilibrium toward products to increase the fraction ionized.
- **D.** \(\text{HA}\) is a stronger acid than \(\text{HB}\) because its \(K_a\) increases as the solution is diluted, whereas a strong acid would display a curve of identical shape shifted upward.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123851/*