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title: "A student compares two monoprotic weak acids, \\(\\text{HA(aq)}\\) and \\(\\text{HB(aq)}\\), at \\(25^\\circ\\text{C}\\). The acid ionization constant \\(K_a\\) for \\(\\text{HA}\\) is \\(1.0 \\times 10^{-4}\\), and the \\(K_a\\) for \\(\\text{HB}\\) is \\(1.0 \\times 10^{-6}\\). What is the value of the ratio \\(\\dfrac{K_b(\\text{A}^-)}{K_b(\\text{B}^-)}\\) for their conjugate bases at \\(25^\\circ\\text{C}\\)?"
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url: "https://nerd-notes.com/ubq/119297/"
date_modified: "2026-08-19T12:39:42+00:00"
---

# A student compares two monoprotic weak acids, \(\text{HA(aq)}\) and \(\text{HB(aq)}\), at \(25^\circ\text{C}\). The acid ionization constant \(K_a\) for \(\text{HA}\) is \(1.0 \times 10^{-4}\), and the \(K_a\) for \(\text{HB}\) is \(1.0 \times 10^{-6}\). What is the value of the ratio \(\dfrac{K_b(\text{A}^-)}{K_b(\text{B}^-)}\) for their conjugate bases at \(25^\circ\text{C}\)?

A student compares two monoprotic weak acids, \(\text{HA(aq)}\) and \(\text{HB(aq)}\), at \(25^\circ\text{C}\). The acid ionization constant \(K_a\) for \(\text{HA}\) is \(1.0 \times 10^{-4}\), and the \(K_a\) for \(\text{HB}\) is \(1.0 \times 10^{-6}\). What is the value of the ratio \(\dfrac{K_b(\text{A}^-)}{K_b(\text{B}^-)}\) for their conjugate bases at \(25^\circ\text{C}\)?

- **A.** \(1.0 \times 10^{-2}\)
- **B.** \(1.0 \times 10^{-1}\)
- **C.** \(1.0 \times 10^1\)
- **D.** \(1.0 \times 10^2\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119297/*