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title: "A student prepares two separate acid solutions at \\(25\\ ^\\circ\\text{C}\\):  Sample 1 contains \\(50.0\\text{ mL}\\) of \\(\\text{HCl(aq)}\\) at \\(\\text{pH} = 3.00\\).  Sample 2 contains \\(50.0\\text{ mL}\\) of a weak monoprotic acid, \\(\\text{HA(aq)}\\) (\\(K_a = 1.0 \\times 10^{-5}\\)), at \\(\\text{pH} = 3.00\\).  Each sample is titrated to its equivalence point with standardized \\(0.100\\text{ M NaOH(aq)}\\). Let \\(V_1\\) be the volume of \\(\\text{NaOH(aq)}\\) required to reach the equivalence point for Sample 1, and let \\(V_2\\) be the volume required for Sample 2. Which of the following correctly compares \\(V_1\\) and \\(V_2\\), and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/123830/"
date_modified: "2026-09-28T12:30:28+00:00"
---

# A student prepares two separate acid solutions at \(25\ ^\circ\text{C}\):

Sample 1 contains \(50.0\text{ mL}\) of \(\text{HCl(aq)}\) at \(\text{pH} = 3.00\).

Sample 2 contains \(50.0\text{ mL}\) of a weak monoprotic acid, \(\text{HA(aq)}\) (\(K_a = 1.0 \times 10^{-5}\)), at \(\text{pH} = 3.00\).

Each sample is titrated to its equivalence point with standardized \(0.100\text{ M NaOH(aq)}\). Let \(V_1\) be the volume of \(\text{NaOH(aq)}\) required to reach the equivalence point for Sample 1, and let \(V_2\) be the volume required for Sample 2. Which of the following correctly compares \(V_1\) and \(V_2\), and provides the correct justification?

A student prepares two separate acid solutions at \(25\ ^\circ\text{C}\):

Sample 1 contains \(50.0\text{ mL}\) of \(\text{HCl(aq)}\) at \(\text{pH} = 3.00\).

Sample 2 contains \(50.0\text{ mL}\) of a weak monoprotic acid, \(\text{HA(aq)}\) (\(K_a = 1.0 \times 10^{-5}\)), at \(\text{pH} = 3.00\).

Each sample is titrated to its equivalence point with standardized \(0.100\text{ M NaOH(aq)}\). Let \(V_1\) be the volume of \(\text{NaOH(aq)}\) required to reach the equivalence point for Sample 1, and let \(V_2\) be the volume required for Sample 2. Which of the following correctly compares \(V_1\) and \(V_2\), and provides the correct justification?

- **A.** \(V_2 > V_1\), because \(\text{HA}\) is only partially ionized, meaning a much greater total concentration of undissociated acid is present to yield \(\text{pH} = 3.00\), providing more titratable protons.
- **B.** \(V_2 > V_1\), because the equivalence point for a weak acid titration occurs at \(\text{pH} > 7.00\), requiring additional moles of \(\text{OH}^-\text{(aq)}\) to reach the more basic equivalence region.
- **C.** \(V_1 > V_2\), because the strong acid is completely ionized in solution, releasing all of its protons immediately, whereas the weak acid only releases a small fraction of its protons.
- **D.** \(V_1 = V_2\), because both samples have identical initial \([\text{H}_3\text{O}^+]\) and equal solution volumes, containing the same number of reactive protons to be neutralized.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123830/*