---
title: "A student investigates the enthalpy of neutralization by mixing solutions of a strong acid and a strong base in an insulated coffee-cup calorimeter. The data collected during the experiment are shown in the table below.  | Quantity | Value | |—|—| | Volume of \\(1.00\\text{ M HCl(aq)}\\) | \\(50.0\\text{ mL}\\) | | Volume of \\(1.50\\text{ M NaOH(aq)}\\) | \\(50.0\\text{ mL}\\) | | Initial temperature of both solutions | \\(21.3^\\circ\\text{C}\\) | | Maximum temperature reached after mixing | \\(28.0^\\circ\\text{C}\\) |  \\[\\text{H}^+\\text{(aq)} + \\text{OH}^-\\text{(aq)} \\rightarrow \\text{H}_2\\text{O(l)}\\]  Assuming the resulting mixture has a density of \\(1.00\\text{ g/mL}\\) and a specific heat capacity of \\(4.18\\text{ J}/(\\text{g}\\cdot^\\circ\\text{C})\\), what is the experimental value of \\(\\Delta H^\\circ_{\\text{rxn}}\\) for the neutralization reaction in \\(\\text{kJ/mol}_{\\text{rxn}}\\) of \\(\\text{H}_2\\text{O(l)}\\) formed?"
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url: "https://nerd-notes.com/ubq/123816/"
date_modified: "2026-09-28T12:30:24+00:00"
---

# A student investigates the enthalpy of neutralization by mixing solutions of a strong acid and a strong base in an insulated coffee-cup calorimeter. The data collected during the experiment are shown in the table below.

| Quantity | Value |
|—|—|
| Volume of \(1.00\text{ M HCl(aq)}\) | \(50.0\text{ mL}\) |
| Volume of \(1.50\text{ M NaOH(aq)}\) | \(50.0\text{ mL}\) |
| Initial temperature of both solutions | \(21.3^\circ\text{C}\) |
| Maximum temperature reached after mixing | \(28.0^\circ\text{C}\) |

\[\text{H}^+\text{(aq)} + \text{OH}^-\text{(aq)} \rightarrow \text{H}_2\text{O(l)}\]

Assuming the resulting mixture has a density of \(1.00\text{ g/mL}\) and a specific heat capacity of \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\), what is the experimental value of \(\Delta H^\circ_{\text{rxn}}\) for the neutralization reaction in \(\text{kJ/mol}_{\text{rxn}}\) of \(\text{H}_2\text{O(l)}\) formed?

A student investigates the enthalpy of neutralization by mixing solutions of a strong acid and a strong base in an insulated coffee-cup calorimeter. The data collected during the experiment are shown in the table below.

| Quantity | Value |
|---|---|
| Volume of \(1.00\text{ M HCl(aq)}\) | \(50.0\text{ mL}\) |
| Volume of \(1.50\text{ M NaOH(aq)}\) | \(50.0\text{ mL}\) |
| Initial temperature of both solutions | \(21.3^\circ\text{C}\) |
| Maximum temperature reached after mixing | \(28.0^\circ\text{C}\) |

\[\text{H}^+\text{(aq)} + \text{OH}^-\text{(aq)} \rightarrow \text{H}_2\text{O(l)}\]

Assuming the resulting mixture has a density of \(1.00\text{ g/mL}\) and a specific heat capacity of \(4.18\text{ J}/(\text{g}\cdot^\circ\text{C})\), what is the experimental value of \(\Delta H^\circ_{\text{rxn}}\) for the neutralization reaction in \(\text{kJ/mol}_{\text{rxn}}\) of \(\text{H}_2\text{O(l)}\) formed?

- **A.** \(-56\text{ kJ/mol}_{\text{rxn}}\)
- **B.** \(-37\text{ kJ/mol}_{\text{rxn}}\)
- **C.** \(-28\text{ kJ/mol}_{\text{rxn}}\)
- **D.** \(+56\text{ kJ/mol}_{\text{rxn}}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/123816/*