10: Enthalpy of Neutralization
- Page ID
- 514172
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- To use coffee-cup calorimetry to determine the enthalpy of neutralization of two acids, hydrochloric acid and acetic acid, with sodium hydroxide.
INTRODUCTION
Enthalpy of neutralization is the heat released or absorbed when an acid and a base react to form water in a neutralization reaction. In this experiment, the enthalpy of neutralization for two different acid-base reactions will be determined using a coffee-cup calorimeter, which is a simple device used to measure heat changes in chemical reactions at constant pressure.
The first reaction involves a strong acid (\(\ce{HCl}\)) and a strong base (\(\ce{NaOH}\)), while the second reaction involves a weak acid (\(\ce{CH3CO2H}\)) and a strong base (\(\ce{NaOH}\)). Since strong acids and strong bases completely dissociate in water, their neutralization reaction typically releases more heat compared to a weak acid that only partially ionizes. By measuring the temperature changes during these reactions, the heat released can be calculated and used to determine the enthalpy of neutralization.
Additionally, the heat capacity of the calorimeter will be determined to account for heat absorption by the apparatus. Understanding these enthalpy changes provides insight into acid-base thermodynamics and the energy differences between strong and weak acids.
- 10.1: Enthalpy of Neutralization - Experiment
- This page provides essential safety guidelines for handling corrosive chemicals such as sodium hydroxide and hydrochloric acid, highlighting the importance of ventilation and quick rinsing during spills. It details the materials and procedures needed for using a coffee-cup calorimeter to measure heat capacity and determine the enthalpy of neutralization for reactions involving \(\ce{NaOH}\), \(\ce{HCl}\), and acetic acid. Additionally, it addresses proper chemical waste disposal methods.
- 10.2: Enthalpy of Neutralization - Pre-lab
- This page covers the First Law of Thermodynamics, highlighting the principle of zero heat exchange between a system and its surroundings. It includes a practical example of enthalpy of neutralization using NaOH and HCl, encouraging students to identify the limiting reactant and calculate enthalpy change. Furthermore, it outlines three methods for determining enthalpy changes—calorimetry, Hess's Law, and standard enthalpies of formation—focusing on the calculation using thermochemical data.
- 10.3: Enthalpy of Neutralization - Data and Report
- This page describes a calorimetry experiment in three parts: Part A measures the heat capacity of a calorimeter; Part B analyzes the enthalpy of neutralization for hydrochloric acid and sodium hydroxide; and Part C examines the neutralization of acetic acid with sodium hydroxide. The page includes temperature change data, calculations of heat transfer, and concludes with post-lab questions on specific heat capacity and enthalpy comparisons.