10: Acids and Bases
- Page ID
- 86250
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 10.1: Acids and Bases Definitions
- This page covers the classification of acids and bases through the Arrhenius and Brønsted-Lowry theories. It explains Arrhenius acids and bases, their limitations, and the broader definition of the Brønsted-Lowry theory, which categorizes acids as proton donors and bases as proton acceptors.
- 10.2: Acid and Base Strength
- This page explains the difference between strong and weak acids and bases, focusing on their ionization in water. Strong acids, such as hydrochloric acid, fully dissociate, while weak acids, like acetic acid, only partially do so. The page also discusses dynamic chemical equilibrium and provides examples relevant to common substances.
- 10.3: Acid Dissociation Constants
- This page explains acid dissociation constants (\(K_a\)) and their significance in assessing weak acid strength through the ionization of a general weak acid, \(\ce{HA}\). It presents the \(K_a\) expression that reflects equilibrium between ionized and non-ionized forms. Strong acids, typically not reported due to complete ionization, have higher \(K_a\) values.
- 10.4: Water as Both an Acid and a Base
- This page explores the amphiprotic nature of water, which can function as either an acid or base by donating or accepting protons. It discusses the autoionization of water into hydronium and hydroxide ions and introduces the ion-product constant \(K_w\). The relationship between hydrogen and hydroxide ion concentrations is examined, alongside examples using strong acids and bases. The page clarifies how water's dual role affects its classification as neutral under certain conditions.
- 10.5: Measuring Acidity in Aqueous Solutions- The pH Scale
- This page discusses the pH scale, which measures acidity and basicity based on hydronium ion concentration, with values indicating different acidic or basic conditions. It highlights the relevance of pH in health and environmental contexts, addressing acid rain, its causes, and ecological impact. While regulations in North America and Europe have reduced acid rain damage, it continues to affect areas in China and India, worsening tree health, soil nutrient depletion, and corroding monuments.
- 10.6: Working with pH
- This page explains how to calculate pH from hydronium ion concentration \([H_3O^+]\) and vice versa using logarithms. It includes examples, highlights the importance of significant figures, and offers calculator guidance for these conversions, ensuring clarity in both methods.
- 10.7: Acid and Base Equivalents
- This page discusses the development of maps, highlighting the time required for locating or creating matching materials. LibreTexts emphasizes delivering completed pages rather than delaying the project. Though the current map is not fully finished and has some missing pages, efforts are ongoing to complete it.
- 10.8: Some Common Acid-Base Reactions
- This page outlines the map-building process for the LibreTexts project, highlighting the time needed to collect or create materials. It emphasizes a progressive release of completed pages rather than delaying for full project completion, and notes that the current map remains incomplete with some pages still under development.
- 10.9: Acidity and Basicity of Salt Solutions
- This page explains the acidity, basicity, or neutrality of salt solutions depending on their source. It details how salts formed from weak acids and strong bases produce basic solutions, while those from strong acids and weak bases yield acidic solutions. Salts from strong acid-strong base pairs create neutral solutions. A table illustrates the outcomes based on the acid-base strength of the reactants.
- 10.10: Buffer Solutions
- This page covers buffer solutions, comprising weak acids and bases that stabilize pH against strong acid or base additions, illustrated with examples like acetic acid and sodium acetate. It contrasts buffered solutions with unbuffered ones, highlighting minimal pH changes with buffers (e.g., acetic acid) versus significant changes in unbuffered scenarios.
- 10.11: Titration
- This page covers titrations, a quantitative analytical method for determining the concentration of an acid or base. It explains the functions of the titrant and analyte, the importance of burettes for accuracy, and introduces the equivalence point. It also includes calculations for determining moles and mass of reactants, and highlights the role of indicators in identifying the equivalence point during the titration process.