10: Acids and Bases
- Page ID
- 15929
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Many of us are familiar with the group of chemicals called acids. But do you know what it takes for a compound to be an acid? Actually, there are several different definitions of acid that chemistry uses, and each definition is appropriate under different circumstances. Less familiar—but just as important to chemistry and ultimately to us—is the group of chemicals known as bases. Both acids and bases are important enough that we devote an entire chapter to them—their properties and their reactions.
- 10.0: Prelude to Acids and Bases
- This page discusses stomach acid production for digestion, highlighting the protective mucus layer and the regeneration of the stomach lining. It notes the risk of ulcers if cell replacement fails or due to Helicobacter pylori infection. Treatment options include antacids and antibiotics to manage these conditions.
- 10.1: Arrhenius Definition of Acids and Bases
- This page explains Arrhenius acids and bases, detailing their definitions, traits, naming conventions, and neutralization processes. It highlights neutralization reactions, such as calcium hydroxide with nitric acid and hydrocyanic acid with potassium hydroxide. Real-life applications include the use of antacids like calcium carbonate to neutralize stomach acid, with calculations shown for neutralizing HCl in various scenarios.
- 10.2: Brønsted-Lowry Definition of Acids and Bases
- This page discusses Brønsted-Lowry definitions of acids and bases, focusing on hydrogen ion transfer and examples of ammonia and water interactions. It highlights hydrochloric acid's behavior and practical applications of acids and bases, such as in pickling and neutralizing odors. The text also covers conjugate acid-base pairs, emphasizing their roles in reactions and drug solubility in the pharmaceutical industry.
- 10.3: Water - Both an Acid and a Base
- This page discusses the dual nature of water (H2O) as both a Brønsted-Lowry acid and base, capable of donating and accepting protons. It illustrates this with examples such as reactions with HCl and amide ions, and mentions water's autoionization into hydronium and hydroxide ions. The text emphasizes water as a prime example of amphiprotic compounds, while noting the rarity of pure water due to environmental influences.
- 10.4: The Strengths of Acids and Bases
- This page discusses the distinctions between strong and weak acids and bases, highlighting their ionization characteristics. Strong acids like HCl fully ionize, while weak acids do not. It elaborates on the pH scale, chemical equilibrium, and ionization constants (K_a and K_b). The autoionization of water (K_w) and the definitions of acidic, basic, and neutral solutions based on hydrogen and hydroxide ion concentrations are presented.
- 10.5: Buffers
- This page discusses buffers, which are solutions that stabilize pH by neutralizing added acids or bases. They consist of a weak acid and its conjugate base, preventing significant pH changes essential for biological functions, such as maintaining blood pH at 7.4. Examples include acetic acid with sodium acetate for bases and ammonia with ammonium chloride for acids.
- 10.E: Acids and Bases (Exercises)
- This page covers definitions of acids and bases, highlighting Arrhenius and Brønsted-Lowry theories. It details neutralization reactions, properties, and related calculations. The Brønsted-Lowry approach emphasizes proton donors and acceptors, with examples involving water's dual role. There’s an exploration of buffers, their preparation, and reactions when exposed to strong acids or bases, including distinctions between strong and weak acids.
- 10.S: Acids and Bases (Summary)
- This page covers important concepts of acids and bases, including their definitions according to Arrhenius and Brønsted-Lowry theories. It explains neutralization, distinguishes between strong and weak acids/bases, and introduces the pH scale for measuring acidity. Additionally, it discusses buffers and their role in maintaining pH stability.