13.1: Tables
- Page ID
- 545601
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 13.1.2: Fundamental Physical Constants
- This page presents a list of essential physical constants with their names, symbols, and values, including key constants like the atomic mass unit, Avogadro's number, Boltzmann's constant, the electron charge and mass, Faraday's constant, and Planck's constant. It also includes molar volumes of ideal gases under specific conditions and the speed of light. These constants are crucial for calculations and understanding phenomena in physics and chemistry.
- 13.1.3: Water Properties
- This page provides an overview of the physical properties of water such as density, vapor pressure, and ion product (Kw). It highlights that water's maximum density is at 4°C, outlines standard melting and boiling temperatures with their enthalpies, and presents cryoscopic and ebullioscopic constants. Additionally, it mentions the spectral absorption of water, though without specific details.
- 13.1.4: Composition of Commercial Acids and Bases
- This page presents a table detailing the properties of various commercial acids and bases, such as acetic acid and hydrochloric acid, focusing on density, mass percentage, and molarity. It notes that these acids and bases are usually found in aqueous solutions and clarifies the importance of specific gravity. Furthermore, it corrects the common misconception that aqueous ammonia should be referred to as "ammonium hydroxide."
- 13.1.5: Standard Thermodynamic Properties for Selected Substances
- This page provides comprehensive data on standard thermodynamic properties for various substances, including elements and compounds in solid, liquid, and gaseous states. Key properties such as enthalpy of formation, Gibbs free energy, and entropy at 298 K are presented for a diverse range of substances, including metals, organic compounds, and metal oxides.
- 13.1.6: Ionization Constants of Weak Acids
- This page provides a list of weak acids, including acetic, carbonic, formic, and phosphoric acids, along with their chemical formulas and ionization constants (Ka) at 25 °C. It highlights that Ka values indicate acid strength, with lower values corresponding to weaker acids. The page underscores the significance of ionization constants for comprehending acid strength and behavior in chemical reactions.
- 13.1.7: Ionization Constants of Weak Bases
- This page discusses the ionization constants (Kb) of several weak bases at 25 °C, including ammonia, dimethylamine, methylamine, phenylamine, and trimethylamine. It explains that Kb values measure the strength of each base's proton-accepting ability, with lower values signifying weaker bases.
- 13.1.8: Solubility Products
- This page provides a detailed list of substances and their solubility products (Ksp) at 25 °C, highlighting the solubility of various compounds from elements like aluminum and barium. It showcases the significant variation in Ksp values, which influences chemical reactions and environmental processes.
- 13.1.9: Formation Constants for Complex Ions
- This page presents formation constants (Kf) for complex ions, highlighting the equilibrium between metal cations (e.g., Al, Cu, Fe) and ligands (e.g., fluoride, ammonia). The Kf values vary widely, reflecting the stability of these metal-ligand complexes, with some showing strong interactions due to high formation constants.
- 13.1.10: Standard Electrode (Half-Cell) Potentials
- This page details standard electrode potentials for various redox half-reactions, showcasing voltages associated with ions like Ag+, Al3+, and halogens. It illustrates the tendency of these species to gain electrons, with positive values indicating strong oxidizing agents and negative values indicating reducing agents.
- 13.1.11: Half-Lives for Several Radioactive Isotopes
- This page presents a detailed table of radioactive isotopes, highlighting their half-lives and types of emissions, such as beta, alpha, electron capture, and spontaneous fission. The isotopes are categorized by half-life, which varies significantly. This information is essential for grasping the stability and decay mechanisms of isotopes in scientific and medical contexts.