Skip to main content
Physics LibreTexts

7.14: End of Chapter Key Terms

  1. Last updated
  2. Save as PDF
  • Page ID
    96544

    • \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

    \( \newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\)

    ( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\id}{\mathrm{id}}\)

    \( \newcommand{\Span}{\mathrm{span}}\)

    \( \newcommand{\kernel}{\mathrm{null}\,}\)

    \( \newcommand{\range}{\mathrm{range}\,}\)

    \( \newcommand{\RealPart}{\mathrm{Re}}\)

    \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\)

    \( \newcommand{\Argument}{\mathrm{Arg}}\)

    \( \newcommand{\norm}[1]{\| #1 \|}\)

    \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\)

    \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\AA}{\unicode[.8,0]{x212B}}\)

    \( \newcommand{\vectorA}[1]{\vec{#1}}      % arrow\)

    \( \newcommand{\vectorAt}[1]{\vec{\text{#1}}}      % arrow\)

    \( \newcommand{\vectorB}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vectorC}[1]{\textbf{#1}} \)

    \( \newcommand{\vectorD}[1]{\overrightarrow{#1}} \)

    \( \newcommand{\vectorDt}[1]{\overrightarrow{\text{#1}}} \)

    \( \newcommand{\vectE}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{\mathbf {#1}}}} \)

    \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}} } \)

    \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash {#1}}} \)

    \(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)

    Solutions, Acids, Bases, and pH

    1. Solution: A homogeneous mixture composed of two or more substances, where one substance (solute) is dissolved in another (solvent).
    2. Solute: The substance that is dissolved in a solution.
    3. Solvent: The substance that dissolves the solute to form a solution; usually the component in greater quantity.
    4. Concentration: The amount of solute present in a given quantity of solvent or solution; commonly expressed in molarity (M), which is moles of solute per liter of solution.
    5. Molarity (M): A unit of concentration, defined as the number of moles of solute per liter of solution.
    6. Solubility: The maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure.
    7. Saturated Solution: A solution that contains the maximum amount of dissolved solute at a given temperature and pressure.
    8. Unsaturated Solution: A solution that contains less than the maximum amount of dissolved solute at a given temperature and pressure.
    9. Supersaturated Solution: A solution that contains more dissolved solute than it would under normal circumstances, typically achieved by changing the temperature or pressure.
    10. Dilution: The process of reducing the concentration of a solute in solution, usually by adding more solvent.
    11. Acid: A substance that donates hydrogen ions (H⁺) in an aqueous solution; characterized by a sour taste and the ability to turn blue litmus paper red.
    12. Base: A substance that accepts hydrogen ions (H⁺) or donates hydroxide ions (OH⁻) in an aqueous solution; characterized by a bitter taste and slippery feel, and the ability to turn red litmus paper blue.
    13. pH Scale: A logarithmic scale used to measure the acidity or basicity of a solution, ranging from 0 to 14, where 7 is neutral, values below 7 are acidic, and values above 7 are basic.
    14. pH: The negative logarithm of the hydrogen ion concentration in a solution, pH = -log[H⁺].
    15. pOH: The negative logarithm of the hydroxide ion concentration in a solution, pOH = -log[OH⁻].
    16. pKa: The negative logarithm of the acid dissociation constant (Ka), a measure of the strength of an acid; lower pKa values indicate stronger acids.
    17. pKb: The negative logarithm of the base dissociation constant (Kb), a measure of the strength of a base; lower pKb values indicate stronger bases.
    18. Buffer: A solution that resists changes in pH upon the addition of small amounts of an acid or base, typically composed of a weak acid and its conjugate base or a weak base and its conjugate acid.
    19. Acid-Base Titration: A laboratory technique used to determine the concentration of an acid or base by reacting it with a standard solution of known concentration.
    20. Equivalence Point: The point in a titration at which the amount of titrant added is exactly enough to completely neutralize the analyte solution.
    21. Indicator: A substance that changes color at a specific pH range, used to determine the endpoint of a titration.
    22. Strong Acid: An acid that completely ionizes in aqueous solution (e.g., hydrochloric acid, HCl).
    23. Weak Acid: An acid that partially ionizes in aqueous solution (e.g., acetic acid, CH₃COOH).
    24. Strong Base: A base that completely dissociates in aqueous solution (e.g., sodium hydroxide, NaOH).
    25. Weak Base: A base that partially ionizes or dissociates in aqueous solution (e.g., ammonia, NH₃).
    26. Acid Dissociation Constant (Ka): A quantitative measure of the strength of an acid in solution, given by the equilibrium constant for the dissociation of the acid into its conjugate base and a hydrogen ion.
    27. Base Dissociation Constant (Kb): A quantitative measure of the strength of a base in solution, given by the equilibrium constant for the dissociation of the base into its conjugate acid and a hydroxide ion.
    28. Neutralization Reaction: A chemical reaction in which an acid and a base react to form water and a salt.
    29. Salt: An ionic compound formed from the neutralization reaction of an acid and a base.
    30. Le Chatelier’s Principle: A principle stating that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
    31. Hydronium Ion (H₃O⁺): A water molecule with an extra proton, representing the form in which hydrogen ions exist in aqueous solution.
    32. Autoionization of Water: The process by which water molecules dissociate into hydrogen ions (H⁺) and hydroxide ions (OH⁻), expressed as H2O⇌H++OH−H_2O \rightleftharpoons H^+ + OH^-H2​O⇌H++OH−.
    33. Ion Product of Water (Kw): The product of the concentrations of hydrogen ions and hydroxide ions in water, equal to 1.0×10−141.0 \times 10^{-14}1.0×10−14 at 25°C.
    34. Standard Solution: A solution of known concentration used in titrations.
    35. Molar Mass: The mass of one mole of a substance, usually expressed in grams per mole (g/mol).

    7.14: End of Chapter Key Terms is shared under a CC BY-NC-SA license and was authored, remixed, and/or curated by LibreTexts.