7: Solutions Acids and Bases pH
- Page ID
- 121828
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 7.1: Introduction and Learning Objectives
- This page covers the basics of solutions, acids, bases, and the pH scale in chemistry. It discusses solubility factors, theories of acids and bases, their properties, and applications in daily life and industry. The text highlights effective teaching strategies, such as hands-on experiments and addressing misconceptions, while connecting these concepts to practical relevance in agriculture, medicine, and environmental science to enhance student interest and understanding.
- 7.2: The Dissolution Process
- A solution forms when two or more substances combine physically to yield a mixture that is homogeneous at the molecular level. The solvent is the most concentrated component and determines the physical state of the solution. The solutes are the other components typically present at concentrations less than that of the solvent. Solutions may form endothermically or exothermically, depending upon the relative magnitudes of solute and solvent intermolecular attractive forces.
- 7.3: Electrolytes
- Substances that dissolve in water to yield ions are called electrolytes. Electrolytes may be covalent compounds that chemically react with water to produce ions (for example, acids and bases), or they may be ionic compounds that dissociate to yield their constituent cations and anions, when dissolved. Dissolution of an ionic compound is facilitated by ion-dipole attractions between the ions of the compound and the polar water molecules.
- 7.4: Fundamentals of Solutions and Solubility
- This page explains solutions as homogeneous mixtures of solute and solvent, detailing types of solutions and factors affecting solubility like solute/solvent nature, temperature, and pressure. It addresses concentration and saturation levels, highlighting practical applications in medicine, environmental science, and cooking, demonstrating the relevance of chemistry in daily life.
- 7.5: Solubility
- The extent to which one substance will dissolve in another is determined by several factors, including the types and relative strengths of intermolecular attractive forces that may exist between the substances’ atoms, ions, or molecules. This tendency to dissolve is quantified as substance’s solubility, its maximum concentration in a solution at equilibrium under specified conditions. A saturated solution contains solute at a concentration equal to its solubility.
- 7.6: Arrhenius Acids and Bases
- Acids are very common in some of the foods that we eat. Citrus fruits such as oranges and lemons contain citric acid and ascorbic acid, which is better known as vitamin C (see figure below). Carbonated sodas contain phosphoric acid. Vinegar contains acetic acid. Your own stomach utilizes hydrochloric acid to digest food. Bases are less common as foods, but they are nonetheless present in many household products.
- 7.7: Brønsted-Lowry Acids and Bases
- This page discusses the evolution of acid-base theory, highlighting the transition from the Arrhenius concept, which faced limitations, to the Brønsted-Lowry definition introduced in 1923. This new theory defines acids as proton donors and bases as proton acceptors, including substances like ammonia that don't fit the Arrhenius framework. It expands the understanding of acid-base behavior by allowing bases to accept protons through anions or molecules with lone-pair electrons.
- 7.8: Introduction to Lewis Acids and Bases
- This page explains Lewis acids and bases as defined by G.N. Lewis in 1923, which expands traditional acid-base concepts beyond the Brønsted-Lowry definitions. Lewis describes acids as electron pair acceptors and bases as electron pair donors, providing a more comprehensive framework for understanding acid-base reactions, especially in cases where the Brønsted-Lowry theory falls short. The interactions lead to the formation of coordinate covalent bonds and the resulting adducts.
- 7.9: Lewis Acids and Bases
- This page discusses the Brønsted-Lowry and Lewis acid-base theories, focusing on proton transfer and electron-pair sharing in chemical reactions. The Brønsted-Lowry model highlights protons, while the Lewis theory prioritizes electron pairs, allowing reactions that do not involve proton transfer. Key concepts include recognizing proton donors and acceptors, examples of Lewis acid-base interactions, and the relevance of non-aqueous systems like ammonia.
- 7.10: Acid-Base Properties of Salt Solutions
- A salt can dissolve in water to produce a neutral, a basic, or an acidic solution, depending on whether it contains the conjugate base of a weak acid as the anion ( A−A− ), the conjugate acid of a weak base as the cation ( BH+ ), or both. Salts that contain small, highly charged metal ions produce acidic solutions in water. The reaction of a salt with water to produce an acidic or a basic solution is called a hydrolysis reaction.
- 7.11: Concept of Strong and Weak Acids and Bases
- This page explains the categorization of acids and bases into strong and weak based on their ionization in water. Strong acids and bases fully dissociate, yielding high concentrations of H⁺ or OH⁻ ions, which results in low or high pH and increased conductivity. Weak acids and bases only partially ionize, producing a smaller ion concentration, leading to higher pH and lower conductivity.
- 7.12: Relative Strengths of Acids and Bases
- The strengths of Brønsted-Lowry acids and bases in aqueous solutions can be determined by their acid or base ionization constants. Stronger acids form weaker conjugate bases, and weaker acids form stronger conjugate bases. Thus strong acids are completely ionized in aqueous solution because their conjugate bases are weaker bases than water. Weak acids are only partially ionized because their conjugate bases are compete successfully with water for possession of protons.
- 7.13: End of Chapter Activity
- This page outlines a lesson plan for 9th graders on solutions, acids, bases, and pH, incorporating AI tools and Bloom's Taxonomy. It aims to define key terms, design engaging experiments, and utilize AI for visuals and assessments. The lesson encourages hands-on activities and promotes the evaluation and synthesis of knowledge.
- 7.14: End of Chapter Key Terms
- This page offers a comprehensive overview of solutions, acids, bases, and pH, defining key terms like solute, solvent, and concentration. It explores types of solutions, properties of acids and bases, and the pH scale. Important concepts such as buffer solutions, titrations, acid-base reactions, the strength of acids and bases, neutralization reactions, and principles like Le Chatelier’s Principle and the ion product of water are also included.