7.4: Fundamentals of Solutions and Solubility
- Page ID
- 98417
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)Fundamentals of Solutions and Solubility
Welcome to the world of solutions and solubility! In this introduction, we'll explore the fascinating ways substances mix, dissolve, and interact to form solutions. These concepts are foundational in chemistry and have practical applications in everyday life, from making a cup of coffee to developing pharmaceuticals.
What is a Solution?
A solution is a homogeneous mixture where one substance (the solute) is uniformly dispersed in another substance (the solvent). The most common example is saltwater, where salt (solute) dissolves in water (solvent).
Key Points:
- Homogeneous: The mixture has a uniform composition throughout.
- Solute: The substance that is dissolved.
- Solvent: The substance that does the dissolving.
Types of Solutions
Solutions can exist in different phases:
- Gas in Gas: Air (oxygen in nitrogen).
- Liquid in Liquid: Vinegar (acetic acid in water).
- Solid in Liquid: Sugar in tea.
- Solid in Solid: Alloys like brass (zinc in copper).
Solubility
Solubility is the ability of a solute to dissolve in a solvent at a specific temperature and pressure. It determines how much solute can be dissolved to form a solution.
Factors Affecting Solubility:
- Nature of Solute and Solvent: "Like dissolves like" – polar solutes dissolve in polar solvents, and non-polar solutes dissolve in non-polar solvents.
- Example: Salt (polar) dissolves in water (polar), but not in oil (non-polar).
- Temperature: Solubility can increase or decrease with temperature.
- Example: Sugar dissolves better in hot water than in cold water.
- Pressure: Mainly affects gases; higher pressure increases gas solubility in liquids.
- Example: Carbon dioxide is more soluble in soda under high pressure.
Concentration of Solutions
Concentration describes how much solute is present in a given quantity of solvent or solution. Common units include:
- Molarity (M): Moles of solute per liter of solution.
- Percent Composition: Percentage of solute in the solution.
- Example: 10% saline solution contains 10 grams of salt in 100 grams of solution.
Saturation
A solution can be:
- Unsaturated: More solute can be dissolved.
- Saturated: Maximum amount of solute is dissolved.
- Supersaturated: Contains more dissolved solute than normally possible at a given temperature; unstable and can precipitate.
Real-Life Applications
Understanding solutions and solubility is crucial in various fields:
- Medicine: Dissolving drugs for effective delivery.
- Environmental Science: Pollutant behavior in water.
- Cooking: Achieving perfect flavor balance.
By grasping these fundamentals, you'll see how chemistry is at play in numerous aspects of daily life and technological advancements. Let's dive deeper into the wonders of solutions and their behavior!