11: Solutions
- Page ID
- 568678
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- 11.1: Solutions - Homogeneous Mixtures
- This page covers solutions, defining solvents and solutes and illustrating the "like dissolves like" principle regarding polarity. It explains how polar solutes dissolve in polar solvents and nonpolar solutes in nonpolar solvents, emphasizing the role of intermolecular forces. Various examples are provided to demonstrate solubility based on polarity relative to water and other solvents.
- 11.2: Solutions of Solids Dissolved in Water
- This page provides an overview of solutions, defining electrolytes and nonelectrolytes, highlighting water's role as a universal solvent. It discusses solubility, saturation, and how temperature affects solubility, with solid solutes generally increasing in solubility while gases decrease. The page explains the dissociation of ionic compounds in water and emphasizes the classification of solutions as saturated or unsaturated based on solute levels relative to solubility limits.
- 11.3: Calculating Solution Concentration- Molarity (is a Conversion Factor!)
- This page covers molarity, essential for expressing solution concentration in chemistry. It explains how to calculate molarity, convert mass of solute to moles, and apply molarity in stoichiometric calculations for laboratory needs. Furthermore, it details how to determine mass from molarity and volume using potassium permanganate as an example, with a focus on using molarity as a conversion factor and concentration notation.
- 11.4: Solution Dilution (M1V1 = M2V2)
- This page covers solution concentrations, explaining the differences between dilute and concentrated solutions. It defines stock solutions and how to use them to prepare a dilution in a volumetric flask. The significance of dilutions is highlighted, emphasizing that adding solvent alters volume and concentration while maintaining constant solute moles, demonstrated through the equation \(M_1V_1 = M_2V_2\).
- 11.5: Calculating Solution Concentration- Mass Percent
- This page covers solution concentration, distinguishing between dilute and concentrated solutions. It introduces mass percent (% m/m) as a method for expressing concentration, detailing its calculation by dividing the mass of solute by the mass of the solution and multiplying by 100. Practical examples and exercises reinforce the significance of precise measurements in solution preparation and chemistry.
- 11.6: Solution Stoichiometry
- This page explains how to quantitate amounts of reactants and products (stoichiometry) in double replacement reactions in aqueous solutions, using molarity as a conversion factor. The text highlights the steps to solve for solution stoichiometry problems through a balanced chemical equation and using molarity, as a conversion factor, to convert in or out of moles of solute.