4.S: Reactions in Aqueous Solution (Summary)
- Page ID
- 91162
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\(\newcommand{\avec}{\mathbf a}\) \(\newcommand{\bvec}{\mathbf b}\) \(\newcommand{\cvec}{\mathbf c}\) \(\newcommand{\dvec}{\mathbf d}\) \(\newcommand{\dtil}{\widetilde{\mathbf d}}\) \(\newcommand{\evec}{\mathbf e}\) \(\newcommand{\fvec}{\mathbf f}\) \(\newcommand{\nvec}{\mathbf n}\) \(\newcommand{\pvec}{\mathbf p}\) \(\newcommand{\qvec}{\mathbf q}\) \(\newcommand{\svec}{\mathbf s}\) \(\newcommand{\tvec}{\mathbf t}\) \(\newcommand{\uvec}{\mathbf u}\) \(\newcommand{\vvec}{\mathbf v}\) \(\newcommand{\wvec}{\mathbf w}\) \(\newcommand{\xvec}{\mathbf x}\) \(\newcommand{\yvec}{\mathbf y}\) \(\newcommand{\zvec}{\mathbf z}\) \(\newcommand{\rvec}{\mathbf r}\) \(\newcommand{\mvec}{\mathbf m}\) \(\newcommand{\zerovec}{\mathbf 0}\) \(\newcommand{\onevec}{\mathbf 1}\) \(\newcommand{\real}{\mathbb R}\) \(\newcommand{\twovec}[2]{\left[\begin{array}{r}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\ctwovec}[2]{\left[\begin{array}{c}#1 \\ #2 \end{array}\right]}\) \(\newcommand{\threevec}[3]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\cthreevec}[3]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \end{array}\right]}\) \(\newcommand{\fourvec}[4]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\cfourvec}[4]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \end{array}\right]}\) \(\newcommand{\fivevec}[5]{\left[\begin{array}{r}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\cfivevec}[5]{\left[\begin{array}{c}#1 \\ #2 \\ #3 \\ #4 \\ #5 \\ \end{array}\right]}\) \(\newcommand{\mattwo}[4]{\left[\begin{array}{rr}#1 \amp #2 \\ #3 \amp #4 \\ \end{array}\right]}\) \(\newcommand{\laspan}[1]{\text{Span}\{#1\}}\) \(\newcommand{\bcal}{\cal B}\) \(\newcommand{\ccal}{\cal C}\) \(\newcommand{\scal}{\cal S}\) \(\newcommand{\wcal}{\cal W}\) \(\newcommand{\ecal}{\cal E}\) \(\newcommand{\coords}[2]{\left\{#1\right\}_{#2}}\) \(\newcommand{\gray}[1]{\color{gray}{#1}}\) \(\newcommand{\lgray}[1]{\color{lightgray}{#1}}\) \(\newcommand{\rank}{\operatorname{rank}}\) \(\newcommand{\row}{\text{Row}}\) \(\newcommand{\col}{\text{Col}}\) \(\renewcommand{\row}{\text{Row}}\) \(\newcommand{\nul}{\text{Nul}}\) \(\newcommand{\var}{\text{Var}}\) \(\newcommand{\corr}{\text{corr}}\) \(\newcommand{\len}[1]{\left|#1\right|}\) \(\newcommand{\bbar}{\overline{\bvec}}\) \(\newcommand{\bhat}{\widehat{\bvec}}\) \(\newcommand{\bperp}{\bvec^\perp}\) \(\newcommand{\xhat}{\widehat{\xvec}}\) \(\newcommand{\vhat}{\widehat{\vvec}}\) \(\newcommand{\uhat}{\widehat{\uvec}}\) \(\newcommand{\what}{\widehat{\wvec}}\) \(\newcommand{\Sighat}{\widehat{\Sigma}}\) \(\newcommand{\lt}{<}\) \(\newcommand{\gt}{>}\) \(\newcommand{\amp}{&}\) \(\definecolor{fillinmathshade}{gray}{0.9}\)- aqueous solutions – solutions in which water is the dissolving medium
4.1: General Properties of Aqueous Solutions
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- electrolyte – substance whose aqueous solution contains ions
- nonelectrolyte – substance that does not form ions in solution
4.2.1 Ionic Compounds in Water
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- dissociate – when ions separate from a solid being dissolved
4.2.2 Molecular Compounds in Water
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- the molecular structure is maintained
4.2.3 Strong and Weak Electrolytes
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- strong electrolytes – ionic compounds that exists entirely of ions in solution
- weak electryolytes – molecular compounds that produce a small amound of ions
- chemical equilibrium – equilibrium of forming ions and recrystalizing ions
4.2: Precipitation Reactions
\[AX + BY \rightarrow AY + BX\]
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- for methathesis to occur:
- 1) the formation of an insoluble product
- 2) the formation of either a weak electrolyte or a nonelectrolyte
- 3) the formation of a gas that escapes from solution
4.5.1 Precipitation Reactions
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- precipitate – insoluble solid formed by a reaction in solution
- solubility – amount of substance that can be dissolved in a given quantity
4.5.2 Solubility Guidelines for Ionic Compounds
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- all common ionic compounds of the alkali metal ions and of the ammonium ion are soluble in water
4.5.3 Reactions in Which a Weak Electrolyte or Nonelectrolyte Forms
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- hydrogen and hydroxide react to form water
- insoluble metal oxides react with acids
4.3: Acid-Base Reactions
4.3.1 Acids
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- substances that ionize to form hydrogen ions
- proton donors
4.3.2 Bases
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- substances that ionize to form hydroxide ions
4.3.3 Strong and Weak Acids and Bases
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- strong acid, strong base – strong electrolyte
- weak acid, weak base – weak electrolyte
4.3.4 Neutralization Reactions and Salts
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- neutralization reaction – when an acid and base are mixed
- produces water and a salt
4.4 Ionic Equations
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- molecular formula – and equation written to show the complete chemical formulas of reactants and products
- spectator ions – ions that do not play a role in a reaction
- net ionic equation – equation where the spectator ions are removed
- only soluble strong electrolytes are written in ionic form
4.4: Oxidation-Reduction Reactions
4.6.1 Reactions in Which a Gas Forms
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- carbonates and bicarbonates
4.6.2 Oxidation and Reduction
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- oxidation – loss of electrons
- reduction – gain of electrons
4.6.3 Oxidation of Metals by Acids and Salts
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- whenever one substance is oxidized, some other substance must be reduced
- metals react with acids to form salts and hydrogen gas
4.6.4 The Activity Series
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- activity series – list of metals arranged in order of decreasing ease of oxidation
- active metals – alkali metals and alkaline earth metals
- any metla on the list can be oxidized by ions of elements below it
4.5: Concentration of Solutions
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- solution – homogeneous mixture of two or more substances
- solvent – component that is present in greatest quantity
- solutes – substances dissolved in the solvent
4.1.1 Molarity
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- concentration – the amount of solute dissolved in a given quantity of solvent or solution
- molarity – number of moles of solute in a liter of solution
4.1.2 Dilution
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- dilution - obtaining a lower concentration of a solution by adding water
- moles solute before dilution = moles solute after dilution
4.6: Solution Stoichiometry and Chemical Analysis
4.7.1 Titrations
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- statndard solution – solution of known concentration
- titration – a known solution that undergoes a specific chemical reaction of known stoichiometry with the solution of unknown concentration
- equivalence point – stoichiometrically equivalent quantities of reactants are brought together
- indicator – used to show the endpoint of the titration