Chem 4

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Solvent

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present in greatest amount

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Solute

Back 2

present in lesser amount(s)

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insoluble

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does not dissolve to a significant amount in the solvent

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hydrated

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surrounded by water molecules (H2O)

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solvated

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surrounded by solvent molecules

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Concentration (Conc)

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refers to a specific composition

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concentrated solution

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contains a relatively high concentration of solute relative to solvent

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dilute solution

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contains a relatively low concentration of solute relative to solvent

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Molarity (M)

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moles od solute / liter of solution

mol solute / L soln

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3M H_3PO_4 means...

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3 moles H_3PO_4 / 1 L soln

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M=

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mol solute / V

mol solute = M x V

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electrolyte

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a substance that dissolves in water to form an electrically conductive solution
- anything that dissolves in water to form ions

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non-electrolyte

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a substance that dissolves in water to form a solution that does not conduct electricity

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strong electrolyte

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essentially completely ionized in solution
-forms high concentration of ions
-gives rise to a high electrical conductivity
Examples
soluble ionic compounds
strong acids
strong bases

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Weak electrolyte

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only partially ionized in solution
-forms a low concentration of ions
-gives rise to a low electrical conductivity
Examples
weak acids
weak bases

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spectator ions

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not involved in reaction

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net ionic equation

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with out spectator ions

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solubility

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the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature

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Simple rules for the solubility of salts in water

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1. most nitrate (NO_3_^-^) salts are soluble
2. most salts containing alkali metals ions (Li^+, Na^+, K^+, Cs^+, Rb^+) and ammonium ion (NH_4_^+) are soluble
3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag^+, PB^2+, Hg_2_^2+
4. Most sulfate salts are soluble. Notable exceptions are BaSO_4, PbSO_4, HgSO_4 and CaSO_4
5. Most hydroxides are only slightly soluble. The important soluble hydroxides are NaOH, and KOH. The compounds Ba(OH)_2, Sr(OH)_2, and Ca(OH)_2 are marginally soluble
6. Most silfide (S^2-), carbonate (CO_3_^2-), chromate (CrO_4_^2-), and phosphate (PO_4_^3-) salts are only slightly soluble, except for those containing the cations in rule 2

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formula equation

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gives overall reaction stoichiometry but not necessarily the actual forms of the reactants and products in solution

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Complete ionic equation

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represents as ions all reactants and products that are strong electrolytes

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net ionic equation

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includes only those solution components undergoing a change. Spectator ions not included

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Arrhenius proposed...

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that an acid is a substance that produces H+ ions (protons) when it is dissolved in water

Base dissolves in water to form OH^- (hydroxide ions)

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Bronsted-Lowery theory

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reaction between acids and base involves H^+ transfer
Acid proton donar
Base proton acceptor

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Neutralization reaction

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a reaction between an acid and a base to give a salt and water

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Salt

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an ionic compound produced from a neutralization reaction that contains the cation from a base and the anion from an acid

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Any time a strong acid reacts with a strong bas the net ionic equation is...

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OH^- ^ +H^+^ --> H_2_O

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Monoprotic

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one proton
can donate 1 proton per acid molecule
HCl
HNO_3_

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Polyprotic

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multiple proton donation
H_2_SO_4_
H_3_PO_4_

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Polyprotic acids

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2 or more acidic hydrogens per molecule

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Quantitive analysis

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determination of the substance amount or concentration of a substance in a sample

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Volumetric analysis

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Titration
-involves volume measurement
-type of reaction utilized
-neutralization
-redox
-complex ion formation

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Gravimetric analysis

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a type of quantative analysis in whihc the amount of a species in a material is determined by converting the species to a product that can be isolated completely and weighted.
involves mass measurement
-type of reaction utilized
-precipitation

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Titration

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method used to determine the concentration of a substance dissolved in a solution

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Equivalence point

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the point of a titration where reaction is just complete; just enough known has been added to completely react with all of the unknown present

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End point

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point where the titration experiment is stopped based on observation

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Oxidation

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gain of oxygen
loss of hydrogen
loss of electrons
Increase in oxidation number

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Reduction

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loss of oxygen
gain of hydrogen
gain of electrons
reduction of oxidation number

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Redox

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have to occur simultaneously

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Oxidation agent

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electron acceptor
species that oxidizes something else
the oxidizing agent is reduced

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Reducing agent

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Electron donar
species that reduces something else
The reducing agent is oxidized