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41 Cards in this Set
- Front
- Back
Solvent
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present in greatest amount
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Solute
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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 |