Vocab – Chemistry – Flashcards
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| solution |
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| a homogeneous mixture of two or more pure substances |
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| nonsolutions |
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| suspension, colloidal dispersion |
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| solvation |
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| process of solution formation |
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| hydration |
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| process of solution formation when water is the solvent |
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| spontaneous |
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| reaction will occur on its own |
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| entropy |
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| amount of randomness or disorder in a system |
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| solubility |
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| amount of a solute that will dissolve in a given amount of solution |
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| unsaturated solution |
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| contains less than the maximum amount of solute |
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| saturated solution |
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| contains the maximum amount of solute |
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| supersaturated solution |
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| contains more than the maximum amount of solute |
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| solute-solute interaction |
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| substances with similar intermollecular forces form solutions |
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| immiscible |
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| two liquids that do not dissolve |
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| miscible |
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| two liquids that do form a solution |
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| concentration |
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| relative amount of solute to amount of solution or solvent |
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| colligative properties |
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| properties of solutions that depend only on the amount of solute present |
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| vapor pressure |
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| pressure exerted by the vapor phase of a volitile liquid that is in equillibrium with the liquid phase |
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| boiling point |
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| temperature where vapor pressure of a liquid equals the external pressure |
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| boiling point elevation |
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| presence of a non-volatile liquid solute increases the boiling point of a liquid |
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| freezing point depression |
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| presence of a solute decreases the freezing point of a liquid due to entropy |
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| osmosis |
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| movement of solvent molecules through a semi-permeable membrane in response to a difference in solute concentration |
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| reaction rate |
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| change in amount (reaction or product) over time |
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| instantaneous reaction rates |
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| rate at a specific time- slope of a line tangent to the concentration/time curve |
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| integrated rate laws |
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| relate concentration and time |
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| first order reaction |
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| rate=K[A] |
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| half life |
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| amount of time required to reach 1/2 original reactant amount |
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| second order reaction |
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| rate=K[A]^2 |
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| collision theory |
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| to react, reactants must encounter each other |
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| activation energy |
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| energy barrier between reactants and products (E required for a successful collision) |
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| transition state |
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| short lived intermediate between reactants and products |
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| molecularity |
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| classifying of elementary steps based on the number of reactants in the collision |
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| rate determining step |
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| slowest step in reaction mechanism |
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| fast initial step |
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| rate limiting step contains an intermediate as a reactant |
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| catalysis |
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| lowers Ea (increases a) |
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| homogeneous catalysis |
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| catalyst is in same phase as reactants |
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| heterogeneous catalysis |
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| catalyst and reactants are in different phases |
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| surface catalyzed |
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| when a solid catalyst binds with liquid or gas reactants |
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| adsorption |
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| binding to a surface |
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| migration |
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| adsorbed reactants move to encounter each other |
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| desorption |
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| product releases from surface |
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| hydrogenation |
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| addition of H2 to an unsaturated hydrocarbon |
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| enzymes |
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| biological catalysts |
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| proteins |
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| strings of amino acids |
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| amino acid |
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| composed of an amine group, acid group and organic group |
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| primary protein structure |
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| amino acid sequence |
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| secondary and tertiary protein structure |
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| describe 3d shape of protein; maintained by interactions between amino acids |
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| dynamic equilibrium |
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| forward and reverse reaction continue to occur at the same rate |
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| K>>1 |
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| products are favored |
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| K<<1 |
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| reactants are favored |
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| heterogeneous equilibrium |
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| reactants and products are in multiple phases |
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| Le Chatelier's Principle |
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| when a system at equilibrium is disturbed, the relative concentrations of reactants and products shift to reestablish equilibrium |
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| Arrhenius theory of an acid |
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| a substance that increases H+ in water |
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| Arrhenius theory of a base |
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| a substance that increases OH- in water |
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| Bronsted-Lowry theory of an acid |
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| proton donor |
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| Bronsted-Lowry theory of a base |
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| proton acceptor |
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| conjugate acid |
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| has one more proton that the base from which it formed |
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| conjugate base |
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| a substance with one less proton than the acid from which it formed |
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| strong acid |
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| donates all available protons |
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| strong base |
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| accepts all available protons |
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| weak acid |
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| donates some available protons |
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| weak base |
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| accepts some available protons |
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| amphoteric |
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| can act as an acid or a base |
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| amphiprotic |
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| can accept and donate protons |
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| neutral solution |
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| pH=7.0 @ 25 degrees C |
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| acidic solution |
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| [H+]>10^-7 and [H+]>[OH-] |
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| basic solution |
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| [OH-]>10^-7 and [OH-]>[H+] |
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| polyprotic acid |
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| multiple acidic protons per acid molecule |
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| salt |
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| ionic compound- composed of cation and anion |
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| anion hydrolysis |
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| anion reacts with H+ of H2O forming a basic solution |
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| Cation hydrolysis |
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| react with OH- through hydrolysis creating an acidic solution |
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| Lewis Acid-Base Theory Acid |
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| electron pair acceptor |
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| Lewis Acid-Base Theory Base |
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| donates electron pair |
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| buffer capacity |
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| amount of acid or base the buffer can neutralize before the pH begins to change to an appreciable degree |
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| pH range of buffer |
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| range over which the buffer acts effectively |
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| Ksp |
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| how soluble a solid is in water |
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| solubility |
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| quantity of substance that dissolves to form a saturated solution |
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| common ion effect |
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| whenever a weak electrolyte and a strong electrolyte contain a common ion, the weak electrolyte ionizes less than it would if it were alone in the solution |
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| buffer |
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| a solution that resists change to pH even upon the addition of an acid or a base |
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| titrant |
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| substance with a known concentration that reacts with the analyte |
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| Ve (equivalence point) |
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| # mols titrant added is stoichiometrically equivalent to the # mols of analyte |
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| dynamic equilibrium |
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| dissolution and precipitation both occur at the same rate |
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| aqueous solubility |
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| solubility with H2O as solvent |
