ChemExam 3
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| Homogenous Equilibrium | When the products and reactants of an equilibrium reaction form a single phase, whether gas or liquid
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| Heterogenous Equilibrium | A system whose reactants, products, or both are in more than one phase
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| Le Châtelier’s Principle | This principle states that if a stress is applied to a system at equilibrium, the composition of the system will change to relieve the applied stress.
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| Buffer | A solution that resists a change in pH when hydroxide or hydronium ions are added.
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| Common Ion Effect | The limiting of acid (or base) ionization caused by addition of its conjugate base (or conjugate acid)
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| Titrant | The substance being added during a titration
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| Equivalence Point | The point in a titration at which one reactant has been exactly consumed by addition of the other reactant, must be determined mathematically
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| Primary Standard | A pure, solid acid or base that can be accurately weighed for preparation of a titrating reagent; has to be cheap to buy, stable on shell, non-hydroscopic, chemistry to be predictable, and high mass
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| End Point | The physical change which results when the equivalence point has been reached. In colorimetric titrations, this is a color change of the indicator.
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| Secondary Standard | A solution that has been titrated against a primary standard. A standard solution is a secondary standard. (NaOH)
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| Titration | A procedure for quantitative analysis of a substance by an essentially complete reaction in solution with a measure quantity of a reagent of known concentration
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| Solubility | The concentration of solute in equilibrium with undissolved solute in a saturated solution
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| Molar Solubility | Number of moles of a solute that dissolve to produce a liter of saturated solution
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| Ksp-Solubility Product Constant | An equilibrium constant relating the concentrations of the ionization products of a dissolved substance
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| Ka–Acid Dissociation Constant | The equilibrium constant for the ionization of an acid in aqueous solution
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| Kb–Base Dissociation Constant | The equilibrium constant for the ionization of a base in aqueous solution
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| Lewis Acid | A substance that is an electron-pair acceptor
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| Lewis Base | A substance that is an electron-pair donor
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| Bronsted-Lowry Acid | Any substance that can donate a proton
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| Bronsted-Lowry Base | Any substance that can accept proton
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| Arrenhius Acid | A substance that dissociates in water to produce H+ ions (protons)
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| Arrhenius Base | A substance that dissociates in water to produce OH- ions (hydroxide)
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| Henderson-Hasselbach Equation | An approximate equation that shows the relationship between the pH/pOH of a solution and the pKa/pKb and the ratio of the concentrations of the dissociated chemical species
pH=pKa+log(salt)-log(base) or pOH=pKb+log(salt)-log(base)
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| Conjugate Acid | Contains one more proton than its base
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| Conjugate Base | Contains one less proton than its acid
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| Reversible Reaction | Reaction can occur in either direction, they do not go to completion
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| Equilibrium | It's a microscopic event, regardless of the direction of approach the forward rate and the reverse rate rate are the same and changes in concentration cannot be observed.
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| Equilibrium Equation | The ratio of the product of the equilibrium concentrations of the products(raised to their coefficients in the balanced equation) to the product of the equilibrium concentrations of the reactants (raised to their coefficients in the balanced equation)
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| Reaction Quotient | The product of concentrations of products divided by the product of concentrations of reactants, each raised to the power of its stoichiometric coefficient in the chemical equation
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| Exothermic | Heat is lost by the system, and is added to the product side
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| Endothermic | Heat is gained by the system, and is added to the reactant side
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| Catalyst | Decreases the activation energy of both the forward and reverse reaction equally; equilibrium will be established faster
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| Autoionization | Interaction of two water molecules to produce a hydronium ion and hydroxide ion by proton transfer
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| pH | The negative of the base-10 logarithm of the hydrogen ion concentration; a measure of acidity
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| pOH | the negative of the base- 10 logarithm of the hydroxide ion concentration; a measure of basicity
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| pKa | The negative of the base- 10 logarithm of the acid ionization constant
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| pKb | The negative of the base- 10 logarithm of the base ionization constant
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| Amphiprotic | A substance that can act as an acid by donating a proton to a base to form the hydroxide ion or as a base by accepting a proton from an acid to form the hydronium ion
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| Amphoteric | Substances that can behave as both an acid and a base
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| Analytical Concentration | the total concentration of all forms of an acid or base that are present in solution, regardless of their stat of protonation
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| Buffer Capacity | The number of moles of strong acid and strong base needed to change the pH of 1 Liter of buffer solution by 1 pH unit
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