Chemistry III – Flashcards
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| Dynamic equilibrium |
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| rates of the forward and reverse reaction rates are equal |
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| larger the k value the ________ product at equilibrium |
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| more product |
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| concentration of reactions at equilibrium |
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| not equal |
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| Keq >> 1 |
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| equilibrium favors products |
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| Keq << 1 |
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| equilibrium favors reactants |
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| K backward = |
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| 1/ K forward |
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| Q > K |
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| fastest in the reverse direction,the [products] will decrease and [reactants] will increase |
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| Q < K |
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| fastest in forward direction, the [products] will increase and [reactants] will decrease |
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| Q = K |
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| reaction is at equilibrium |
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| Properties of acids |
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| sour reacts with active metals corrosive litmus blue turns to red reacts with carbonates |
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| Binary acids |
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| acid hydrogens attached to a nonmetal atom |
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| Oxy acids |
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| acid hydrogens attached to an oxygen atom |
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| Carboxylic acids |
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| have COOH group |
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| Properties of Bases |
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| bitter red litmus turns blue known as alkalis Solutions feel slippery |
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| Indicators |
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| change color depending on acidity or basicity,litmus, Phenolphthalein |
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| Arrhenius Base |
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| dissociate in water to produce OH? ions and cations |
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| Arrhenius Acid |
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| ionize in water to produce H+ ions and anions |
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| Arrhenius Acid–Base Reactions |
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| acid + base > salt + water |
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| Bronsted-Lowry Acid |
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| acid is an H donor |
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| Bronsted-Lowry Base |
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| base is an H acceptor |
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| Amphoteric |
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| can act as an acid or a base (water) |
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| Conjugate acid has one ________ proton |
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| has one more proton (hydrogen) |
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| strong acid or base is a ________ electrolyte |
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| strong, and vise versa |
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| larger Ka = ________ acid |
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| stronger |
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| pH formula |
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| pH = -log[H3O+], to get [H3O+] 10^-(pH) |
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| autoionization |
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| atoms and molecules spontaneously emit a valence electrons |
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| Dissociation Constant of Water |
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| Ion Product of Water: [H3O+] x [OH–] = Kw = 1.00 x 10^?14 @ 25 °C |
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| pOH formula |
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| pOH = ?log[OH?], [OH?] = 10^?pOH |
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| pH+ pOH = |
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| 14.00 |
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| strength of an acid or base formula |
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| pKa = -log(Ka), Ka = 10^-pKa pKb = -log(Kb), Kb = 10^-pKb |
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| stronger the acid the _________ pKa |
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| smaller |
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| larger Ka = ________ pKa |
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| smaller |
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| polyprotic acids |
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| more than one ionizable H-, stronger than monoprotic acids |
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| Percent Ionization = |
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| (molarity of ionized acid / initial molarity) * 100 |
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| Salts |
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| water-soluble can be acidic or basic |
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| anion |
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| conjugate base of an acid |
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| stronger the acid, the _________ the conjugate base |
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| weaker the conjugate base |
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| higher electronegativity = _________ acidity |
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| higher acidity, increases right and down periodic table |
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| Lewis Acid Base theory |
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| focuses on transferring an electron pair |
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| Lewis Base |
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| electron donor electron rich, therefore nucleophile |
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| Lewis Acid |
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| electron acceptor electron deficient, therefore electrophile |
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| acid rain |
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| pH less than 5.6, corrodes carbonate (bridges, cement, marble, limestone) |
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| danger of antifreeze |
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| contains ethylene glycol which is turned into glycolic acid by liver, lowers blood pH causes acidosis |
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| buffers |
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| resist changes in pH when an acid or base is added |
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| Making an Acid Buffer |
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| weak acid mixed with solution of soluble salt containing conjugate base anion |
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| common ion |
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| conjugate base of the acid |
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| Relationship between pKa and pKb |
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| ?log(Ka) + ?log(Kb) = 14 pKa + pKb = 14 |
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| Henderson-Hasselbalch Equation |
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| pH=pKa+log(A-/HA) |
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| buffering capacity |
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| amount of acid or base a buffer can neutralize |
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| buffering range |
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| pH range the buffer can be effective |
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| effectiveness of a buffer depends on |
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| 1. relative amounts of acid and base 2. absolute concentrations of acid and base |
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| buffers will work when |
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| 0.1 < [base]:[acid] < 10 |
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| buffers most effective when there are |
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| equal concentrations of acid and base |
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| titration |
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| a solution of unknown concentration (titrant) is slowly added to a solution of known concentration |
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| the equivalence point |
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| inflection point of the curve |
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| solubility product, Ksp |
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| constant of dissociation of a solid salt into its aqueous ions |
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| molar solubility |
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| number of moles of solute that will dissolve in a liter of solution |
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| complex ions |
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| Ions that form by combining a cation with several anions or neutral molecules |
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| ligands: the (H2O) in Ag(H2O)2 |
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| attached ions or molecules of complex ions |
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| conjugate base has one _______ hydrogen |
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| has one less proton (hydrogen) |
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| Ka x Kb = |
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| kw = 1*10^-14 |
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| What is the difference between a strong and weak acid |
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| strong acid completely ionizes where a weak one partially ionizes |
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| what is the autoionization of water? |
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| water acts as an acid and a base with itself |
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| Do both protons ionize instantaneously from a diprotic acid such as H2CO3 |
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| No polyprotic acids ionize in successive steps, the lst proton easily separates from the nuetral atom while the next protons have difficulty in separating from the anions |
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| Describe the relationship between molecular structure and acid strength |
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| The stronger the bonds the weaker the acid, the greater the electronegativity & polarity the stronger the acid |
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| compound that is in antifreeze and is toxic to pets |
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| ethylene glycol |
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| Sketch the titration curve for a strong acid titrated with a strong bas |
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| [image] |
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| Identify the compound that is in stalactites and stalagmites |
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| Calcium carbonate |
