Term
|
Definition
rates of
the forward and reverse reaction rates are equal |
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|
Term
| larger the k value the ________ product at equilibrium |
|
Definition
|
|
Term
| concentration of reactions at equilibrium |
|
Definition
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|
Term
|
Definition
| equilibrium favors products |
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Term
|
Definition
| equilibrium favors reactants |
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Term
|
Definition
|
|
Term
|
Definition
| fastest in the reverse direction,the [products] will decrease and [reactants] will increase |
|
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Term
|
Definition
| fastest in forward direction, the [products] will increase and [reactants] will decrease |
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Term
|
Definition
| reaction is at equilibrium |
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|
Term
|
Definition
sour
reacts with active metals
corrosive
litmus blue turns to red
reacts with carbonates |
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|
Term
|
Definition
acid hydrogens attached
to a nonmetal atom |
|
|
Term
|
Definition
acid hydrogens attached to
an oxygen atom |
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|
Term
|
Definition
|
|
Term
|
Definition
bitter
red litmus turns blue
known as alkalis
Solutions feel slippery |
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Term
|
Definition
| change color depending on acidity or basicity,litmus, Phenolphthalein |
|
|
Term
|
Definition
dissociate in water to produce OH− ions
and cations |
|
|
Term
|
Definition
ionize in water to produce H+ ions and
anions |
|
|
Term
| Arrhenius Acid–Base Reactions |
|
Definition
| acid + base → salt + water |
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Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| can act as an acid or a base (water) |
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|
Term
| Conjugate acid has one ________ proton |
|
Definition
| has one more proton (hydrogen) |
|
|
Term
| strong acid or base is a ________ electrolyte |
|
Definition
|
|
Term
| larger Ka = ________ acid |
|
Definition
|
|
Term
|
Definition
| pH = -log[H3O+], to get [H3O+] 10^-(pH) |
|
|
Term
|
Definition
| atoms and molecules spontaneously emit a valence electrons |
|
|
Term
| Dissociation Constant of Water |
|
Definition
| Ion Product of Water: [H3O+] x [OH–] = Kw = 1.00 x 10^−14 @ 25 °C |
|
|
Term
|
Definition
| pOH = −log[OH−], [OH−] = 10^−pOH |
|
|
Term
|
Definition
|
|
Term
strength of an acid or
base formula |
|
Definition
pKa = -log(Ka), Ka = 10^-pKa
pKb = -log(Kb), Kb = 10^-pKb |
|
|
Term
| stronger the acid the _________ pKa |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| more than one ionizable H-, stronger than monoprotic acids |
|
|
Term
|
Definition
| (molarity of ionized acid / initial molarity) * 100 |
|
|
Term
|
Definition
water-soluble
can be acidic or basic |
|
|
Term
|
Definition
|
|
Term
| stronger the acid, the _________ the conjugate base |
|
Definition
|
|
Term
| higher electronegativity = _________ acidity |
|
Definition
| higher acidity, increases right and down periodic table |
|
|
Term
|
Definition
focuses on transferring
an electron pair |
|
|
Term
|
Definition
electron donor
electron rich, therefore nucleophile |
|
|
Term
|
Definition
electron acceptor
electron deficient, therefore electrophile |
|
|
Term
|
Definition
| pH less than 5.6, corrodes carbonate (bridges, cement, marble, limestone) |
|
|
Term
|
Definition
| contains ethylene glycol which is turned into glycolic acid by liver, lowers blood pH causes acidosis |
|
|
Term
|
Definition
| resist changes in pH when an acid or base is added |
|
|
Term
|
Definition
| weak acid mixed with solution of soluble salt containing conjugate base anion |
|
|
Term
|
Definition
| conjugate base of the acid |
|
|
Term
| Relationship between pKa and pKb |
|
Definition
−log(Ka) + −log(Kb) = 14
pKa + pKb = 14 |
|
|
Term
| Henderson-Hasselbalch Equation |
|
Definition
|
|
Term
|
Definition
amount of acid or
base a buffer can neutralize |
|
|
Term
|
Definition
pH range the buffer can
be effective |
|
|
Term
| effectiveness of a buffer depends on |
|
Definition
1. relative amounts of acid and base
2. absolute concentrations of acid and base |
|
|
Term
|
Definition
|
|
Term
| buffers most effective when there are |
|
Definition
| equal concentrations of acid and base |
|
|
Term
|
Definition
a solution of unknown concentration
(titrant) is slowly added to a solution of known concentration |
|
|
Term
|
Definition
| inflection point of the curve |
|
|
Term
|
Definition
constant of dissociation of a
solid salt into its aqueous ions |
|
|
Term
|
Definition
number of moles of
solute that will dissolve in a liter of solution |
|
|
Term
|
Definition
| Ions that form by combining a cation with several anions or neutral molecules |
|
|
Term
| ligands: the (H2O) in Ag(H2O)2 |
|
Definition
| attached ions or molecules of complex ions |
|
|
Term
| conjugate base has one _______ hydrogen |
|
Definition
| has one less proton (hydrogen) |
|
|
Term
|
Definition
|
|
Term
| What is the difference between a strong and weak acid |
|
Definition
| strong acid completely ionizes where a weak one partially ionizes |
|
|
Term
| what is the autoionization of water? |
|
Definition
| water acts as an acid and a base with itself |
|
|
Term
| Do both protons ionize instantaneously from a diprotic acid such as H2CO3 |
|
Definition
| 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 |
|
|
Term
| Describe the relationship between molecular structure and acid strength |
|
Definition
| The stronger the bonds the weaker the acid, the greater the electronegativity & polarity the stronger the acid |
|
|
Term
| compound that is in antifreeze and is toxic to pets |
|
Definition
|
|
Term
| Sketch the titration curve for a strong acid titrated with a strong bas |
|
Definition
|
|
Term
| Identify the compound that is in stalactites and stalagmites |
|
Definition
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