Term
| Arrhenius defition of acids and bases |
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Definition
| Arrhenius acid will dissociate to form an excess of H+ in solution, Arrhenius base will dissociate to form an excess of OH- in solution |
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Term
| Brønsted-Lowry definition of acids and bases |
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Definition
| acid is a species that donates hydrogen ions while a base is a species that accepts them |
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Term
| Lewis definition of acids and bases |
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Definition
Lewis acid is an electron pair acceptor
Lewis base is an electron pair donor |
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Term
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Definition
| describes a species that reacts like an acid in a basic environment and like a base in an acidic environment |
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Term
| acid-base nomenclature of oxyanions |
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Definition
| oxyanions - if the anion ends in -ite, acid will end with -ous acid; if anion ends in -ate, acid will end with -ic acid |
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Term
| how to determine pH and pOH |
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Definition
pH = -log[H+] = log(1/[H+])
pOH = -log[OH-] = log(1/[OH-]) |
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Term
| approximation for -log(n x 10-m) |
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Definition
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Term
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Definition
completely dissociate in solution
strong acids: HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), H2SO4 (sulfuric acid), HNO3 (nitric acid), HClO4 (perchloric acid)
strong bases: NaOH (sodium hydroxide), KOH (potassium hydroxide), other soluble hydroxides |
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Term
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Definition
do not completely dissociate, dissociation equation can be written as
Ka = ([H3O+][A-])/[HA], for acids
Ka is the acid dissociation constant
Kb = ([B+][OH-])/[BOH], for bases
Kb is the base dissociation constant
smaller constants means weaker acids |
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Term
| What is the relationship between Ka and Kb? |
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Definition
| The Ka of an acid times the Kb of its conjugate base will equal Kw, 10-14. The same goes for Kb. This means that a strong acid will have a weak conjugate base and a strong base will have a weak conjugate acid |
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Term
| Calculate the concentration of H3O+ in a 2.0 M aqeuous solution of acetic acid, CH3COOH. (Note: Ka = 1.8 x 10-5) |
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Definition
Ka = ([H3O+][CH3COO-]/[CH3COOH] = 1.8 x 10-5
Ka = [x][x]/[2.0M - x] = 1.8 x 10-5
Ka = [x][x]/[2.0M] = 1.8 x 10-5
x2 = 3.6 x 10-5
x = 6 x 10-3 |
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Term
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Definition
when acids and bases react together to form a salt and often, but not always, water
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Term
| strong acid reacts with weak base |
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Definition
| salt is produced, slightly acidic pH |
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Term
| strong base reacts with weak acid |
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Definition
| salt is formed, slightly basic pH |
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Term
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Definition
| the reverse reaction of a neutralization, the salt ions react with water to give back the acid or base |
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Term
| strong acid and strong base titration |
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Definition
| equivalence point will be at pH 7 |
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Term
| titration of weak acid with strong base |
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Definition
| equivalence point will be basic, curve of graph will be more gardual to the equivalence point |
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Term
| titration of weak base with strong acid |
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Definition
| equivalence point will be acidic, slopes more gradually to equivalence point on graph compared to strong acid and strong base |
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Term
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Definition
| the midpoint of the buffering region when half of the titrant has been protonated or deprotonated |
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Term
| bicarbonate buffer system |
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Definition
CO2 (g) + H2O (l) ↔ H2CO3 (aq) ↔ H+ (aq) + HCO3- (aq)
if blood becomes too acidic breathing increases removing CO2 from the body and pushing the equilbrium to the left and neutralizing the hydronium ions to increase blood pH. if blood is too basic breathing slows to increase CO2 and increase the hydronium concentration to lower blood pH |
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Term
| Henderson-Hasselbalch equation |
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Definition
used to estimate the pH or pOH of a buffer solution
for a weak acid buffer solution
pH = pKa + log([A-]/[HA])
for a weak base buffer solution
pOH = pKb + log([B+]/[BOH])
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