Acids And Bases

Acids and Bases

Term	Definition
Solute	What gets dissolved in a solution
Solvent	The predominant component of a solution; other things get dissolved in it
Hydration Number	The number of water molecules associated with a particular ion
Strong Electrolyte	Their solutions conduct electricity well
Weak Electrolyte	Their solutions conduct electricity poorly
Nonelectrolyte	Their solutions conduct no electricity
Strong Electrolyte	Dissociates completely in aqueous solution
Strong Electrolyte	Soluble salts, strong acids, and strong bases
Weak Electrolyte	Partially dissociates in aqueous solution
Weak Electrolyte	Weak acids, weak bases
Arrhenius Acid	Proton (H+) Producer
Arrhenius Base	OH- Producer
Bronsted-Lowry Acid	Proton (H+) Donor
Bronsted-Lowry Base	Proton (H+) Acceptor
Lewis Acid	electron pair acceptor
Lewis Base	electron pair donor
Amphoteric	Can act as acid or base
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Term	Definition
Complete Ionic Equation	All strong electrolytes are represented as ions
Net Ionic Equation	Only lists solution components that react
Spectator Ions	Not included in Net Ionic Equations
Stoichiometric Point = Equivalence Point	The point in a titration when enough titrant has been added to react exactly with the substance being determined
Indicator	A chemical that changes color at the equivalence point of a titration
Buffer Solution	Contains weak acid or weak base
Buffer Solution	Resists pH changes when OH- or H+ are added
Strong Acids	HCl, HBr, HI, HNO3, HClO4, H2SO4
Strong Bases	NaOH, KOH, Ca(OH)2
Weak Monoprotic Acids	HSO4-, HClO2, HC2H2ClO2, HF, HNO2, HC2H3O2, [Al(H2O)6]3+, HOCl, HCN, NH4+, HOC6H5
Weak Polyprotic Acids	H3PO4, H3AsO4, H2CO3, H2SO3, H2S, H2C2O4, H2C6H6O6
Weak Bases	NH3, CH3NH2, C2H5NH2, C6H5NH2, C5H5N
Conjugate Acid	What results when a base gains a proton
Conjugate Base	What remains of an acid after H+ is lost
Conjugate Acid	BH+ for the base B
Conjugate Base	A- for the acid HA
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Term	Definition
Oxidation/Reduction	Electron Transfer
Redox Reaction	Electron Transfer
Oxidation	An increase in oxidation state or number
Oxidation	A loss of electrons
Reduction	A decrease in oxidation state or number
Reduction	A gain of electrons
Oxidizing Agent	It gets reduced
Oxidizing Agent	Electron acceptor
Reducing Agent	Electron donor
Reducing Agent	It gets oxidized
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Term	Definition
pH	-log[H+]=-log[H3O+]
pOH	-log[OH-]
pH	14-pOH
pOH	14-pH
[H+]=[H3O+]	10-pH=1014-pOH
[OH-]	10-pOH=1014-pH
Kw	10-14=[H+][OH-]=[H3O+][OH-]=Ka x Kb
Ka	[H3O+][A-]/[HA] = [H+][A-]/[HA]
Ka	Large for strong acids, small for weak acids
Ka	Kw/Kb=10-14/Kb
Kb	[BH+][OH-]/[B]
Kb	Large for strong bases, small for weak bases
Kb	Kw/Ka=10-14/Ka
pKa	-log[Ka]
pKb	-log[Kb]
Henderson-Hasselbalch Equation	pH=pKa+log([A-]/[HA])=pKa+log([base]/[acid])
Henderson-Hasselbalch Equation	pOH=pKb+log([BH+]/[B])=pKb+log([acid]/[base])
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Term	Definition
pH of aqueous solution of KCl, NaCl, NaNO3, or KNO3 salt	7 (neutral)
pH of aqueous solutions of salts with cations of strong bases and anions of strong acids	7 (neutral)
pH of aqueous solutions of salts with cations of strong bases and anions of weak acids	>7 (basic)
pH of aqueous solution of NaC2H3O2, NaF, or KCN salt	>7 (basic)
pH of aqueous solutions of salts with cations of weak bases and anions of strong acids	<7 (acidic)
pH of aqueous solutions of salts with anions of strong acids and cations of highly charged metal ions that form hydrated ion complexes with H2O	<7 (acidic)
pH of aqueous solutions of salts with cations of weak bases and anions of weak acids	Ka > Kb gives acidic (<7), Ka = Kb gives neutral (=7), Ka < Kb gives basic (>7)
pH of aqueous solution of NH4Cl, NH4NO3, FeCl3, Al(NO3)3, or AlCl3	<7 (acidic)
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Acid Names

Anions ending in -ate generally give acids ending in -ic.

Mnemonic: "I ate the icky one".

Acid Name	Chemical Formula
Nitric Acid	HNO3
Nitrous Acid	HNO2
Sulfuric Acid	H2SO4
Sulfurous Acid	H2SO3
Hydrosulfuric Acid	H2S
Perchloric Acid	HClO4
Chloric Acid	HClO3
Chlorous Acid	HClO2
Hypochlorous Acid	HClO
Hydrochloric Acid	HCl
Acetic Acid	HC2H3O2
Hydrocyanic Acid	HCN
Phosphoric Acid	H3PO4
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Solubilities of Salts in Water (p.114)

Salt	Is it soluble in water?
Most nitrate (NO3-) salts	yes
Most salts of Na+, K+, NH4+	yes
Most chloride (Cl-) salts	yes
AgCl, PbCl2, Hg2Cl2	no
Most sulfate (SO42-) salts	yes
BaSO4, PbSO4, CaSO4	no
Most hydroxide (OH-) salts	slightly
NaOH, KOH, Ca(OH)2	yes
Most sulfide (S2-) salts	slightly
Most carbonate (CO32-) salts	slightly
Most phosphate (PO43-) salts	slightly
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Reference: "Chemistry" by Steven S. Zumdahl, D.C. Heath and Company, 1986
(ISBN=0-669-04529-2).