Chemical Equations in Aqueous Solutions

Hydrochloric acid

strong acid

HCL (aq) --> H+ (aq) + Cl- (aq)

Hydrobromic acid

strong acid

HBr (aq) --> H+ (aq) + Br- (aq)

Hydroiodic acid

strong acid

HI (aq) --> H+ (aq) + I- (aq)

Nitric acid

strong acid

HNO3 (aq) --> H+ (aq) + NO3- (aq)

Chloric acid

strong acid

HClO3 (aq) --> H+ (aq) + ClO3- (aq)

Perchloric acid

strong acid

HClO4 (aq) --> H+ (aq) + ClO4- (aq)

Sulfuric acid

strong acid

H2SO4 (aq) --> H+ (aq) + HSO4- (aq)

HSO4- (aq) --> H+ (aq) + SO42- (aq)

only first ionization is complete

Lithium hydroxide

strong base

group IA

LiOH

Sodium hydroxide

strong base

group IA

NaOH

Potassium hydroxide

strong base

group IA

KOH

Rubidium hydroxide

strong base

group IA

RbOH

Cesium hydroxide

strong base

group IA

CsOH

Calcium hydroxide

strong base

group IIA

Ca(OH)2

Strontium hydroxide

strong base

group IIA

Sr(OH)2

Barium hydroxide

strong base

Water-Soluble Compounds

compounds containing an alkali metal cation (Li+, Na+, K+, Rb+, Cs+) or the ammonium ion (NH4+)

Water-Soluble Compounds

compounds containing the nitrate ion (NO3-), acetate ion (C2H3O2-), chlorate ion (ClO3-), or perchlorate ion (ClO4-)

Water-Soluble Compounds

compounds containing the chloride ion (Cl-), bromide ion (Br-), or iodide ion (I-)

Water-Soluble Compounds

compounds containing the sulfate ion (SO42-)

Insoluble Exceptions

compounds containing Ag+, Hg22+, or Pb2+

Insoluble Exceptions

compounds containing Ag+, Hg22+, Pb2+, Ca2+, Sr2+, or Ba2+

Water-Insoluble Compounds

compounds containing the carbonate ion (CO32-), phosphate ion (PO43-), chromate ion (CrO42-), sulfide ion (S2-), or sulfite ion (SO32-)

Water-Insoluble Compounds

compounds containing the hydroxide ion (OH-) or oxide ion (O2-)

Soluble Exceptions

compounds containing Li+, Na+, K+, Rb+, Cs+, or NH4+

Soluble Exceptions

compounds containing Li+, Na+, K+, Rb+, Cs+, Ba2+, Ca2+, or Sr2+

Solution

a homogenous mixture

Solute

the component that is dissolved in solvent; usually in smaller amounts

Solvent

medium into which solutes are mixed; usually in greater amount

Concentration

describes solution composition

Dilute

ratio of solute to solvent is very small

Concentrated

ratio of solute to solvent is very large; syrup = sugar/H2O

Saturated

contains as much solute as can be dissolved

Unsaturated

can dissolve more solute

Supersaturated

contains more solute than a saturated solution at a given temperature

formed by cooling saturated solution from higher temperature (solutes typically more soluble at higher temp.)

any slight disturbance (tap, dust, etc.) and solute comes out quickly as solide

Precipitate (ppt)

solid that comes out of solution

Electrolyte

substance that dissolves in H2O giving a solution that conducts electricity

form ions in solutions; ionic compounds (electrolytes) dissociate into constituent ions

Nonelectrolyte

substance who aqueous solution does not conduct electricity

no charged particles in the solution, and thus solution cannot conduct electricity

Ionization

formation of ions by molecular substance when dissolving

some molecular compounds ionize when dissolving in water (therefore electrolytes)

Strong electrolytes

dissociate/ionize completely (100%)

strong conductors of electricity

all water soluble ionic compounds

all strong acids

all strong bases

Acids

produce protons (H+) in aqueous solution

tart/sour taste

corrode metals

typically dangerous 

examples; vinegar, lemon juice

Bases

produce OH- in aqueous solutions

bitter taste

soapy feeling (change oils/fats in skin to soap)

Weak electrolytes

DO NOT dissociate/ionize completely (<100%)

weak conductors of electricity (mainly unionized)

weak acids

weal bases

slightly soluble ionic compounds