A very basic inorganic Chemistry

Units of MeasurementQuantity SI Units Conversion Factor USCS Units... of volumesolute of mass ppm kg mg example solution of mass solute of example solution of volume solute of volume 3 m

BASIC CHEMISTRY

Units of Measurement

Quantity SI Units Conversion Factor USCS Units

Group 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 Period

of volume

solute of

mass

ppm kg

mg example solution

of mass

solute of

example solution

of volume

solute of

volume

3

m

mg example solution

of volume

solute of

mass

The relation between ppm and mg/l for gaseous solutions depends on pressure, temperature and

molecular weight

The ideal gas Law: P V=n R T

Temperature (K=273+ o C)

Gas constant 0.082 (L.atm/K.mol) (see

Appendix C)

Number of moles Volume

Pressure

atm

atm

P K

T

K weight

molecular

ppm m

mg

1

)

( )

(

15

273 414

22

25 273

(

15

273 414

22

K m

mg

Other Concentration Units

volume of solution (L)

weight Molecular

solute of

mass solute

of

Normality = equivalentmass of solute/Lweight

Equivalent weight = equivalent numberMW

Kinetics

a

]A[

kdt

]A

[

Reactions take time to reach equilibrium This time could

be very short or very long

xA yC + zD

A Time

D

C

The rate of change of A with

respect to time, if the reaction is

irreversible, takes the form:

Constant determined experimentally.

Reaction rate constant

Many reactions rates in the

environment are modeled

as first-order (i.e a=1):

kt

o ] e A [ ] A

a

]A[

kdt

]A[

Consider the following balanced chemical reaction

a X+ b Y c Z

; [ ]= molar concentration

If the chemical is in the solid state or pure liquid then its [ ]=1

pressure (P)

b a

c

Y X

Z K

][][

][



Note: K for the above reaction is written as

In-Class Exercise (Example 2.2 modified)

2 M of C6H12O6 are completely oxidized to CO2 and H2O Find the amount of oxygen required to complete the reaction.

] [

] [

] [

] [

] [

) ( 6 12 6

6 2

6 2 )

( 6 12 6

6 ) ( 2

6 ) ( 2

6 ) ( 2

aq O

CO aq

g

g

l

O H C P

P O

H C O

CO O

H

O2 = 6x2= 12 M = (12 M)(32 g/mol) = 384 g/L

 Acid-base rxns

H2O H+ + OH

-C at

OH H

O H

OH H

l

aq aq

] [

] ][

) ( 2

) ( )

/ (

033 0

] [

2

) ( 2

atm L

mol P

CO K

In-Class Exercise (Example 2.9)

Find the solubility of fluoride ions in water caused by the dissolution of CaF 2

Organic compounds contain carbon except compounds such as CO,

CO 2 , CO 3 .

Hydrocarbons: Organic compounds that contain H and C

Alkanes (single bond): Methane (CH 4 ), Ethane (C 2 H 6 ) , Propane (C 3 H 8 ), Butane (C 4 H 10 ), Pentane (C 5 H 12 ), Hexane (C 6 H 14 ), Heptane (C 7 H 16 ),

Octane (C 8 H 18 ), Nonane (C 9 H 20 ), Decane, (C 10 H 22 ) etc.

Alkenes (double bond): Ethene (C 2 H 4 ), Propene (C 3 H 6 ), etc.

Alkynes (triple bond): Ethyne (C 2 H 2 ), Propyne (C 3 H 4 ), etc.

Organic compounds

Saturated (Paraffins) Unsaturated (Olefins)

Organic Chemistry

CH 3 C

Cl C H 1,1,1-trichloroethane (TCA)

H H

C

Cl Cl C

Trichloroethylene (TCE)

Cl H

Examples

C

H C

Organic Compounds with Functional Groups

•Aldehyde: contain group C-H

O

H-C -OH H

Formaldehyde

•Ketones:

contain group with carbon

atom attached to carbon atoms

•Ethers: contain(-O-) group

•Carboxylic acids:

C O

C -OH O

H3C-C-CH3

O

O -C-OH

Benzoic acid

H 3 C-CH 2 -NH 2 Ethyl amine

 Trihalomethanes (THMs): These compounds are

present in chlorinated waters.

 BTEX: benzene, toluene, ethylbenzene, and xylene.

 Polynuclear Aromatic Hydrocarbons (PAHs):

naphthalane, anthracene, etc.