Part 19 - Factors affecting solubility

solubility

• number of ml of a solvent that will dissolve 1g of a solid

• parts of solvent needed to dissolve 1 part solute

very soluble

<1

freely soluble

1-10

soluble

10-30

sparingly soluble

30-100

slightly soluble

100-1000

very slightly soluble

1000-10,000

practically insoluble

10,000>

• polar

• nonpolar

polar solvents dissolve ___ solutes
nonpolar solvents dissolve ___ solutes

non-polar

has equally distributed electrons

polar

has unequally distributed electrons

• diatomic molecules

• noble gases

• hydrocarbons

• symmetrical molecules

• electronegativity difference

under non-polar (5)

• H attached to N,O,F

• lacks symmetry

under polar (2)

• water (H₂O)

• hydrogen fluoride (HF)

• acetic acid (CH₃COOH)

• ammonia (NH₃)

• methylamine (CH₃NH₂)

• methanol (CH₃OH)

6 examples of molecules with H+ directly attached to N, O, F

• carbonyl sulfide (OCS)

• sulfur dioxide (SO₂)

2 examples of molecules that lack symmetry

• H₂

• N₂

• F₂

• CL₂

• I₂

• Br₂

diatomic molecules (6)

• methane (CH₄)

• ethane (C₂H₆)

2 examples of nonpolar hydrocarbons

• carbon tetrachloride (CF₄)

• carbon dioxide (CO₂)

2 examples of symmetry-nonpolar molecules

0 - 0.4

electronegativity difference of nonpolar covalent

0.5 - 1.7

electronegativity difference of polar covalent

ionic bond

electronegativity difference of >1.7

• higher

• greater

for solids in general, the _____ the temperature, the _____ the solubility of solid

decrease

in exothermic dissolution in solids, solubility increases with _____ in temperature

increase

in endothermic dissolution in solids, solubility increases with ____ in temperature

• higher

• lesser

for gases, the ____ the temperature, the _____ the solubility of gas

• solid

• gas

pressure does not affect the solubility of _____ but affects ____

higher

in gas, the higher the pressure, the _____ the solubility of gas

Henry’s Law

principle that states the solubility of gas is proportional to the partial pressure of gas

• partial pressure

• increases

according to Henry’s law, if you increase the ______ of gas, the solubility of the gas ____

• increase

• increase

decrease particle size = ____ surface area = _____ solubility

agitation

physical force that increases the rate of solubility

a) F₂

which molecule contains a nonpolar bond?

a) F₂
b) HCl

c) chloroform
d) acetic acid

c) asymmetrical

which statement is true about polar molecules?

a) similar charges on each end
b) symmetrical

c) asymmetrical

d) they dissolve with nonpolar substance

c) unequal pull between the shared electron

which best describes a polar bond?

a) equal transfer of electrons resulting in a positive or negative ion
b) equal pull between the shared electron
c) unequal pull between the shared electron

d) unequal transfer of electrons resulting in a (+) & (-) ion

c) hexane

which one does not act as a polar solvent?

a) water

b) ethanol
c) hexane
d) vinegar

b) freely soluble

200 parts of solvent is needed to dissolve 100 parts of solute

a) very soluble

b) freely soluble
c) slightly soluble

d) very slightly soluble

Alpha waves

• 2 protons, 2 neutrons (same as helium)

• +2 charge

• relatively large mass

• slow speed

• least penetrating ionizing effectbet

beta waves

• negatively charged, same mass as electron

• -1 charge

• very small mass

• fast speed

• more penetrating ionizing effect (can penetrate 1 inch thick aluminum)-

gamma waves

• electromagnetic wave

• no charge

• no mass

• speed of light (299, 792 km/s)

• excellent penetrating power (can penetrate thick lead)

Ci (Curie)

Non-SI unit of radiation

Bq (Becquerel)

SI unit of radiation

3.7×10¹⁰ Bq

1 Ci =

2.7×10^-11 Ci

1 Bq (to Ci) =

1 decay/s

1 Bq (decay) =

Roentgen Equivalent in Man (R.E.M)

unit of radiation damage

Rad or gray

unit of amount of exposure