KIMIA

                        a. Substance Type influence on solubility

Substance substance with structured chemical kindred one generally gets each other get mingling with every consideration, meanwhile structured substance substance its different chemical by and large reducing can mutually get mingling  (like dissolves like) . Compound that gets character polar will be easily leach in dissolving polar, meanwhile compound nonpolar will be easily leach in dissolving nonpolar. Its example is alcohol and water gets perfect mingling  (completely miscible) , water and ether gets to mix a portion  (partially miscible),  meanwhile oil and nots water get mingling  (completely immiscible) .

 b. Temperature influence on solubility

Solubility gases generally dwindling on superordinate temperature. E.g. if water is heated, therefore evoked secretory gas bubbles from within water, so gas that most water-soluble that becomes dwindling. Mostly solubilities solid substance it be even greater on superordinate temperature. There are several solid substance that its solubility decreases on superordinate temperature, e.g. sulphate sodium and sulphate cerium. On saturated solution to be gotten kesetimbangan among processes dissolution and crystallizing process be back. If one of process gets endoterm's character, therefore contrariwise process gets eksoterm's character. If temperature is raised, therefore in accordance with principality Le Chatelier (Henri Louis Le Chatelier: 1850 - 1936)  kesetimbangan is shifting toward endoterm's process. So if processes dissolution to get endoterm's character, therefore its solubility increases on superordinate temperature. On the contrary if processes dissolution to get eksoterm's character, therefore its solubility decreases on superordinate temperature. 

solubility

Pb (NO. ₃ ) ₂

KCl

Na ₂ SO ₄

NaCl

. Na ₂ SO ₄ .10H ₂ O

Ce ₂  (SO ₄ ) ₃

temperature

Image 1. subjective curve among salt umpteen solubility with temperature. 

c. Pressure influence on solubility

Its influence pressure change little to hydrogen solubility or thickly. Pressure change as big as 500 atm just revamp NaCl's solubilities about 2,3 % and NH ₄ Cl is vicinity 5,1 %. solubility gases to equal pressure partial that gas. Legally Henry (William is Henry: 1774 - 1836)  mass gases that melarut in to amount to liquid particular (its dissolving) straight equal with pressure that did by that gas (pressure partial ), one that lies deep kesetimbangan with that solution. Its example is oxygen solubility in crescent water as 5 times if pressures partial -the is raised 5 times. This law is inoperative for gas what do react with dissolving, e.g. HCl or NH ₃ in water. 

3. Solution concentration

Solution concentration declares for a lot of dissolved substance in to amount to solution particular. Physics ala concentrates to get is declared for deep % (percent) or ppm  (part per million)  = bpj (a part about million). In chemical concentrates stated solution in molar (M ), molal (m ) or normal (N ). 4

a. Molaritas (M )

Molaritas declares for to foot up dissolved substance mole in each solution liter. 

LmLxmLmolLmollaruvolumeterlarutzatmolM /1000tan===

b. Molality (m )

Molality declares for to foot up dissolved substance mole in each gram kilo (1 000 gram) dissolving. 

c. Normality (N )

Normality declares for to foot up dissolved substance equivalent in each solution liter. 

MxnLmolxnLMrgramxnLnMrgramLekuivalenmassasolutemassalaruLsoluteekuivalenN ======tan

Equivalent mass is substance mass required just for catch or releasing 1 electron mole in reacts (redoks's reaction). 

kggxpelarutgterlarutzatmolpelarutkgterlarutzatmolm /1000==

Trifling example: 

As much 1,11 g CuCl ₂ dissolved into 100 g waters. If water type mass 1 g / mL, Cu's relative atomic mass = 40 and Cl's relative atomic masses = 35,5, therefore accounts that solution concentration is deep: 

a. Molar

b. Molal

c. Normal

Answer: 

molar CuCl's mass ₂ = 40 + (2 x 35,5 ) = 111 g / moles

Water volume = mass: type mass = 100 g: 1 g / mL = 100 mL

CuCl's mole ₂ = mass: molar's mass = 1,11 g: 111 g / moles = 0,01 mole

If solution volume = water volume, therefore

a. M CuCl ₂ = (mole: mL) x 1000 mL / l = (0,01 mole: 100 mL) x 1000 mL / l = 0,1 M

b. m CuCl ₂ = (mole: g ) x 1000 g / kg = (0,01 mole: 100 g) x 1000 g / kg = 0,1 m

c. CuCl _{2 (aq)}  ? ?  Cu ^{2 +}  _(aq)  + 2 Cl ^-    _(aq) 

Cu ^{2 +}  _(aq)  + 2 e ? ?  Cu  _{(s )}

2 equivalent electron moles with 1 CuCl's mole ₂ . So n = 2 ek / moles. 

N CuCl ₂ = n x moles: L = 2 ek / moles x 0,001 mole: 0,1 L = 0,2 N