SOLUTION

SOLUTESOLVENT

Mostly process of chemistry run away in the solution Solution is homogeneous mixture Solution can be solid-solid, solid-liquid, solid- gaseous, liquid-solid, liquid-liquid, liquid-gaseous, solid-gaseous, gaseous-gaseous Composition of solution called concentrationThe concentration of solution is amount of solute per unit of solvent or solution

The Concentration can be represented by:-percentage (W,V); part per million (ppm);-Molar (M): amount of mol of solute per volume of solution (liter)-Molal (m): amount of mol of solute per 1000 gram of solvent-Mol fraction: amount of mol of solute per amount of mol of solute + mol of solvent-Normal: amount of equivalent of solute per volume of solution (liter)How relation mol and equivalent of substances?We have 2 relation: acid-base; reduction-oxidation

Acid-bases equivalent1 eq ~ 1 mol of H+ or 1 mol of OH-How about 1 mol HCl =eq 1 mol Ba(OH)2 =eq 1 eq H2SO4=mol 1 mol NaCl=eq 1 eq Na2CO3=molReduction-oxidation equivalent1 eq ~ 1mol of electronHow about 1 mol Cl2 =eq (Cl- Cl2) 1 mol SO4-2 =eq (SO4-2 SO2) 1 eq Mn+2 =mol (MnO2 Mn+2) 1 eq ClO3- =mol (ClO3- Cl-)

IDEAL SOLUTIONSThe ideal solutions has property precise in between its solute and its solvent, but really there are no solution like thatThe model of solution like that called ideal solutionsIn the ideal solutions, i = o + RT ln Xi i = potential chemistry of i in the solutiono = potential chemistry of pure solventR = constantT = TemperatureXi = mol fraction of i in the solutionRaoults Law: The solution consist of liquids solute j and solvent i, Pj = Xj.Pjo Pi = Xi.Pio

NON IDEAL SOLUTIONS(Real solutions)There is deviation property of the real solutions from the ideal solutions: positive deviation (the property of solutions bigger than of ideal solutions); ether carbon tetra chlorideNegative deviation (the property of solutions lower than of ideal solutions); acetone-chloroform

COLLIGATIVE PROPERTIES OF SOLUTION

Colligare collective influence There are 4 colligative properties of solutions:- Vapour pressures of solutions- Boiling-point elevation- Melting-point depression- Osmotic pressureColligative properties of non electrolyte solution- Pj = Xj.Pj j = solvent- P = Xi.Pj i = solute- Tb = mi.Kb - Tf = mi.Kf- = CRT

Colligative properties of electrolyte solutionsComparing with non electrolyte solutions, the electrolyte solution have more particlesAmount particles of the electrolyte solution equal 1 + (n-1) amount particles of the non electrolyte solution- P = Xi.Pj {1 + (n-1)} - Tb = mi.Kb {1 + (n-1)} - Tf = mi.Kf {1 + (n-1)} - = CRT {1 + (n-1)}

THE IONIZATION OF WATER AND THE pH CONCEPTWater is very weak electrolyte, the reaction isH2O + H2O = H3O+(aq) + OH-(aq)the chemical equation become:H2O = H+ + OH-Kw= (H+).(OH-) Kw = 10-14In pure water T=25oC (H+) = (OH-) = 10-7pH concept p mean -log pH = - log(H+)pOH = -log(OH-)pKw = -log KwpKa = -log KapKb = -log KbIf the (H+) = (OH-) the solution is neutral (H+) > (OH-) the solution is acid (H+) < (OH-) the solution is base

Strong Acid and Strong BaseHX H+ + X- (1) pH = -log(H+)LOH L+ + OH- (1) pOH = -log(OH-)What is th pH of HCl (aq) 0,001M?What is the oH of HCl (aq) 10-8M?What the pH of HY (aq) 0,1 M, if the is 0,8?

Weak Acid and Weak BaseHA H+ + A- (

HYDROLYSISHydrolysis is the reaction of salt with water become its weak acid or weak base Salt (strong acid and strong base) no hydrolysisFor expl: NaCl, KI, Ba(NO3)2 etcSalt (strong acid and weak base) basis hydrolysisFor expl: NH4Cl, C6H5NH2 etcSalt (weak acid and strong base) acid hydrolysisFor expl: KCN, Na.Asetat, etcSalt (weak acid and weak base) total hydrolysisFor expl: NH4CN, C6H5NHOOCCH3

BUFFERBuffers solution resist significant change the pHBuffers solution can be found for a weak acid and its base conjugation solution (namely buffer acid); or from a weak base and its acid conjugation solution (namely buffer base)For expl: Buffer acid (CH3COOH + CH3COO-) Buffer base (NH4OH + NH4+)(H+) = (acid)/(base conjugation). Ka(OH-) = (base)/(acid conjugation). KbEffectively of buffers solution can be done from (acid)/(base conjugation) or (base)/(acid conjugation) between 0,1 to 1,0

ACID-BASE TITRATIONEquivalence pointThe end of titration pointACID-BASE INDOCATORSThe range of pH in difference color

SOLUBILITY AND SOLUBILITY PRODUCT CONSTANT (Ksp)The solubility in moles of solute per dm3 of saturated solution is called the molar solubilityAmBn(s) + H2O = mA+n(aq) + B-m(aq) Ksp AmBn = (A+n)m.(B-m)n

Relation of solubility (l) and KspSolubility of AmBn = (Ksp AmBn/mmnn).exp mmnnHow to know the precipitation? For the AmBn If the (A+n)m.(B-m)n = Ksp AmBn saturated solution (A+n)m.(B-m)n < Ksp AmBn diluted solution (A+n)m.(B-m)n > Ksp AmBn precipated AmBn

Complex ions and SolubilityA Complexing agent is a substance that can for a complex with a metal ion (e.g NH3)AgCl(s) + 2NH3(aq) = Ag(NH3)2+(aq) + Cl-(aq) ..Kc?KcKspKformKc = Ksp.Kform