Chapter 1 : Properties of Solutions

Factors Affecting Solubility

Quantitative Ways of Expressing Concentration

Colligative Properties of Solutions

Solutions and Solubility

Solubility : Maximum amount of solute that dissolves completely in a given amount of solvent at particular temperature

Solute : Dissolved substances in liquid solution

Saturated solution: contain maximum amount of dissolved solute at particular temperature

Unsaturated solution: It has more capacity to dissolve more solute

Solvent : Can be gas , liquid or solid

Solution : Solvent+Solute (Homogeneous)

Dissolution: Process of dissolving a solute in a solvent

Supersaturated solution: contain more than the equilibrium amount of dissolved solute.

Parts per Billion(ppb)=mass(solute)/mass(solute+solvent) x 10^9

Mole-fraction(x)=moles(solute)/moles(solute+solvent)=1

Mass percentage=mass(solute)/mass(solute+solvent) x 100%

Molarity(M)=Mol of solute/Volume of solution(in L)

Parts per Million(ppm)=mass(solute)/mass(solute+solvent) x10^6

Molality(m)= Mol of solute/mass of solvent(in kg)

Temperature: When the temperature increases, solubility increase (kinetic energy increase), except cerium sulfate

Pressure(gases): When pressure increases, more collisions of the gas molecule per unit time with the surface of the solvent so the solubility increase.

Solute-Solvent interaction: Ionic bond, Hydrogen bond, Dipole-dipole, London dispersion forces (strength increases)

Boiling point elevation

Freezing point depression

Vapor pressure lowering

Gas liquid system: (Henry's Law) Sgas=kHPgas(constant T) where Sgas is the solubility of the gas , Pgas is the partial fraction of the gas above the solution and kH is Henry's Law constant

Solid liquid system: Qsp>Ksp, precipitate will form Qsp<Ksp no precipitate will form

Osmotic pressure

Psolution= XsolventPsolvent, Psolution is the vapor pressure of solution, Xsolvent is the mole fraction in the solution, Psolvent is the vapor pressure of pure solvent

Change in temperature =Kbmi, Kb is the boiling point elevation constant which depends on the solvent, m is the molality of the solution and i the number of particle formed when compound dissolved

Change in temperature=Kfmi, Kf is the freezing point depression constant which depends on the solvent, m is the molality of the solution and i the number of particle formed when compound dissolved

(3.142)=MRT M is the molar concentration , R is the ideal gas constant and T is temperature in kelvin

Change of P=P*solvent-Psolution