Solutions The story continues
Heterogeneous mixture Particles of varied size
Heterogeneous mixtures Suspension – Particles settle out if left alone Colloids – Based on size of particles and the action of solution (477 table 1)
Homogeneous mixtures You cannot see various parts of the solution. (479 table 2)
Concentration Compares the amount of solute that is in a solvent Many ways to express this…
Concentration Percent by mass % by mass = (mass solute/mass solvent)*100
Concentration Percent by volume % by volume = (volume solute/volume solution)*100
Concentration Molarity Molarity = (moles solute/liters solvent)
Concentration Molarity
Concentration Molality Molality = (Moles solute/ Kg solution)
Solvation Surrounding solute with solvent
Solvation Soluble Insoluble Miscible Immiscible
Types of Solutions Unsaturated Saturated Supersaturated
Factors Agitation Surface area Temperature Solubility
Saturated Solutions Temperature effect Sugar in Water
Solubility Page 493 Figure 15
Solubility of a gas Depends on: Temperature Pressure Higher pressure “Pushes” molecules into the solution
Solubility of a gas
Solubility 10 g of a gas dissolves in 2 L of water. What is the solubility of this gas in water? 3 moles of H 2 dissolves in 10 L of water. What is the solubility of H 2 ?
Solubility of a gas
The solubility of a gas is.35 g/l at S.T.P. What is the solubility of the material if the pressure is reduced to.75 atm?
Solubility of a gas At 25°C and 1 atm, 1 g of a gas dissolves in 2 L of water. What mass of the same gas will dissolve in 2 L of water at 25°C and 4 atm?
Find the molarity of the solution formed by dissolving g Na Cl in.5 L solution.