properties of solutions solution: homogenous mixture of 2 or more substances; particles are small...
TRANSCRIPT
Properties of Solutions
Solution: Homogenous mixture of 2 or more substances; particles are small (transparent)
Colloid: Homogenous mixture of 2 or more substances; particles are larger (opaque)
Solutions can be liquid, solid or gaseous
Examples: Ocean, sugar water
Gold alloy
Air, humid oxygen
Solvent: Substance present in a solution in the greatest amount
Example: Water in the ocean; nitrogen in air
Solute: Substance present in a solution in lesser amounts than the solvent
Example: Salt in ocean; oxygen in air
Solutes can be electrolytes or nonelectrolytes
Electrolytes: solutes that dissociate in solution into ions that carry charge (ionic compounds)
Nonelectrolytes: solutes that do not dissociate in solution, and do not carry any charge
Solubility
Soluble substance: Substance that is able to dissolve in a solvent
Insoluble substance: Substance that does not dissolve in a solvent
Solubility: Maximum amount of solute that can be dissolved in a specific amount of solvent under specific conditions of temperature and pressure (g solute/100 mL solution)
Saturated Solution: Solution containing maximum amount of solute that will dissolve under current conditions
Unsaturated Solution: Solution containing less than the maximum amount of solute that will dissolve under current conditions
Supersaturated Solution: Unstable solution containing amount of solute greater than the solubility value
General Rules for the Solubility of Ionic Compounds
•A compound is soluble if it contains one of the following cations:
-Group 1A cations: Li+, Na+, K+, Rb+, Cs+
-Ammonium, NH4+
•A compound is soluble if it contains one of the following anions:
-Halide: Cl-, Br-, I-, except for salts with Ag+, Hg22+, Pb+2
-Nitrate, NO3-
-Acetate, CH3CO2-
-Sulfate, SO42-, except for salts with Ba+2, Hg2
2+, Pb+2
Solubility of Solids and Liquids vs. Gases
•Solubility of liquids and solids in water increases with increasing temperature
Example: More sugar will dissolve in warm water than in cold water
•Solubility of gases in water decreases with temperature
•Solubility of gases in water increases with increasing pressure (Henry’s Law)
“Like dissolves like:”
polar solvents will dissolve polar solutes
nonpolar solvents will dissolve nonpolar solutes
Examples: wax in CCl4, sugar in water; oil in water?
Solutes fail to dissolve when:
1) forces between solute particles out-weigh attractions between solute and solvent
2) solvent particles are more attracted to each other than to solute
Examples of Like Dissolves Like
Solvents Solutes
Water (polar) Ni(NO3)2
(ionic)
CH2Cl2 (nonpolar)
I2 (nonpolar)
Solutes dissolve faster when:
Concentration: Relationship between amount of solute contained in a specific amount of solution
Solute particles are small
Solvent is heated
Solution is stirred
Concentration as Percent
Percent: Solution concentration giving the amount of solute in 100 parts of solution
% = part/total x 100
Weight/weight percent: Concentration giving the mass of solute in 100 mass units of solution
%(w/w) = solute mass/solution mass x 100
Example: 12.0%(w/w) sugar solution
12 g sugar per 100 g solution
Weight/volume percent: Concentration giving the grams of solute contained in 100 mL of solution
%(w/v) = grams solute/mL solution x 100
Example: 12.0%(w/v) sugar solution
12 g sugar per 100 mL solution
Molarity: Unit of concentration used with solutions; number of moles of solute per liter of solution
Molarity (M) = moles of solute/liters of solution
Examples: 2 moles of NaCl dissolved in 1 L of water
M = 2 moles/1 L = 2 M
1.5 moles NaCl dissolved in 2 L of water:
M = 1.50 moles/2.00 L = .750 M
Dilution
Dilution: addition of solvent to decrease theconcentration of solute. The solution volume changes,but the amount of solute is constant.
moles of solute (mol) = molarity (M) x volume (V)
initial values final values
M1V1 = M2V2
M1 V1 =M2 V2
Practice Problem: Prepare 250 mL of 0.100 M NaCl solution from a 2.00 M NaCl solution.
M1 = molarity of starting solution (in this case 2.00M NaCl)
V1 = volume of starting solution required (always unknown)
M2 = molarity of final solution after dilution (in this case 0.100M NaCl)
V2 = volume of final solution, after dilution (in this case 250ml)
Prepare 250 mL of 0.100 M NaCl solution from a 2.00 M NaCl solution.
M1 = molarity of starting solution (in this case 2.00M NaCl)
V1 = volume of starting solution required (always unknown)
M2 = molarity of final solution after dilution (in this case 0.100M NaCl)
V2 = volume of final solution, after dilution (in this case 250ml)
M1 V1 =M2 V2
V1 = M2 V2 / M1
V1 = (0.100M) x (250 ml) / (2.00M) = 12.5ml
Osmotic Pressure
Osmosis: Movement of water through a semipermeable membrane, from more dilute solution towards more concentrated solution
Osmotic pressure: amount of pressure required to stop flow of water due to osmosis
Isotonic solutions: solutions with identical osmotic pressure; no urge for water to flow
4% starch
10% starch
H2O
Example:
During osmosis, water flows across the semi-permeable membrane from the 4% starch solution into the 10% solution.
Eventually, the flow of water across the semi-permeable membrane becomes equal in both directions.
7% starch
7% starch
H2O
Hypotonic solution: the more dilute of 2 solutions separated by a semipermeable membrane; water leaves this solution and flows across membrane to the more concentrated solution
Hypertonic solutions: the more concentrated of 2 solutions separated by a semipermeable membrane; water enters this solution, moving across the membrane from the more dilute solution
Crenate Burst No Change
(hypertonic) (hypotonic) (isotonic)