Notes on Solutions. Qualitative ways of describing solutions Dilute vs. concentrated Unsaturated, saturated, supersaturated Miscible/immiscible Solute,

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Presentation transcript:

Notes on Solutions

Qualitative ways of describing solutions Dilute vs. concentrated Unsaturated, saturated, supersaturated Miscible/immiscible Solute, solvent, solution

Quantitative methods (memorize formulas) Molarity M = mol solute 1 liter sol’nn % Mass Dilution (M 1 V 1 = M 2 V 2 )

Factors affecting RATE of solution (how fast it dissolves) Temperature Agitation (stirring) Surface area Video

Solubility of solids (how well it dissolves) Nature of solute and solvent “Like dissolves like” As temperature increases, most solids become MORE soluble Pressure does NOT affect solubility of solids

Solubility of gases As temperature increases, solubility of gases DECREASES because of kinetic energy As pressure increases, solubility of gases INCREASES

Be able to read solubility curves

Know the steps for making a standard solution.

Know the steps for diluting a solution (M 1 V 1 = M 2 V 2 )

Properties of Solutions - Electrolytes Strong electrolytes (use solubility rules) Weak electrolytes (weak acids and bases) Non-electrolytes (dissolve but DO NOT break apart into ions; e.g. sugar)

Colligative Properties of Solutions 1. Vapor pressure lowering 2. Boiling point elevation 3. Freezing point depression These properties depend ONLY on the number of particles in solution.

Earth is at the triple point!

Calculations of Boiling Point Elevation and Freezing Point Depression   T b = K b x m x i   T f = K f x m x i K f and K b are constants (given to you) Van’t Hoff factor (i) is the number of ions that a solute dissolves into –How many particles a substance will dissolve into: »NaCl  Na + + Cl -

Bonding in H 2 O Polar covalent bonds between H and O within the molecule Bent shape Polar molecule overall Hydrogen bonding between multiple water molecules

Hydrogen Bonding

Properties of H 2 O Good solvent High surface tension Adhesion/Cohesion Low vapor pressure High heat of vaporization High boiling point High specific heat capacity Solid (ice) is less dense than liquid Blue in color (appears clear in small quantities)