Concepts

• When substances are mixed, mass is conserved, but volume might not be because particles fill gaps between each other.
• “Like dissolves like.” Whether a solute can dissolve in a solvent depends on a balance of attractive forces (solute-solvent vs. solvent-solvent and solute-solute). This means that polar substances tend to dissolve in other polar substances, and non-polar substances tend to dissolve in non-polar substances.
• When molecular (covalent) substances dissolve, their particles remain intact but separate from each other.
• When ionic solids dissolve, their ionic bonds are actually broken, producing free-floating ions.  This is called dissociation.
• The concentration of a solution is measured in molarity, meaning mol/L.
• The greater the concentration of ions dissolved in water, the greater the electrical conductivity of the solution.

Skills

Quiz 5a

• Based on polarity or ionic charge, predict whether a covalent or ionic species will dissolve in a given solvent.
• Determine the concentration of a solution.
• Perform dilution and mixing calculations.

Quiz 5b

• Describe the effect of a solvent on electrical conductivity.
• Perform stoichiometric calculations involving solutions.

Homework

• Data Booklet for Chemistry 11

Quiz 5a

• 5a.1 Predicting solubility (“like dissolves like”)
• 5a.2 Concentration
• 5a.3 Dilution problems
• 5a.4 Making solutions (includes dilution)

Quiz 5b

• 5b.1 Solution stoichiometry (includes notes)
• 5b.2 Solution stoichiometry 2

Projects & Labs

Quiz 5a

• Lab 5a.1: Like dissolves like
• Lab 5a.2: Preparing a Solution

Quiz 5b

• Lab 5b.1: Conductivity of Gatorade (may need modification)
• Lab 5b.2: Limiting reactant and percent yield in a precipitation reaction

Assessment

• Quiz 5a: Solubility, concentration, dilutions
• Quiz 5b: Conductivity, solution stoichiometry
• Test 5: Solutions