Work through the list without notes. If you cannot do a statement, follow its link, then come back. Guide = study guide; Practice = practice questions.
Understanding
- I can explain the difference between a solution (homogeneous mixture) and a heterogeneous mixture in terms of whether properties depend on where you sample. (Guide: “Homogeneous and heterogeneous mixtures”; Practice Q1)
- I can give an example of a gaseous, a liquid and a solid solution. (Guide: “Solutions are not only liquids”; Practice Q1)
- I can explain why molarity uses the volume of the solution, not the volume of the solvent. (Guide: “Molarity”; Practice Q6)
- I can explain why a portion of a solution has the same molarity as the whole sample. (Practice Q4, Q6(d))
Calculation
- I can calculate molarity from a mass of solute and a volume of solution, converting mL to L. (Guide: “Molarity”; Practice Q4)
- I can calculate the mass of solute needed to make a given volume of a solution of known molarity. (Practice Q6(a))
- I can find the concentration and number of moles of each ion produced by an ionic solute. (Practice Q2, Q3)
- I can count the number of solute particles in a given volume of solution. (Guide: Worked example 1; Practice Q4(b))
- I can carry out single and two-step dilution calculations with M₁V₁ = M₂V₂. (Guide: Worked example 2; Practice Q5)
- I can find ion concentrations after mixing two solutions that do not react, and check the charges balance. (Guide: Worked example 3; Practice Q7)
Reasoning
- I can evaluate a method for making a standard solution and describe the correct use of a volumetric flask. (Practice Q6)
- I can explain why averaging concentrations gives the wrong answer when unequal volumes are mixed. (Practice Q7(b))
- I can state the assumptions behind a solution calculation, such as complete dissolving and additive volumes. (Revision notes: “Assumptions”)
All ticked? Move on to Topic 3.8, Representations of Solutions, or return to the course roadmap.