In addition to learning the theoretical content of the course, students should remember not to neglect preparing for first-hand investigations and other practical skills-based dot-points that are in the HSC Chemistry or Physics syllabus. These dot-points can be examined in one or several of the following ways:
- Exam question asking for correct procedure, safety issues, sources of error, or other related discussion
- Practical exams
Practical exams are particularly important because all students will definitely have at least one in year 12, and they are often worth around 20% of total internal assessment. We recently filmed some of our in-class practical demonstrations of experiments that are most likely to come up in practical exams at school.
In addition to learning the theoretical content of the course, students should remember not to neglect preparing for first-hand investigations and other practical skills-based dot-points that are in the HSC Chemistry or Physics syllabus. These dot-points can be examined in one or several of the following ways:
Exam question asking for correct procedure, safety issues, sources of error, or other related discussion
Practical examsPractical exams are particularly important because all students will definitely have at least one in year 12, and they are often worth around 20% of total internal assessment. We recently filmed some of our in-class practical demonstrations of experiments that are most likely to come up in practical exams at school.
HSC Chemistry
Perform a first-hand investigation and solve problems using titrations including the preparation of standard solutions, and use available evidence to quantitatively and qualitatively describe the reaction between selected acids and bases
This experiment is important because it is one of the most commonly chosen experiments for Prac Exams. Prac Exams could come any time throughout year 12 — but most of the time they occur as part of your trial HSC exams, and usually worth around 20% of total internal assessment. Therefore it is important to pay close attention to proper titration procedure and understand the underlying processes of neutralization reactions.
For this titration, our unknown was a solution of NaOH (the analyte) and our standard solution was oxalic acid (crystals in dihydrate form) — the titrant. Glassware was rinsed properly with either deionised water or with the solution it was to contain (conical flask, volumetric flask — water / pipette, burette — solution). A total of 1 ‘rough titre’ and 3 accurate titres were done. The average of the 3 accurate titres were recorded and used to finally calculate the concentration of the unknown NaOH. Our indicator was phenolphthalein due to its slightly basic endpoint (the titration was between a strong base and a weak acid, therefore the equivalence point would be slightly basic). Tip: If required to make your own standard solution, make sure you design your standard solution so that it was enough moles for you to do 3 titres.