AS Chemistry CourseworkWatch
1. "Suggest a reason why the procedure in step 2 and 3 is only possible with a carbonate that is insoluble in water such as magnesium carbonate."
>Step 2 was adding magnesium carbonate to sulfuric acid and stirring until the solution went clear, and repeating this step until the solution would no longer clear.
>Step 3 was to heat the beaker containing the solution until it became clear again, and then to add more magnesium carbonate so that some solid was in excess.
Was this something pertaining neutralisation reactions or?
2. "Suggest how your sample of magnesium sulfate would be different if in step 6, all of the water had been evaporated off."
>Step 6 being to boil the solution of magnesium sulfate on a tripod gauze until about 2/3 water evaporates.
Presumably wanting you to discuss the state of the crystals after total evaporation(?)
3. "Suggest one reason why a student carrying out the preparation apparently obtains a yield over 100%."
(this isnt my post if anyone was wondering but i have the exact same questions i need to answer. originally posted by llennon_04)