SUMMARY
The discussion focuses on calculating the mass of aluminum sulfate hydrate, Al2(SO4)3·18H2O, required to prepare a 50 mL solution with a concentration of 40 mg/mL of Al3+. The molar mass of Al2(SO4)3·18H2O is established as 666 g/mol. To achieve the desired concentration, 2 grams of Al3+ is necessary, leading to the conclusion that 24.7 grams of Al2(SO4)3·18H2O is required to provide this amount of aluminum ions.
PREREQUISITES
- Understanding of molar mass calculations
- Knowledge of solution concentration and preparation
- Familiarity with stoichiometry in chemical reactions
- Basic principles of aqueous solutions
NEXT STEPS
- Study molar mass calculations for various compounds
- Learn about stoichiometric conversions in chemical equations
- Research preparation techniques for aqueous solutions
- Explore the properties and applications of aluminum sulfate
USEFUL FOR
Chemistry students, laboratory technicians, and professionals involved in solution preparation and chemical analysis will benefit from this discussion.