SUMMARY
The discussion centers on calculating the molarity of Ca2+ ions required in a reaction mixture containing 9.99 g of solid CaSO4 and a total volume of 4 L. The balanced chemical equation provided is Al2(SO4)3(aq) + 3 CaBr2(aq) → 2 AlBr3(aq) + 3 CaSO4(s). The correct conversion of 9.99 g of CaSO4 to moles is approximately 0.0293 moles, not 1.36 moles as initially assumed. The molarity of Ca2+ ions can be determined using the formula concentration = moles/volume, leading to a final calculation of approximately 0.0117 M for the Ca2+ ions.
PREREQUISITES
- Understanding of stoichiometric ratios in chemical reactions.
- Knowledge of molar mass calculations, specifically for CaSO4.
- Familiarity with the concept of molarity and its formula (moles/volume).
- Basic skills in unit conversions related to mass and volume.
NEXT STEPS
- Learn how to perform stoichiometric calculations in chemical reactions.
- Study the molar mass of common compounds, focusing on calcium sulfate (CaSO4).
- Explore examples of calculating molarity for various ionic solutions.
- Investigate the implications of stoichiometry in real-world chemical applications.
USEFUL FOR
Chemistry students, educators, and anyone involved in chemical analysis or laboratory work requiring stoichiometric calculations and molarity determinations.