Discussion Overview
The discussion revolves around stoichiometry calculations related to the empirical formulas of hydrated salts, specifically NiSO4 and MnSO4. Participants explore the calculations required to determine the mole ratios of the compounds and the water of hydration lost upon heating.
Discussion Character
- Homework-related
- Mathematical reasoning
- Technical explanation
Main Points Raised
- One participant calculates the moles of NiSO4 from a mass of 22.14g and finds a ratio that does not match the expected NiSO4.7H2O.
- Another participant suggests a different calculation method for the moles of NiSO4, yielding a ratio of approximately 1:6.79, and questions the accuracy of their calculations.
- A subsequent reply corrects the molar mass of NiSO4 provided by a participant, indicating that 150.76 g/mol is incorrect.
- After recalculating with a corrected molar mass, a participant arrives at a ratio of approximately 1:7, supporting the formula NiSO4.7H2O.
- A new question is posed regarding the empirical formula of MnSO4, with calculations leading to a proposed formula of MnSO4.4H2O.
- Participants discuss the naming of the hydrate, with conflicting responses regarding the correct nomenclature for MnSO4.4H2O.
Areas of Agreement / Disagreement
There is no consensus on the naming of the manganese sulfate hydrate, as participants provide conflicting answers. The calculations for both NiSO4 and MnSO4 lead to different interpretations and results, indicating multiple competing views remain.
Contextual Notes
Participants express uncertainty regarding the accuracy of their calculations and the correct molar masses. There are unresolved questions about the naming conventions for hydrates, which depend on the definitions used.