Discussion Overview
The discussion revolves around calculating the equilibrium concentration of copper(I) ions in a solution where copper(I) nitrate is mixed with sodium cyanide, leading to the formation of a complex ion, Cu(CN)3. The context includes a homework problem involving chemical equilibrium and formation constants.
Discussion Character
- Homework-related
- Mathematical reasoning
- Technical explanation
Main Points Raised
- One participant presents a dilution calculation leading to new concentrations of copper and cyanide ions.
- Another participant suggests that due to the excess of cyanide, its concentration can be assumed constant after dilution, and that all copper can be assumed to be complexed based on the large formation constant.
- A participant calculates the concentration of the copper cyanide complex and attempts to use it to find the equilibrium concentration of copper ions, but arrives at a value that differs from the answer booklet.
- Another participant points out a misunderstanding regarding the stoichiometry of the complex formation, indicating that a concentration higher than 10 M suggests an error in the calculations.
Areas of Agreement / Disagreement
Participants express differing views on the assumptions made regarding the concentrations of reactants and products, particularly concerning the extent of complexation and the validity of calculated concentrations. The discussion remains unresolved regarding the correct equilibrium concentration of copper ions.
Contextual Notes
There are limitations in the assumptions made about the constancy of cyanide concentration and the implications of the formation constant. The calculations presented rely on these assumptions, which may not hold under the conditions described.