Why is it that copper (II) sulfate with barium hydroxide --> copper hydroxide (solid) + barium sulfate (solid)? According to the solubility rules given to me by my professor, both are insoluble, and therefore should be labeled as solids. Is there something I'm missing here? I'm in a first semester college chemistry class.
double post.
In the reaction between copper (II) sulfate and barium hydroxide, copper hydroxide is indeed a solid precipitate and barium sulfate is also a solid precipitate. The solubility rules you mentioned are correct - both copper hydroxide and barium sulfate are generally considered insoluble in water.
However, there is one crucial factor to consider when determining the solubility of a compound: the overall reaction. In this case, copper (II) sulfate(aq) reacts with barium hydroxide(aq) to form copper hydroxide(s) and barium sulfate(s). The reaction is a double replacement or precipitation reaction.
Here's the explanation behind the formation of solid precipitates:
1. Copper (II) sulfate dissociates into copper (II) ions (Cu2+) and sulfate ions (SO4 2-) in aqueous solution.
2. Barium hydroxide dissociates into barium ions (Ba2+) and hydroxide ions (OH-) in aqueous solution.
3. In the reaction, Cu2+ ions combine with OH- ions to form copper hydroxide (Cu(OH)2), which is insoluble in water.
4. Similarly, Ba2+ ions combine with SO4 2- ions to form barium sulfate (BaSO4), which is also insoluble in water.
These insoluble compounds, copper hydroxide and barium sulfate, form solid precipitates that can be observed in the reaction mixture.
In summary, while both copper hydroxide and barium sulfate are considered insoluble, they still form as solid precipitates in the reaction due to the specific combination of reactants and products. It's important to consider the overall reaction and the interaction between different ions involved in the chemical equation to determine the resulting products and their states.