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.
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Frankly I don't understand your question. You're right. Both Cu(OH)2 and BaSO4 are solids and you have labeled them correctly. According to the solubility rules, a reaction proceeds when ONE of the products is a solid. This doesn't change when BOTH products are solids.
Should've phrased it differently. I meant, why is CuSO4 and Ba(OH)2 given as aqueous solutions in the beginning? That's the problem I was given. I'm not sure why they're soluble when they're not "supposed" to be, according to my solubility rules.
An unknown compound contains only C, H, and O. Combustion of 3.70 g of this compound produced 9.03 g of CO2 and 3.70 g of H2O.
Im so confused.
Im so confused.
1 answer