Why does the following reaction occur when Ba(OH)2 is not good soluble? Both reactants need to be good soluble for the reaction to occur.

Ba(OH)2 + CuSO4 -- Cu(OH)2 (precipitate) + BaSO4 (precipitate)

Thanks!

Question

Why does the following reaction occur when Ba(OH)2  is not good soluble? Both reactants need to be good soluble for the reaction to occur.

Ba(OH)2 + CuSO4 --> Cu(OH)2 (precipitate) + BaSO4 (precipitate)  

Thanks!

anonymous · Answer

In my table it says that all hydroxides are not good soluble only NaOH an KOH are good soluble. But I googled the solublity of Ba(OH)2 and see its 1.67 g/100 mL (0 °C) , well i guess that is still right according to the table, but you would have to add not more than 1.67g of both reactants in a solution of 100ml for the reaction to complete, am I right?