Consider two solutions, the first being 50.0 mL of1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH.When the two solutions are mixed in a constant-pressurecalorimeter, a precipitate forms and the temperature of themixture rises from 21.5 to 27.7 °C. (a) Before mixing, howmany grams of Cu are present in the solution of CuSO4?(b) Predict the identity of the precipitate in the reaction.(c) Write complete and net ionic equations for the reactionthat occurs when the two solutions are mixed. (d) From thecalorimetric data, calculate ΔH for the reaction that occurson mixing. Assume that the calorimeter absorbs only a negligiblequantity of heat, that the total volume of the solutionis 100.0 mL, and that the specific heat and density of thesolution after mixing are the same as those of pure water.
Consider two solutions, the first being 50.0 mL of
1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH.
When the two solutions are mixed in a constant-pressure
calorimeter, a precipitate forms and the temperature of the
mixture rises from 21.5 to 27.7 °C. (a) Before mixing, how
many grams of Cu are present in the solution of CuSO4?
(b) Predict the identity of the precipitate in the reaction.
(c) Write complete and net ionic equations for the reaction
that occurs when the two solutions are mixed. (d) From the
calorimetric data, calculate ΔH for the reaction that occurs
on mixing. Assume that the calorimeter absorbs only a negligible
quantity of heat, that the total volume of the solution
is 100.0 mL, and that the specific heat and density of the
solution after mixing are the same as those of pure water.
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