50 ml of 0.2 M solution of $\ce{HCl}$ is mixed with 75 ml of 0.2 M solution of $\ce{NaOH}$ in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$

$\Delta H = -57\ \mathrm{kJ}$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature?


I think you can't. You will obtain the heat produced on the reaction. Then, with this value an the specific heat for the final solution you can calculate an increase of temperature. I.e. if you obtain a increase of 10 K, and the inutial temperature is 293 K, the final temperature will be 303 K, but if originally is 313 K, at the en it will be 323 K.

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