100.0 mL of 1.020 M HCl and 50.0 mL of 2.040 M NaOH, each at 24.53ºC, are mixed in a Styrofoam cup calorimeter. What is the final temperature of the mixture if the heat of acid-base neutralization (ΔHneut) = −57 kJ per mole of H2O formed? (Assume density of the solution = 1.00 g/mL and specific heat of the solution = 4.184 J/g•ºC, and assume an insignificant heat capacity of the Styrofoam cup)

Question

100.0 mL of 1.020 M HCl and 50.0 mL of 2.040 M NaOH, each at 24.53ºC, are mixed in a Styrofoam cup calorimeter.  What is the final temperature of the mixture if the heat of acid-base neutralization (ΔHneut) = −57 kJ per mole of H2O formed?  (Assume density of the solution = 1.00 g/mL and specific heat of the solution = 4.184 J/g•ºC, and assume an insignificant heat capacity of the Styrofoam cup)

aaronq · Answer

you gotta use $q=m*C_p*\Delta T$

remember that $\Delta T=T_f-T_i$