The weak acid, HX, is neutralized by sodium hydroxide as shown below:
HX(aq) + NaOH(aq) → NaCN(aq) + H2O(l).
Suppose you carried out this reaction in a coffee cup calorimeter using 50.0 mL of 0.500 M HX and 50.0 mL of 0.500 M NaOH.
If the temperature of the calorimeter increases by 2.79 °C, what is the enthalpy of this neutralization reaction (in kJ/mol)?
Assume the density of the solution is 1.00g/mL and that the specific heat is 4.184 J/g °C