1. Assuming the density of solution=1.00 g/mL
Volume of solution=Volume of HX+Volume of NaOH
=50.0 mL+50.0 mL=100.0 mL
Mass of solution=Volume x Density
=100.0 mL x 1.00 g/mL
=100.0 g
As the temperature of the calorimeter increases by 1.79°C, this means heat released in the neutralisation reaction is absorbed by the calorimeter
Heat absorbed=Mass of solution x specific heat of solution x rise in temperature
=100.0 g x 4.184 J/g°C x 1.79°C=748.94 J
Number of moles of HX=Molarity x volume (L)
=0.500 M x 50.0 mL/1000 mL/L=0.025 mol
Number of moles of NaOH=Molarity x volume (L)
=0.500 M x 50.0 mL/1000 mL/L=0.025 mol
So HX and NaOH completely neutralise each other as number of moles of HX and NaOH are equal.
Enthalpy of neutralisation=-heat absorbed by the solution/number of moles of HX
=-748.94 J/0.025 mol=(-748.94 J/1000 J/kJ)/0.025 mol
=-29.96 kJ/mol
So Enthalpy of neutralisation=-29.96 (without units as asked in the question)
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