multiply the mass of the solution by its specific heat capacity and by the temperature change. 

multiply the calorimeter constant by the temperature change.

multiply the specific heat capacity of the solution by the temperature change. 

multiply the calorimeter constant by the mass of the calorimeter and by the temperature change.

Weigh the sample tube, cap and NaOH before adding it, weigh the sample tube, cap after adding NaOH to solution. Calculate difference in masses. 

Tare balance with empty sample tube, add NaOH and measure mass. 

Tare balance with empty sample tube, add NaOH and measure mass. Re-weigh after adding NaOH to solution. 

There is excess HCl. 

This is a stoichiometric mixture, there is no limiting reagent. 

The limiting reagent is NaOH. 

The limiting reagent is HCl.

Verifying the acidity/basicity of the final solution with litmus paper. 

Accurately measuring the volume of NaOH solution in part A. 

Stirring the mixture in the calorimeter continuously while making temperature measurements. 

taking the heat absorbed by the calorimeter and then changing the sign

adding the heat absorbed by the calorimeter to the heat absorbed by the solution, and then changing the sign

taking the heat absorbed by the solution, and then changing the sign

adding the heat absorbed by the calorimeter to the heat absorbed by the solution

∆H_A = ∆H_B + ∆H_C

∆H_C = ∆H_A + ∆H_B

∆H_B = ∆H_A + ∆H_C

multiply the mass of the solution by its specific heat capacity and by the temperature change. 

multiply the calorimeter constant by the temperature change.

multiply the calorimeter constant by the mass of the calorimeter and by the temperature change.

Point "D"

Point "A"

Point "B"

Point "C"

Point "E"