[Gweedo8]

I obtained a calorimeter and added 10mLs of 6.00M sulfuric acid. I obtained a burette and added 50mLs of 6.00M sodium hydroxide. I collected the pH meter and titration data (This lab was done on the computer). I Started the titration by adding NaOH and watched the temperature. I continued the titration until 30.0mLs of NaOH has been added.
At the highest temperature of this titration the Volume was19.8 mL, The Ph levels was 1.4252 pH and the temperature was 58.2867C
When I stopped the titration with 30mL of NaOH the Volume was 30 mL, The Ph levels was 14.1532 pH and the temperature was 49.3241C

Here are the question I cannot figure out:

Assume the solution density is 1g/mL. Using the mass of the solution as the mass of water, determine how much heat was absorbed by the water?

What is the theoretical heat of the solution?

What is the percent error? (absolute value)

If I left some info out will you please tell me what I ma missing so I can try to get some help on this, Thank you!

[calciumoxide]

For the heat absorbed by water, you would use heat (absorbed by water)= heat (released by the rxn)=mass x specific heat x change in temperature. So you know the density of water (1g/ml) and the volume at max temperature (20 ml), you can calculate for mass of water and you will you this mass for that equation since you are assuming mass solution = mass water. Now for temperature, I think you assume the initial temperature to be the room temperature (25C) and you use max temp - room temp = change in temperature.

Theoretical heat of solution is just the enthalpy of the reaction so you would need to know the reactants and products and find their enthalpies of formation of this reaction.