Your answer to the first post was significantly different to the 11292C/mol quoted here.
The equations are correct although your use of density seems a little extravagent - it would be far easier to actually weigh the solution!
E = mass x shc x temp rise
Then calculate the number of moles of water formed in your reaction (or the number of moles of H+ used) an divide your answer in part 1 by this number.
Using your value above 11292C/mol you are now in the ball park (17% error) and this remaining error can be explained by the heat losses I previouly outlined.
You should now be able to see some variation between strong and weak acids with the weak having perhaps a decrease of 5-10% with respect to the strong acids.
|