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  1. So we have a lab on the heat of neutralization of NaOH and HCl given: mass of NaOH = 48.01 g Volume of NaOH = 1000.00 mL Amount of HCl = 83.3 mL of 12.0 M of HCl in 1000.00 mL solution And we found the initial temperature, final temperature Temp initial = 21.5 degrees C Temp final = 25.0 degrees C And we have to find the heat of neutralization using this equation: ΔHθneutralization = (-specific heat capacity of liquid water x mass (acid solution + base solution) x change in temp) / mole of limiting base or acid And I should be getting an enthalpy of around -58 -ish but I'm wayyy off. Help please!! P.S. I'm not that great at writing chem labs... :/
  2. Aim: the aim of this experiment is to determine the difference of enthalpy changes of neutralization reactions of strong acids and weak acids. So my strong acids were hydrochloric and nitric and weak were citric and ethanoic. Most of them are within literature value range or under which is obviously attributed to heat loss. However my ethanoic ended up being a lot higher than the others. What kind of error is that? What would be a suitable improvement? What other errors can I mention beyond more insulation, trials and accounting for the specific heat capacities of my equipment (PS what's an improvement to this one?).
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