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Chem help: adding solid NaOH pellets to HCL?
Suppose that you had added solid sodium hydroxide pellets to hydrochloric acid, instead of adding hydrochloric acid to sodium hydroxide solution?
a) Do you think that you would have obtained a different enthalpy change?
b)would the enthalpy change have been higher or lower?
d)what change do you need to make to the thermochemical equation if you perform the investigation using solid sodium hydroxide?
I don't necessarily need the full answer, but I would like to know how to answer these questions... I don't really know :S
1 Answer
- JohnLv 610 years agoFavorite Answer
There are some steps taking place with the solid NaOH that wouldn't happen with a solution.
The lattice energy of solid sodium hydroxide needs to be overcome, to seperate all the sodium ions from the hydroxide ions. That's an endothermic change.
But you get back the enthalpy of solvation of sodium; the Na+ ions get covered by a shroud of water molecules. This part is exothermic.
If you dissolve some sodium hydroxide, does the solution get warmer or cooler? That's the energy change that you need to take into account because that's the step you're adding into the neutralisation reaction.
The link below will tell you more
