so as i'm thinking a bit sustainable in all this, i was wondering if changing the NaOH in my solutions to NaCl through adding HCl would be a good way to go for this


and when doing this, if a glass jar or sth likewise in glass would hold it's form (as in not break or dissolve or such) during the reaction


also what would be a good ratio of grams of HCl towards grams of NaOH ?

I'd also be interested in opinions on this point.

it seems to be an exothermic reaction, so things will heat up

i'm not really sure if it would be safe, glass could break, and water could probably also splash upwards i guess

so yeah, opinions more than welcome i'd say

I dont have the answer yet, but will ask my aunt who is a chemist, this is kind of basic chemistry....

But I wonder what is the tec you are doing, are you using HCL instead of vinegar?

I want to do the same thing...

take care
Jox

NaOH(aq) + HCl(aq) -> H2O(l) + NaCl(aq)
Delta(H,rxn) = Delta(H,f,NaCl)-(-detla(H,f,HClaq) - delta(H,f,NaOHaq))
= -407-(470.1+167.2)) = -1044.3 KJ/mol
DeltaH,f NaCl(aq)=(-407.27)-(-411.12)=3.85kj/mol
deltaH,f HCl(aq)=(-167.2--92.3)=-74.9kj/mol
deltaH,f NaOH(aq)=(-469.15--425.93)=-43.22
deltaH,rxn=3.85-(43.22+74.9)= -114.27KJ/mol

IF my math is correct, this reaction is exothermic. But this is at standard conditions and I bet [HCl], [NaOH], {NaCl] will be below 1M.

Hi D Empty,

Baby! you seem to know a lot, but.... so please simple english:

1. hmmmmm like what would happen with:

Naoh + HCl ? What concentration of both is needed not to make explosion in our "kitchen lab"

I think we are trying to use HCl in setead of vinegar, thinking it will give more yield, so the question is how to safely neutralize the HCl with NaOH...

Jox

there is no danger of explosion when you are neutralizing hydrochloric acid, unless the reaction vessel is closed and the pressure and energy from the reaction is not released.otherwise, depends how concentrated your solutions are, my guess is you will only see bubbling and gasses.

use Ph meter or ph strips, do not improvise with these things or you will have trouble. use dilluted solutions first and add dropwise later if its not enough, just to be on the safe side.

yes neutralization reactions are exothermic, using HCl won't give you a better yield, vinegar is just fine.

You can use either to safely neutralize NaOH. With HCl the math would of course be easier because its just a 1 to 1 molar ratio.

You could get away with adding vinegar to the NaOH until its no longer basic, no enviromental harm done, you'll be creating sodium acetate.

If your not interested in balancing equations this is the safest way to go.

Hi,

just want to say that my anunt, the chemist told me that NaOH + HCl should not be done for milions of reasons... Don't want to bother what the reasons are, but for me its enough...

and I think I will stick to the vinegar and end up eating the sodium acetate with harmalas... or is it a way to take it out?

Jox

hmm.. influencing yields ?


i was more talking about neutralizing an end-solution before ditching it in the drain kinda thing

It's OK to ditch basic solution in the drain as is. The majority of drain cleaners are concentrated NaOH anyway, so you'll be practically cleaning your pipes. When it hits the sewers, the environment there is acid enough to neutralise NaOH, so don't worry about releasing potentially casutic lye on the environment.

You could also neutralise it with any acid if that's your style, but that makes no sense and it is no more environmental as you waste more materials (acids in this case).

okay, that sounds logical


thanks !