Rob

Its OK guys, don't fret too much any more - NaOH + COOH -> COONa + H2O

Well, I though NaCO3, but something in the balancing didn't seem to add up

OK, a titration question for you here: "In order to determine the aspirin content of a commercial aspirin tablet, a tablet weighing 0.400g was dissolved in aqueous ethanol and titrated with 0.100M NaOH solution: 16.7cm^3 of the NaOH was required to reach the end point. Under the conditions of the titration, only the Carboxylic acid group reacts with the NaOH". Obviously, the question goes on to ask about moles in the aspirin, and the % by mass of aspirin in the tablet, but what I need to know is what is the balanced equation for this reaction? NaOH + COOH -> ? Cheers, Thanks for your help.

2Mg + 2NaOH -> 2MgO + 2Na + H2 Aqueous solution of NaOH or something else?

I certainly think that anywhere away from the smokers house should be somewhere that they can't light up, and for a number of reasons. Firstly, because of the health risk to other people, and that is the effects of extended passive smoking on anyone, for example that of waiters in restaurants &c. Even though smokers are banned from doin so on the premesis, restaurants and pubs still give them places to smoke outside, which is a mockery of the whole idea of banned smoking in public places, and would still contribute to staff passive smoking, because they're still smoking in their vicinity. Also, to walk through a town centre at night gives this passive smoking, because you have to walk past pubs which used to contain their smoke, but have now shoved it onto the street, meaning that when you get to wherever you're going you stink of a thousand cheap cigarrettes and are coughing horribly. Then, we have the whole aesthetic situation, which is one of quite unnapealing men and women stood drunk outside bars, swaying, with a lit rod in their mouth, which they drop on the streets. Which obviously isnt incredibly nice - to have hundreds of dropped cigarette ends littering the floor. That would also increase the city council's spending on street cleaning, when that money could be more helpfully spent elsewhere.

I don't think that twelve year old kids can really understand chemical forulae and proper terms though ... so they should have a bit of a problem with that aspect of this forum.

Well, i agree that lots of people might not know what is safe or not are a bit in danger, but anyone with a GCSE in chemistry (christ knows what that is in america, high school or something?) will know what is safe and what isn't. And any way, being from England, i don't have what seems to be a selectively american litigation compulsion - it just wouldn't work.

Why is it that any time you post something asking a question about anything interesting that may be considered dangerous moderators shut your thread down? Surely its better to give the info out and then let us decide whether its something that we want to try at our own personal risk? someone answer me, especially if you're a damned moderator. Thankyou.

and how large would this voltage have to be?

hmmm ... for that you'd need one of those permeable diaphragms ... but i dont know where to get one.

bored

I'm looking for a way to get some kind of reasonably reactive nitrate for a reaction ... either that or dilute nitric acid. Does anyone know where i can get them in the UK, in decent extractable concentrations if they're in solution, or in thir pure form? thanks Merged post follows: Consecutive posts mergedAlso, if you used sodium nitrate and KCl, how would you part the two in the resultant solution? (as this is what i am aiming for)

mmm, i could have been more specific. I mean aqeous NaCl, with a view to obtain Sodium Hydroxide, Chlorine and Hydrogen.

What should i use for the anode and cathode in the electrolysis of NaCl - two Carbon or something else? Regards

is this with the NaOH dissolved in water or melted?

How can i produce Acetylene from Acetic acid?

The bi-products of the electrolysis of NaCl(aq) are Chlorine and Hydrogen, so surely you could just put a lit splint into whatever you've collected from the electolysis, then add Purified (Distilled) water. So that's your hydrochloric acid.

could you not just use Aqeuous Sodium Hydroxide? Wait, no, stupid question

Ok, again, in my search for sodium, as my last thread was shut down by the moderator and i can't generate the heat needed to make Sodium from liquid Sodium Chloride, Is there any way of getting sodium (by SIMPLE electrolysis or anything else that doesn't need something more reactive than sodium to get rid of it) out of Sodium Hydroxide that i've obtained fro the electrolysis of aqueous Sodium Chloride? Cheers.

yeah, if you electrolyse aqueous (CuSO4 in water) Copper Sulphate with copper electrodes then you should get copper stuck to the electrodes and a (sulpur trioxide?) solution (or gas, im not quite sure) which when added to water would get you sulphuric acid. I think ... which kind of makes redundant the whole adding SO3 to water to make H2SO4 to make the CuSO4 that you need to make the sulphur trioxide.

Ok, I'd like to extract sodium metal from Sodium Chloride, but I do have a few problems with the electrolysis of molten Sodium Chloride, a few of which are that: A. I have no idea where to get Calcium chloride from to reduce the melting temperature of the Sodium Chloride. B. I dont have the means to heat anything up to 600*C, and have no idea where to legally get a bunsen burner other than online in the UK, as I dont have a credit card. Also, I have a query about the method that involves the electrolysis of aqueous NaCl, which is; How would you prevent the formation of Sodium Hydroxide &c after, or indeed during, the electrolysis?