rocketsurgeon
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sulfuric acid
hello,
I just got a 500ml bottle of acs grade sulfuric acid and 700 ml of hydrochloric acid.
I would like to know a few good syntheses I can do.
Right now I don't have a lot of reagents, mainly just household chemicals.
By the way I know the sugar and sulfuric acid reaction.
and yes i know sulfuric acid is very unforgiving and reactive.
thank you.
[Edited on 26-7-2013 by rocketsurgeon]
[Edited on 26-7-2013 by rocketsurgeon]
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subsecret
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Sulfuric acid can be used as a catalyst in many, many reactions. You may want to look some of them up. Copper sulfate can be made with electrolysis of
a sulfuric acid solution with copper electrodes.
Be careful with that stuff!
Fear is what you get when caution wasn't enough.
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Fantasma4500
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oh man (: im just too sure this will be moved to detritus
you just dont buy something like sulfuric acid, and then consider if you think its an ''amusing'' chemical hahahahhaha
this is not some toy xD
you should perhaps look onto ''detritus'' as you might not know what it is yet, lol
i actually have some suggestions, but earlier conversation with admin has talked me from sharing such .. well.. ''self-reactive'' reactions or what
you might call it
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ElectroWin
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well, you can use H2SO4 to make other acids
you can get some bone ash and have the H2SO4 attack that, forming CaSO4 which precipitates, and depending on the pH, monocalcium phosphate, which is
soluble.
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bfesser
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Experiments and Advice for rocketsurgeon
<u>A simple series of experiments/demonstrations:</u>
- add a small scoopful of the <a href="http://en.wikipedia.org/wiki/Copper(II)_sulfate" target="_blank">CuSO<sub>4</sub>
· 5 H<sub>2</sub>O</a> <img src="../scipics/_wiki.png" /> to one of the glass culture tubes (test tubes without
rims)
- carefully add enough of the <a href="http://en.wikipedia.org/wiki/Sulfuric_acid"
target="_blank">H<sub>2</sub>SO<sub>4</sub></a> <img src="../scipics/_wiki.png" /> to cover the salt
- make careful observation of the color of the salt over time
- record procedures and observations in the lab notebook in labeled and dated entries
- take photos and share with is, if you like
- keep small samples of each new chemical in labeled/dated vials
- neutralize by carefully pouring the mixture into a beaker of cold water and adding <a href="http://en.wikipedia.org/wiki/Sodium_bicarbonate"
target="_blank">NaHCO<sub>3</sub></a> <img src="../scipics/_wiki.png" />
- if you want, you can recover the <a href="https://en.wikipedia.org/wiki/Copper(II)_carbonate"
target="_blank">CuCO<sub>3</sub></a> <img src="../scipics/_wiki.png" /> that precipitates using the glass funnel (with the
narrow stem) and a circle of coffee filter paper
- write reactions to explain why it's not Cu(HCO<sub>3</sub> <sub>2</sub> (hint: <a href="https://en.wikipedia.org/wiki/Carbon_dioxide"
target="_blank">CO<sub>2</sub></a> <img src="../scipics/_wiki.png" /> gas is evolved)
- rinse the filtrate with distilled water, and carefully spread it out to dry
- dilute some of the <a href="http://en.wikipedia.org/wiki/Hydrochloric_acid" target="_blank">HCl</a> <img src="../scipics/_wiki.png"
/>, and use it to dissolve some of the <em>filtered and dried</em> CuCO<sub>3</sub> in the spot plate
- record observations
- allow the solution to evaporate, and recover the <a href="http://en.wikipedia.org/wiki/Copper(II)_chloride"
target="_blank">CuCl<sub>2</sub> · 2 H<sub>2</sub>O</a> <img src="../scipics/_wiki.png" />
- <em>gently</em> heat a little of the CuCl<sub>2</sub> · 2 H<sub>2</sub>O in a tube and explain your
observations
- write out the chemical equations for all of this in your new notebook
- I <em>wouldn't</em> recommend doing the same with the <a href="https://en.wikipedia.org/wiki/Cobalt_chloride"
target="_blank">CoCl<sub>2</sub> · 6 H<sub>2</sub>O</a> <img src="../scipics/_wiki.png" />
(toxic/corrosive HCl gas, carcinogen, etc.), but you can try <em>gently</em> heating it
- rehydrate/dissolve in H<sub>2</sub>O
- precip. with NaHCO<sub>3</sub>
- dissolve precip. with dil. H<sub>2</sub>SO<sub>4</sub>
- etc.
note: Cu<sup>2+</sup>(aq) is very harmful to marine environments, avoid dumping it down the drain
<u>Other ideas:</u>
- use the crucible to prepare <a href="https://en.wikipedia.org/wiki/Sodium_carbonate"
target="_blank">Na<sub>2</sub>CO<sub>3</sub></a> <img src="../scipics/_wiki.png" /> from your
NaHCO<sub>3</sub>
- make some nice crystals of the CuSO<sub>4</sub> · 5 H<sub>2</sub>O
- find some <a href="http://en.wikipedia.org/wiki/Sodium_acetate" target="_blank">sodium acetate</a> <img src="../scipics/_wiki.png"
/> (sorry, I forgot to grab some), and using the H<sub>2</sub>SO<sub>4</sub> and retort, distill a little <a
href="http://en.wikipedia.org/wiki/Acetic_acid" target="_blank">acetic acid</a> <img src="../scipics/_wiki.png" />
- purify some expired <a href="http://en.wikipedia.org/wiki/Aspirin" target="_blank">aspirin</a> <img src="../scipics/_wiki.png" />
tablets, and make <a href="viewthread.php?tid=9920">copper(II) aspirinate</a>! 
- get a 6 volt lantern battery and try some <a href="https://en.wikipedia.org/wiki/Electrochemistry" target="_blank">electrochemistry</a>
<img src="../scipics/_wiki.png" />
- carefully melt a little of the <a href="https://en.wikipedia.org/wiki/Sulfur" target="_blank">S</a> <img
src="../scipics/_wiki.png" />, and pour it into water
- compare reactivity of <a href="https://en.wikipedia.org/wiki/Magnesium" target="_blank">Mg</a> <img src="../scipics/_wiki.png" />
and <a href="https://en.wikipedia.org/wiki/Calcium" target="_blank">Ca</a> <img src="../scipics/_wiki.png" /> with water, weak
acids, strong acids, etc.
- use the Mg, Ca, or some <a href="https://en.wikipedia.org/wiki/Aluminum" target="_blank">Al</a> <img src="../scipics/_wiki.png" />
to reduce Cu<sup>2+</sup> or Co<sup>2+</sup>
- catalytically decompose household <a href="https://en.wikipedia.org/wiki/Hydrogen_peroxide"
target="_blank">H<sub>2</sub>O<sub>2</sub></a> <img src="../scipics/_wiki.png" /> with the <a
href="https://en.wikipedia.org/wiki/Manganese_dioxide" target="_blank">MnO<sub>2</sub></a> <img src="../scipics/_wiki.png"
/>, and experiment with <a href="https://en.wikipedia.org/wiki/Oxygen" target="_blank">O<sub>2</sub></a> <img
src="../scipics/_wiki.png" />
<u>Things <em>not</em> to do (until you're more experienced):</u>
- don't mix the MnO<sub>2</sub> with the HCl
- don't mix the <a href="https://en.wikipedia.org/wiki/Ammonium_chloride" target="_blank">NH<sub>4</sub>Cl</a> <img
src="../scipics/_wiki.png" /> with either acid
- don't burn the S (toxic gases, UV destroys your retinas)
- burn the Mg (supervision, don't look directly at it)
- don't mix the <a href="https://en.wikipedia.org/wiki/Potassium_nitrate" target="_blank">KNO<sub>3</sub></a> <img
src="../scipics/_wiki.png" /> with the H<sub>2</sub>SO<sub>4</sub>
- use the <a href="https://en.wikipedia.org/wiki/Carbon" target="_blank">C</a> <img src="../scipics/_wiki.png" />, S, and
KNO<sub>3</sub> to make <a href="https://en.wikipedia.org/wiki/Black_powder" target="_blank">black powder</a> <img
src="../scipics/_wiki.png" /> (unless supervised)
- use the KNO<sub>3</sub> and <a href="https://en.wikipedia.org/wiki/Sucrose" target="lank">sucrose</a> <img
src="../scipics/_wiki.png" /> (table sugar) to make a smoke mixture (supervised)
I recommend reading through the paperback textbook. Reactions are fun, but knowing how to predict them is better. Stay safe, and enjoy the new
reagents!
[edit]
Since I didn't demonstrate how corrosive H<sub>2</sub>SO<sub>4</sub> is; your flesh would be the sponge:<iframe sandbox
width="560" height="315" src="//www.youtube-nocookie.com/embed/F5jfRjzXLbE?rel=0" frameborder="0" allowfullscreen></iframe>
<strong>Antiswat</strong>, I gave him the acids, with a short safety lecture/demonstration and his father's approval. 
[edited to appease the anti-nanny faction]
[Edited on 7/26/13 by bfesser]
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woelen
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Why not things to do? This sounds like the nannies we hear around us everywhere!
I would say. Do those things, but be warned. There is some danger involved. Toxic gases are produced, reactions can be violent. So take safety
measures. Use small amounts of chemicals, do the experiments outside and do not do them near large amounts of flammable materials.
Actually, making some Cl2 can be very interesting. Seeing a colored gas for the first time is quite special. Seeing the incredibly bright flame of
magnesium is spectacular. Just don't look at it for a long time! Brief exposure does not kill your eyes.
So my advice is not to completely steer away from the more dangerous and spectacular experiments, but to read a lot about them, try to obtain a real
understanding and try to obtain an idea of the risks involved. Then you are prepared to do the experiments on a small scale, outside. With time and
better understanding you will get to the level that you can scale up things in order to make your own chemicals.
There are only few things which you really should steer away from and that is from extremely unstable compounds which can explode without reason (e.g.
acetone peroxide, nitrogen chloride) or exceedingly toxic compounds with long term effects (e.g. arsenic compounds, some organics, phosgene).
Just read, read and read...
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ElizabethGreene
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Hello.
Congratulations on getting into Chemistry. It's lots of fun.
First, some book recommendations.
I got "E-Z Chemistry" from Barron's Publishing from my local library. It covers most of what's in a high school chemistry course. There is some math
in it, but if you want to understand the experiments you are doing, it's great.
The joy of chemistry : the amazing science of familiar things (Cathy Cobb) was at the same library. It had some cool experiments in it.
The Library section of this site has a lot of books too. Some of them will be way over your head. Don't feel bad, they are over my head too.
Now, experiments!
All Atoms have electrons. The atoms share electrons with other atoms to bond together and form molecules. A lot of metals, including Iron and
Copper, can share different numbers of electrons. In this experiment, you can see two different share numbers (These are called "oxidation states")
of Iron.
You need:
Steel Wool
Sulfuric Acid
Hydrogen Peroxide (The kind from the drugstore you use on cuts and scrapes.)
DO THIS OUTSIDE. You don't want to breathe the fumes.
Place some Steel Wool in a clear heat resistant container and add a small amount of Sulfuric Acid and water. As the acid attacks the iron, you should
see the clear solution change color. You can heat this up to make it go faster, or you can let it react for a few days. If all the steel wool
dissolves, add more. Once the reaction finishes, meaning that it stops bubbling and changing color, you'll have Ferrous Sulfate.
Now the cool part. Add some hydrogen peroxide. Add it slowly, as it heats up and you don't want it to boil all over your driveway. Your solution
will change color. This is from the hydrogen peroxide "oxidizing" the Ferrous Sulfate. This makes Ferric Sulfate.
Filter off the undissolved steel wool and keep the liquid. Put it somewhere safe where all the water can evaporate away. Once it dries, put it in a
container marked
"Iron(III) sulfate - Fe2(SO4)3
Poisonous - Do not eat"
Go read the MSDS: (This is a great habit to get into.) www.sciencelab.com/msds.php?msdsId=9924046
You can do this same reaction with Hydrochloric acid and steel wool to make Iron(II) and Iron(III) Chloride. Remember to read the MSDS!
Have fun!
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