Thanks for the great videos, and for the book, Illustrated Guide to Home Chemistry. Is there a method one can use to concentrate the resulting 5 Molar Hydrochloric to a 12 Molar Solution? Please correct if necessary - If you start with 5mol/L Solution of pure HCL and distilled water off until you had approx. 420 mL of Solution, wouldn't the final molarity of the HCL be 12 Mol/L, or about 50% concentration? Thanks 1x10^6! (1,000,000)
unless reagent grade HCI dose not react with aluminum this does not work. the distilled water container contained 80 ml of ???? the muratic acid container still reacted with aluminum and the reagent grade hci did not
@Zanragnar You are correct in saying it will dilute the acid, however, the purpose is to eliminate impurities often found in technical grade HCl acid.
So you are left with, as he said, two solutions of 5.1 M HCl acid from the original 10.2 M solution.
can i make pure ammonia(28-30%) or concentrated hydrochlorid acid (37,5%) by bubbling anhydrous ammonia gas or hydrogen chloride gas respectively into a water container?
Would you be able to accelerate this process if you placed your two containers into a home vacuum-seal container and evacuated said container? Of course you would be concerned with pulling HCl gas into your pump during the initial vacuum, but I bet the quantity would be small.
I followed the instructions in the video, I started with Muriatic Acid which contained 31.45% Hydrochloric Acid. After a few days over two weeks I expect to have 5.1 molar reagent grade HCl, but I'm wondering what that resulting percentage of concentration the distilled Tupperware container is going to contain of HCl. Is it between 36-38%?
If you started with 100ml of technical grade on your emitter and 50ml in your collector, wouldn't you get 5.1M in your emitter and 10.2 in your collector? Seeing as the volume is half so the concentration would be double with the same vapor pressure.
No, that's not how equilibrium and vapor pressure work. Regardless of the volumes in the two vessels, at equilibrium the concentration will be the same in both.
I would like to know what concentration of HCI is generally considered the common or typical concentration for "concentrated" HCI. I've come across 1N and 10N concentrate and 37% solution (~12M) reagent. I'm looking for the most typical concentration if there is such a thing. Thanks for any tip!
@god0fgod it would chemically burn your skin and spread if untreated. if you spill hydrochloric acid on your skin, immediately rinse with water for at least 5-15 minutes depending on the severity of the burn. if the burn is severe get medical attention immediately.
Ok, so I guess distilling would be the only way to get 32 to 37%? when distilling can you start with 32% on both sides for faster results? Do you need to start with distilled?
I have 32% reagent grade Hydrochloric acid. I'm trying to get a 20.2% HCL, 29.8% H2O and 50%Alcohol mixture. Would it be possible to use this method by adding x% (I guess 50%) distilled water and 99.9% alcohol in the reagent jar? Maybe I can get to 20.2% HCL after doing this twice. Would this be the same as starting out with 40.4% HCL?
The 32% is m/m. 100 grams of the solution contains 32 grams of HCl. Ordinarily alcohol (ethanol and isopropanol, anyway) mixtures are v/v. Combining 100 mL of water with 100 mL of absolute ethanol or isopropanol yields a 50% v/v mixture. Unfortunately, volumes aren't additive. That is, mixing 100 mL of each doesn't give you 200 mL of solution. Also, the water/alcohol solution is less dense than water or the HCl solution, so the m/m percentage of HCl changes.
Never thought this would be so simple, Ive always thought on distillation. The good thing about science is that there is always someone more intelligent and clever than you, and you get to learn very usefull things! Thank you.
HCl forms an azeotrope at 20.2% HCl. If you distill 31.45% hydrochloric acid, you'll drive off HCl gas until the concentration drops to 20.2%. You can route that gas into distilled water to produce any concentration of hydrochloric acid you wish, until it reaches saturation at just under 40% HCl. Of course, that leaves you with a lot of waste 20.2% acid.
i know this is a pretty morbid sounding question when you think about it, but i'm asking it more so i dont purify the Hydrochloric acid to the point that it's borderline weapons grade haha xD
anyway, once i've made the hydrochloric acid, i know there's a few other chemicals in the compound that dilute it..how would i get those out? how would i test the percent of pure HCL acid and at what percent does it become HIGHLY highly corrosive, cuz i've seen 10% on aluminum foil
Placing in one container a mixture of sulfuric acid,and potassium nitrate, and a separate container of distilled water,both sealed in a larger container.
Would that produce nitric acid in the distilled water?
If so,what should the ratio of potassium,and sulfuric be?
Nitric acid is easy to buy, although you'll have to pay a hazardous shipping surcharge. I order it from Elemental Scientific for $10 or so per pint bottle. They can ship up to eight bottles for one hazardous shipping surcharge.
@TheHomeScientist Does nitric acid decompose over time? I don't know much about chemistry but doesn't it decompose into nitrogen dioxide oxygen and water?
Depends on the concentration and purity. Typical 68% or 70% concentrated nitric acid is reasonably stable, but does eventually assume a yellowish color caused by free nitrogen oxides. Some discoloration is normally no cause for concern.
Too bad my local home depot stopped selling Muratic acid. They replaced it with a phosphoric acid based cleaner for cleaning brick. It also 2.5 times as expensive.
Fred Myer's sells some "green" low fume Muratic acid, which probably is either just dilute or has some stupid additive that would make me need to distill it!
A quick warning regarding hydrochloric acid and plastic bottles as shown in this video. The HCl gas can diffuse through the plastic and escape into the surrounding air. If you store those bottles anywhere near things made of iron or steel (like tools), you will find they start rusting like crazy. Store the bottle in a well ventilated place far away from anything you care about.
it came from that friendly place a*e is the place but we dont want to say that on line haha anyway it said muratic acid for cleaning bricks swinmming pool use etc.. it says(hydrocloric acid) 20 Baume (31.45) on the side by the skull and cross bones. s*nbe*lt chemical company (mispelled for law sue etc..) but we are sure you know what we were typing. Anyway we are going to watch the video again and try again Thanks fr all your answers VERY FAST responses Joseph T fly2000jtb.
well we checked and the distilled water is still distilled water?we put a soda tab in a pyrex custard glass and it did nothing, so we put the yellow contaminated into one and it started to eat it. the wild thing is this we put some from the original container of muratic acid and it started to eat the soda tab way faster than the sample that was in the test tub? anyway did we hear it wrong or did we take it out to early you said in a email over night that the video was wrong? ours was not strong
I have no idea what you did wrong. Was the original acid the 31.45% stuff? That's the most concentrated form sold in hardware stores, but they also sell HCl of lower concentrations, which may not work as well. After even an hour, there should be significant HCl in the container that started as distilled water.
Thanks for the fast answer, so when it is done in a week or so the distilled water container should be clear because it is the transfer container and the iron wont come along for the ride/ Hope it is the way it works dont want to sound like an idiot hahah Joseph T fly2000jtb
It shouldn't take a week, although I think I did let it equilibrate that long when I was shooting the video. It should equilibrate overnight.
Yes, the distilled water will appear unchanged, clear and colorless.
You can use different amounts of distilled water to get different concentrations of pure acid. For example, if you start with 1 L of 10M acid and 0.1 L of distilled water, that 10 moles of HCl ends up evenly distributed over 1.1L, so the final concentration is about 9.1 M.
@charliewecker I think the reason he said Howes or Lome Depot is that earlier in the video he said Lowes or Home Depot. He probably started to say Home Depot but his mindset made him say Lowes first, hence Howes.
us again, well we tryed to reproduce the purify hydrochloric acid thing in plastic containers. is it normal for the acid to be yellow, also is it normal for the distilled water to raise a fog like cloud when set next to the muratic acid? my wife said; look at the small misty looking puffs of smoke!! I said yes it looks like the acid is trying to get to the water hahaha. Anyway is that normal? Joseph T fly2000jtb.
Technical grade HCl often has iron impurities that give it a yellow color. The concentrated acid outgasses HCl vapor. If the air is humid, the HCl gas can combine with the water vapor to produce tiny droplets of HCl solution, which appear as a fog.
hi it is us again we were wondering what acid will eat rubber tires? all those tires out there just waiting to catch fire and smoke the sky up!! Why cant we just use a acid to eat it up like the hydro acid does to aluminium? Just wondering dont know much about acids but we are learning watching your series haha kepp posting them Joseph T fly2000jtb
forget what that is called but we do that all the time whoes lomedepot GREAT brain fart but made the video forgot to say that in the last video response Joseph T fly2000jtb
Love the series! I have sucessfuly concentrated ammonium hydroxide from the regular store strenght to maximum (35%) by heating the solution and catching and redisolving the gas in distilled water. I used a hot water bath for the gas source and a chilled recieving solution. Could you do the same thing here? Gently heat your "store grade" HCL solution in a water bath and drive off the HCL gas. Then redisolve in chilled distilled water using a bubble stone. Faster & higher concetrations possible.
Yes, absolutely, although you'll use up a lot of technical-grade acid. HCl forms a high-boiling azeotrope at 20.2%, so a gallon of the 31.45% stuff will yield only about a liter of 37% reagent-grade acid using this method.
Not necessarily. The most common reason for a yellow color is the presence of iron. It depends on how much of solution you're looking through, but a concentration of 0.01 M or even 0.001 M iron can lend a yellow color. I'd expect your acid to be perfectly acceptable for routine use, such as syntheses. I'd use reagent-grade acid for quantitative analysis or other critical tasks.
When the system equilibrates, the concentration of HCl in the original acid container and the distilled water container will be identical. So, if you start with equal amounts of 31.45% HCl and distilled water, both containers will contain acid at half that concentration (less a tiny amount for the gas left in the large container). If you want 10% HCl, you can use twice as much distilled water as 31.45% acid, e.g., 100 mL of 31.45% acid and 200 mL of water.
No. Aqua regia is actually a mixture of concentrated HCl (>36%) and concentrated nitric acid (>67%). For best results, you really should use fuming HCl and fuming HNO3.
I've never tried making up aqua regia with dilute acids. I suspect you'd get some results, but nowhere near what you wanted. Also aqua regia is very short-lived; you need to make it up immediately before using. I'm not sure if the dilute version would be more or less stable.
I've done a bit more research since this post, and have found many people simply combine sodium nitrate and muriatic acid to make poor man's AR. It's effective, but I imagine like you said it wouldn't quite produce the results hoped for. I will prolly try the poor man's AR to begin with, just to see how well it works. I don't think I want to make true AR, considering the price of mats or even the amount of work and danger involved in the making of conc HNO3 or conc HCl.
Concentrated HCL with a nitrate salt may do what you're looking for. What really matters for stuff like reacting metallic gold is that the nitric acid (which you produce on the fly) oxidizes the gold and the chloride ions react with those gold ions to complex them. That drives equilibrium to favor oxidizing more gold, so the reaction continues.
Certainly most of the aqua regia that's been used industrially has been very impure.
Certainly. Supermarket ammonia is usually about 6 molar, so using equal amounts of it and distilled water would give you pure 3 molar ammonia (along with the same amount of impure 3 molar ammonia).
You could instead use much less distilled water to get a higher concentration in the pure ammonia. For example, 275 mL of the impure stuff with 25 mL of water would yield about 5.5 molar product.
im having trouble understanding why you would want to go down in molarity to concentrate it more.. If the muriatic acid was around 10 Molar wouldnt that make it more concentrated, cuz it has more solute per liter then the 5 molar reagent grade HCl? im sorry if this is a silly question.. just trying to understand.
We don't *want* to reduce the molarity. We want to purify technical-grade acid to get reagent-grade acid. We accept the reduction in molarity in return for getting purer acid.
Sure, if you have the necessary equipment and are comfortable working around boiling hydrochloric acid, distillation will let you get very pure 20.2% acid. But for most purposes more dilute acid is fine and using the method in the video is a very easy way to get very pure acid at reasonable concentrations.
Hey Home scientist will this method concentrate it or just purify it?and another question I have around 5 % hcl using your method the concentration I will get can be 35 percent purity?.if it is needed I can repeat the process by adding new hcl in the unpure hcl container
The concentration in both containers is the same once equilibrium is reached. If you start out with 100 mL of 10 M acid and 100 mL of water, you end up with 100 mL of 5 M acid in each container. You can keep replacing the impure acid with more 10 M acid and you'll eventually end up with both containers holding acid that's a fraction under 10 M.
How about adding some (just SOME) sulphuric acid in the first container? maybe the reciving container would get higher concentration of hydrochloric acid than the first container ????
Yes, for most purposes the technical grade HCl works fine. Because of the production process, the only contaminants normally present are those in the tap water used to absorb the HCl gas. Depending on where it's made, that tap water may be pretty pure.
The two containers of liquid achieve equilibrium when the concentration of HCl in both containers is identical. So, for example, if you started with 100 mL of 31% HCl and 100 mL of distilled water, you'd end up with both containers being 15.5% (less some loss to the air). With 100 mL of 31% HCl and 1 mL of distilled water, both containers would be very slightly less than 31%.
I have tried this on a toilet cleaner that says had 20% HCL but after a month I found that the distilled water has no change in weight and ph. help me please?
That's very strange. HCl is very volatile and should have outgassed from the toilet cleaner and been absorbed by the distilled water. I used relatively pure muriatic acid from the hardware store. Perhaps there's something in the toilet cleaner that's interfering.
I don't know. I'm not familiar with that compound, although it sounds like a quaternary ammonium surfactant. A 20% HCl solution should have a noticeable sharp HCl odor from outgassing. Does your toilet cleaner have that odor?
You can still get pure hydrochloric acid, because HCl has a very high vapor pressure and H2SO4 a very low vapor pressure. All of the sulfuric acid will remain in the first container, and the second container will contain pure hydrochloric acid.
Read the other comments. You can get it up to about 20% HCl by boiling off water. Alternatively, you can use a larger volume of technical acid and a smaller volume of water to get pure acid of higher molarity.
Exactly. HCl and water form a low-boiling azeotrope at about 20.2% HCl. If you boil acid of a lower concentration, water boils off until the HCl concentration rises to 20.2%. If you boil more concentrated acid, HCl boils off until the concentration falls to 20.2%.
Yes. The exact type and percentage of impurities in reagent grade chemicals varies depending on the chemical. Technically, a reagent-grade chemical is one that has been assayed to test for the types of impurities common to that chemical (and production method, if different methods are used). The assay lists the impurities and their percentages. An ACS reagent-grade chemical is one that the ACS has published standards for and that meets those standards.
Sure, at the cost of using a lot more raw acid. The HCL vapor pressure in the two containers reaches equilibrium when the molarity of the acid in the two containers is the same.
oh! i did not catch that i though it was just the waters natural ability to absorb gasses which brings me to another question after you let it sit can you put it in the fridge so that way the water could better absorb the gasses?
At equilibrium, the molarity of the acid in both containers will be identical, regardless of the volume of liquid in each container. Think of it this way: if you start with 100 mL of 10 M acid and add 100 mL of water, you end up with 200 mL of 5 M acid. That's true whether you add the water directly to the acid or keep it in a separate container. Same if you add only 11 mL of water. You end up with 111 mL of 9 M acid, whether you add the water directly to the acid or use a second container.
No. Typical soil contains very low nitrate concentrations unless it has recently been heavily treated with nitrate fertilizer. You're thinking about the way potassium nitrate was originally extracted from soil and straw that had been soaked with urine. They had to treat a lot of soil to get a little bit of saltpeter. In practical terms, this isn't a reasonable way to get nitrates. It's much easier to obtain them from other sources such as cold packs, fertilizer, stump remover, etc.
No, it's not possible. Depending on the type of wood burned, wood ash contains varying amounts of sodium and potassium carbonates and hydroxides with smaller amounts of sulfates and other salts. Like most nitrates, potassium nitrate is a strong oxidizer, and wouldn't survive the flames without reacting with the fuel.
Hello, TheHomeScientist, i have a question, can hydrogen peroxide be concentrated in a similar way? Not exactly the same way, but similar, i would have two containers, one with dilute hydrogen peroxide and other with anhydrus calcium chlorhidre.
I don't know. I've never tried it. But you'd use up a lot of anhydrous CaCl2, because drugstore H2O2 is about 97% water, and the dehydration would take forever.
It's easier just to buy more concentrated H2O2. You can buy 6% or 12% H2O2 from a beautician supply store, or just search google for "food grade hydrogen peroxide" for a local source of 30% or 35% H2O2.
I actually have access to 50% hydrogen peroxyde, but i want it up to at least 80% as it will be suitable for liquid hobby rocket propellant. I was actually wondering if H2O2 was reactive with calcium chlorhidre. boiling off the water of H2O2 just decomposes it..
Please don't do that, even if you can somehow get your hands on some. Even 30% H2O2 is a dangerous oxidizer, let alone 50%. And with 80%, you might as well be dealing with nitroglycerin. The 80% stuff will oxidize stuff spontaneously that you don't even think of as combustible. Bad accidents are commonplace with high percentage H2O2.
not to worry, i know all of the dangers involved, but i must tell you is not an explosive by itself. I know that it may generate the dangerous organic peroxides or just set things on fire with only the touch of it. But I know you know a more than me, so ok, i'll stay away of it.
I've seen that before. my teacher was pouring about 85% H2O2 on a cotton. a few minutes later, the cotton ignites by its self. its shock the whole class.
I've read about that method on a forum once. Someone took 32% H2O2 and put it in a dessicator with CaCl2 as the hygroscopic. He said it didn't work, probably because O2 is released from the H2O2 (forming H2O) over time, so he ended up with less concentrated H2O2.
You floored me when you just put the acid and water containers in the big container and let them sit to get the high grade acid!!! Thats great!! On of the things I love about chemistry is that it gets you to think and solve problems
Yeah, it wasn't until my first-year organic prof explained what the word "elegant" really meant that I got it. I thought elegant meant fashionable, expensive, whatever. What it really means is simple but effective. An elegant synthesis requires the fewest possible steps with the simplest possible reagents at room temperature, but provides yields near theoretical. As a means of purifying acid, this process definitely meet the requirements for being called elegant.
You can concentrate hydrochloric acid to 20.2% (w/w) by boiling. HCl forms a negative azeotrope with water at 20.2% HCl by mass. If you boil a hydrochloric acid solution that's less than 20.2% concentration, water will boil off until the solution reaches 20.2%. If you boil hydrochloric acid that's greater than 20.2% HCl by mass, HCl will boil off until the concentration reaches 20.2%.
If I stock up on muriatic acid, and store it in a plastic mini-shed outside in my backyard, will the seasonal variations in temperature cause it to degrade faster? I live in the northern tier of the U.S. and rarely is it 20º C often.The shed supposedly does keep out rain and moisture though.
can i distil technical grade HCl to purufy it?
nikola96uf 21 hours ago
My HCl solution is green. What is this, and what do I do about it?
elementcollector1 1 week ago
Thanks for the great videos, and for the book, Illustrated Guide to Home Chemistry. Is there a method one can use to concentrate the resulting 5 Molar Hydrochloric to a 12 Molar Solution? Please correct if necessary - If you start with 5mol/L Solution of pure HCL and distilled water off until you had approx. 420 mL of Solution, wouldn't the final molarity of the HCL be 12 Mol/L, or about 50% concentration? Thanks 1x10^6! (1,000,000)
daviddanielgraham 1 week ago
Hi, thanks for the video. The result that is very purified HCL can it be regarded as a 'food grade' HCL?
cyberlightbeing 2 weeks ago
would adding heat speed the process?
carlip 2 weeks ago
unless reagent grade HCI dose not react with aluminum this does not work. the distilled water container contained 80 ml of ???? the muratic acid container still reacted with aluminum and the reagent grade hci did not
cybob43 2 weeks ago
this is a great video!! thanks heaps!!
keglimp 2 weeks ago
Comment removed
Salmagundiii 2 months ago
Doesn't this dilute the acid, as the HCl is being split between the two containers?
Zanragnar 4 months ago
@Zanragnar You are correct in saying it will dilute the acid, however, the purpose is to eliminate impurities often found in technical grade HCl acid.
So you are left with, as he said, two solutions of 5.1 M HCl acid from the original 10.2 M solution.
TerminalRhinoVirus 2 months ago
Hmm.... Ot does not burn on my skin but tastes like salt
Tutorializer100 5 months ago
and what amount of both and water?
MrPaneKe 6 months ago
can i make pure ammonia(28-30%) or concentrated hydrochlorid acid (37,5%) by bubbling anhydrous ammonia gas or hydrogen chloride gas respectively into a water container?
MrPaneKe 6 months ago
does it works for impure hydrochloric acid?
stevenliang96 6 months ago
couldnt i just take my 14% hcl and throw it in the freezer overnight? then in the morning what is not frozen would be the purified hcl right?
dmaryniak 7 months ago
couldnt i just take my 14% hcl and throw it in the freezer overnight? then in the morning what is not frozen would be the purified hcl right?
dmaryniak 7 months ago
Hoes or Lome Depot....What the?! lol xD
utube8353 7 months ago 2
Would you be able to accelerate this process if you placed your two containers into a home vacuum-seal container and evacuated said container? Of course you would be concerned with pulling HCl gas into your pump during the initial vacuum, but I bet the quantity would be small.
jaidormi 7 months ago
I followed the instructions in the video, I started with Muriatic Acid which contained 31.45% Hydrochloric Acid. After a few days over two weeks I expect to have 5.1 molar reagent grade HCl, but I'm wondering what that resulting percentage of concentration the distilled Tupperware container is going to contain of HCl. Is it between 36-38%?
myers8 8 months ago
is this the same as concentrated hydrochloric acid?
jackn8r 8 months ago
could i purify 10%HCL by this method? and if yes; what would the percentage then be?
hamsterboy13 9 months ago
Hoe's or Lome Depot LOL xD
poopieman123456789 9 months ago
Could you distill muriatic acid w/CaCl2 and a small amount of water in the receiving flask (to dissolve HCl gas before azeotrope comes over)?
ChemCrazy81 9 months ago
I saw a video with you on Amazon,; I loved it. I am glad I found your channel I'm definitely subscribing.
BoaC2323 9 months ago
What is the PH diff. between the technical grade 30-32% acid and the reagent grade 38-39%+ acid?
ABOlsen69666 10 months ago
@ABOlsen69666
Not much. The pH of 31.45% (10 molar) acid is -1.0. The pH of 36% to 38% is -1.1.
TheHomeScientist 10 months ago
If you started with 100ml of technical grade on your emitter and 50ml in your collector, wouldn't you get 5.1M in your emitter and 10.2 in your collector? Seeing as the volume is half so the concentration would be double with the same vapor pressure.
TakronRust 10 months ago
@TakronRust
No, that's not how equilibrium and vapor pressure work. Regardless of the volumes in the two vessels, at equilibrium the concentration will be the same in both.
TheHomeScientist 10 months ago
Howes or Lome Depot... What? ^_^
DactaDork 10 months ago
Hoes or lome deopt, haha. Nice videos! Thank you!
masyn92 10 months ago
I would like to know what concentration of HCI is generally considered the common or typical concentration for "concentrated" HCI. I've come across 1N and 10N concentrate and 37% solution (~12M) reagent. I'm looking for the most typical concentration if there is such a thing. Thanks for any tip!
monkeylogique 10 months ago
Couldn't you just Vomit in a bucket and distill that?
TheNarath 11 months ago
Thanks, I appreciate these videos!
PyroPortrayal 1 year ago
Do both containers have the same concentration of hcl? Can we combine them?
Cheenman11 1 year ago
What would pure hydrochloric acid do to your skin?
god0fgod 1 year ago
@god0fgod it would chemically burn your skin and spread if untreated. if you spill hydrochloric acid on your skin, immediately rinse with water for at least 5-15 minutes depending on the severity of the burn. if the burn is severe get medical attention immediately.
benscardude 1 year ago
Ok, so I guess distilling would be the only way to get 32 to 37%? when distilling can you start with 32% on both sides for faster results? Do you need to start with distilled?
collura1 1 year ago
I have 32% reagent grade Hydrochloric acid. I'm trying to get a 20.2% HCL, 29.8% H2O and 50%Alcohol mixture. Would it be possible to use this method by adding x% (I guess 50%) distilled water and 99.9% alcohol in the reagent jar? Maybe I can get to 20.2% HCL after doing this twice. Would this be the same as starting out with 40.4% HCL?
collura1 1 year ago
@collura1
The 32% is m/m. 100 grams of the solution contains 32 grams of HCl. Ordinarily alcohol (ethanol and isopropanol, anyway) mixtures are v/v. Combining 100 mL of water with 100 mL of absolute ethanol or isopropanol yields a 50% v/v mixture. Unfortunately, volumes aren't additive. That is, mixing 100 mL of each doesn't give you 200 mL of solution. Also, the water/alcohol solution is less dense than water or the HCl solution, so the m/m percentage of HCl changes.
TheHomeScientist 1 year ago
can you use the same purification process for sulfuric acid?
adjuvants12780 1 year ago
Never thought this would be so simple, Ive always thought on distillation. The good thing about science is that there is always someone more intelligent and clever than you, and you get to learn very usefull things! Thank you.
kaskito 1 year ago
I wish someone would make a Hydrochloric acid saftey video, for clean up, proceger, what gear is best to use, etc.
bob84676 1 year ago
HCl forms an azeotrope at 20.2% HCl. If you distill 31.45% hydrochloric acid, you'll drive off HCl gas until the concentration drops to 20.2%. You can route that gas into distilled water to produce any concentration of hydrochloric acid you wish, until it reaches saturation at just under 40% HCl. Of course, that leaves you with a lot of waste 20.2% acid.
TheHomeScientist 1 year ago
@TheHomeScientist
what variables cause higher or lower concentrations? and can you do this with other acids?
pyrosparkerII 1 year ago
@TheHomeScientist
i know this is a pretty morbid sounding question when you think about it, but i'm asking it more so i dont purify the Hydrochloric acid to the point that it's borderline weapons grade haha xD
anyway, once i've made the hydrochloric acid, i know there's a few other chemicals in the compound that dilute it..how would i get those out? how would i test the percent of pure HCL acid and at what percent does it become HIGHLY highly corrosive, cuz i've seen 10% on aluminum foil
synyst3rrev 1 year ago
How could one concentrate HCl acid form 31.45 % HCl?
bendope1 1 year ago
what is the shortest time the proses can take
zap1726 1 year ago
Just a question.
Using your method to obtain a different acid.
Placing in one container a mixture of sulfuric acid,and potassium nitrate, and a separate container of distilled water,both sealed in a larger container.
Would that produce nitric acid in the distilled water?
If so,what should the ratio of potassium,and sulfuric be?
BillyCumber 1 year ago
@BillyCumber
No.
TheHomeScientist 1 year ago
Comment removed
98JMA 1 year ago
Is there a similar process to get >= 6M HNO3?
1RadicalOne 1 year ago
@1RadicalOne
No, this works only with HCl.
TheHomeScientist 1 year ago
So, is there any way at all to acquire at least low-grade reagent grade Nitric acid?
I am not a chemist, so I have no licensing to purchase such material.
(Which is ironic, because I do have a license to purchase reactor-grade uranium.) ;)
1RadicalOne 1 year ago
@1RadicalOne
Nitric acid is easy to buy, although you'll have to pay a hazardous shipping surcharge. I order it from Elemental Scientific for $10 or so per pint bottle. They can ship up to eight bottles for one hazardous shipping surcharge.
TheHomeScientist 1 year ago
Really? At 6 or greater molar?
1RadicalOne 1 year ago
@1RadicalOne
Yeah, really. Elemental sells ACS Reagent grade 70% nitric acid (~ 16 M).
TheHomeScientist 1 year ago
Wow.
Thank you. :)
1RadicalOne 1 year ago
@TheHomeScientist Does nitric acid decompose over time? I don't know much about chemistry but doesn't it decompose into nitrogen dioxide oxygen and water?
yellowmetalcyborg 1 year ago
@yellowmetalcyborg
Depends on the concentration and purity. Typical 68% or 70% concentrated nitric acid is reasonably stable, but does eventually assume a yellowish color caused by free nitrogen oxides. Some discoloration is normally no cause for concern.
TheHomeScientist 1 year ago
@TheHomeScientist
2 questions:
1 - can i add more distilled water instead of 100ml?
2 - once the distilled water turns to pure hydrochloric acid, can i use that pure acid to make more of it?
moctezuma112 1 year ago
Too bad my local home depot stopped selling Muratic acid. They replaced it with a phosphoric acid based cleaner for cleaning brick. It also 2.5 times as expensive.
Fred Myer's sells some "green" low fume Muratic acid, which probably is either just dilute or has some stupid additive that would make me need to distill it!
alancj05 1 year ago
A quick warning regarding hydrochloric acid and plastic bottles as shown in this video. The HCl gas can diffuse through the plastic and escape into the surrounding air. If you store those bottles anywhere near things made of iron or steel (like tools), you will find they start rusting like crazy. Store the bottle in a well ventilated place far away from anything you care about.
ib9rt 1 year ago
this guy is the MAN! so dang helpful
CAP118 1 year ago
@ZED74
They're polypropylene, which is resistant to concentrated HCl.
TheHomeScientist 1 year ago
it came from that friendly place a*e is the place but we dont want to say that on line haha anyway it said muratic acid for cleaning bricks swinmming pool use etc.. it says(hydrocloric acid) 20 Baume (31.45) on the side by the skull and cross bones. s*nbe*lt chemical company (mispelled for law sue etc..) but we are sure you know what we were typing. Anyway we are going to watch the video again and try again Thanks fr all your answers VERY FAST responses Joseph T fly2000jtb.
fly2000jtb 1 year ago
well we checked and the distilled water is still distilled water?we put a soda tab in a pyrex custard glass and it did nothing, so we put the yellow contaminated into one and it started to eat it. the wild thing is this we put some from the original container of muratic acid and it started to eat the soda tab way faster than the sample that was in the test tub? anyway did we hear it wrong or did we take it out to early you said in a email over night that the video was wrong? ours was not strong
fly2000jtb 1 year ago
@fly2000jtb
I have no idea what you did wrong. Was the original acid the 31.45% stuff? That's the most concentrated form sold in hardware stores, but they also sell HCl of lower concentrations, which may not work as well. After even an hour, there should be significant HCl in the container that started as distilled water.
TheHomeScientist 1 year ago
OH YEAH! You're getting some thumbs ups and a subscription :)
lexichronicle2 1 year ago
Thanks for the fast answer, so when it is done in a week or so the distilled water container should be clear because it is the transfer container and the iron wont come along for the ride/ Hope it is the way it works dont want to sound like an idiot hahah Joseph T fly2000jtb
fly2000jtb 1 year ago
@fly2000jtb
It shouldn't take a week, although I think I did let it equilibrate that long when I was shooting the video. It should equilibrate overnight.
Yes, the distilled water will appear unchanged, clear and colorless.
You can use different amounts of distilled water to get different concentrations of pure acid. For example, if you start with 1 L of 10M acid and 0.1 L of distilled water, that 10 moles of HCl ends up evenly distributed over 1.1L, so the final concentration is about 9.1 M.
TheHomeScientist 1 year ago
hahahahah Hoes or Lome Depot!!!!!! I love when that happens.
charliewecker 1 year ago
@charliewecker I think the reason he said Howes or Lome Depot is that earlier in the video he said Lowes or Home Depot. He probably started to say Home Depot but his mindset made him say Lowes first, hence Howes.
FortNikitaBullion 1 year ago
us again, well we tryed to reproduce the purify hydrochloric acid thing in plastic containers. is it normal for the acid to be yellow, also is it normal for the distilled water to raise a fog like cloud when set next to the muratic acid? my wife said; look at the small misty looking puffs of smoke!! I said yes it looks like the acid is trying to get to the water hahaha. Anyway is that normal? Joseph T fly2000jtb.
fly2000jtb 1 year ago
@fly2000jtb
Technical grade HCl often has iron impurities that give it a yellow color. The concentrated acid outgasses HCl vapor. If the air is humid, the HCl gas can combine with the water vapor to produce tiny droplets of HCl solution, which appear as a fog.
TheHomeScientist 1 year ago
So did you ever figure out that bromine reaction?
FortNikitaBullion 1 year ago
@FortNikitaBullion
No. I haven't returned to it simply because I haven't had time and the dilute bromine solution I did produce was adequate for what I needed.
TheHomeScientist 1 year ago
hi it is us again we were wondering what acid will eat rubber tires? all those tires out there just waiting to catch fire and smoke the sky up!! Why cant we just use a acid to eat it up like the hydro acid does to aluminium? Just wondering dont know much about acids but we are learning watching your series haha kepp posting them Joseph T fly2000jtb
fly2000jtb 1 year ago
@fly2000jtb
None, so far as I know. I'm sure nitric acid would degrade them noticeably, but rubber is basically a hydrocarbon, and those are pretty inert.
TheHomeScientist 1 year ago
forget what that is called but we do that all the time whoes lomedepot GREAT brain fart but made the video forgot to say that in the last video response Joseph T fly2000jtb
fly2000jtb 1 year ago
@fly2000jtb
A Spoonerism, for the Reverend William Spooner, not the great 19th century Constitutional law expert, Lysander Spooner.
TheHomeScientist 1 year ago
Can't you just distill it?
FortNikitaBullion 1 year ago
@FortNikitaBullion
Sure, but HCl forms a high-boiling azeotrope with water at 20.2% HCl, so you can't get more concentrated than 20.2% by distillation.
TheHomeScientist 1 year ago
@FortNikitaBullion So just curious, why did you say Howes and Lome's Depot?
FortNikitaBullion 1 year ago
@FortNikitaBullion
Because my mouth and brain temporarily lost sync.
TheHomeScientist 1 year ago
Awesome someone who explains!!
MrKillermeatball 1 year ago
Love the series! I have sucessfuly concentrated ammonium hydroxide from the regular store strenght to maximum (35%) by heating the solution and catching and redisolving the gas in distilled water. I used a hot water bath for the gas source and a chilled recieving solution. Could you do the same thing here? Gently heat your "store grade" HCL solution in a water bath and drive off the HCL gas. Then redisolve in chilled distilled water using a bubble stone. Faster & higher concetrations possible.
ccronn 1 year ago
@ccronn
Yes, absolutely, although you'll use up a lot of technical-grade acid. HCl forms a high-boiling azeotrope at 20.2%, so a gallon of the 31.45% stuff will yield only about a liter of 37% reagent-grade acid using this method.
TheHomeScientist 1 year ago
now that was easy! great video too! do you have more videos out there? Joseph T FLY2000JTB
fly2000jtb 1 year ago
I have some 31.45% HCl(aq) (muriatic acid) but it's yellow. Does this mean it's very impure?
AHW214 1 year ago
@AHW214
Not necessarily. The most common reason for a yellow color is the presence of iron. It depends on how much of solution you're looking through, but a concentration of 0.01 M or even 0.001 M iron can lend a yellow color. I'd expect your acid to be perfectly acceptable for routine use, such as syntheses. I'd use reagent-grade acid for quantitative analysis or other critical tasks.
TheHomeScientist 1 year ago
@wsbh69
When the system equilibrates, the concentration of HCl in the original acid container and the distilled water container will be identical. So, if you start with equal amounts of 31.45% HCl and distilled water, both containers will contain acid at half that concentration (less a tiny amount for the gas left in the large container). If you want 10% HCl, you can use twice as much distilled water as 31.45% acid, e.g., 100 mL of 31.45% acid and 200 mL of water.
TheHomeScientist 1 year ago
Would the resulting acid be strong enough for use in creating aqua regia?
MalumSin 1 year ago
@MalumSin
No. Aqua regia is actually a mixture of concentrated HCl (>36%) and concentrated nitric acid (>67%). For best results, you really should use fuming HCl and fuming HNO3.
I've never tried making up aqua regia with dilute acids. I suspect you'd get some results, but nowhere near what you wanted. Also aqua regia is very short-lived; you need to make it up immediately before using. I'm not sure if the dilute version would be more or less stable.
TheHomeScientist 1 year ago
@TheHomeScientist
I've done a bit more research since this post, and have found many people simply combine sodium nitrate and muriatic acid to make poor man's AR. It's effective, but I imagine like you said it wouldn't quite produce the results hoped for. I will prolly try the poor man's AR to begin with, just to see how well it works. I don't think I want to make true AR, considering the price of mats or even the amount of work and danger involved in the making of conc HNO3 or conc HCl.
MalumSin 1 year ago
@MalumSin
Concentrated HCL with a nitrate salt may do what you're looking for. What really matters for stuff like reacting metallic gold is that the nitric acid (which you produce on the fly) oxidizes the gold and the chloride ions react with those gold ions to complex them. That drives equilibrium to favor oxidizing more gold, so the reaction continues.
Certainly most of the aqua regia that's been used industrially has been very impure.
TheHomeScientist 1 year ago
@MalumSin
Go here to goldrefiningforum..com
This is all you will ever need and its free!
Also you can check out my vid on how to make 50% nitric acid. You can use it to make AR that is better than poor mans.
metalicmario 1 year ago
Will it be possible to purify cheap supermarket cloudy ammonia using this method?
mewrox99 1 year ago
@mewrox99
Certainly. Supermarket ammonia is usually about 6 molar, so using equal amounts of it and distilled water would give you pure 3 molar ammonia (along with the same amount of impure 3 molar ammonia).
You could instead use much less distilled water to get a higher concentration in the pure ammonia. For example, 275 mL of the impure stuff with 25 mL of water would yield about 5.5 molar product.
TheHomeScientist 1 year ago
Would this method work for sulphuric acid?
MrEugenalicious 1 year ago
@MrEugenalicious
No, H2SO4 has a very low vapor pressure, and this purification method depends on the high vapor pressure of HCl.
TheHomeScientist 1 year ago
@TheHomeScientist
Thankyou.
Just looking for an easy way to produce nitric acid.
BillyCumber 1 year ago
im having trouble understanding why you would want to go down in molarity to concentrate it more.. If the muriatic acid was around 10 Molar wouldnt that make it more concentrated, cuz it has more solute per liter then the 5 molar reagent grade HCl? im sorry if this is a silly question.. just trying to understand.
barbarossaaaa 1 year ago
@barbarossaaaa
We don't *want* to reduce the molarity. We want to purify technical-grade acid to get reagent-grade acid. We accept the reduction in molarity in return for getting purer acid.
TheHomeScientist 1 year ago
@TheHomeScientist
oh i see..i really enjoy your videos. very informative
barbarossaaaa 1 year ago
LMAO I like the ending you can buy it howes or lomedepot what lol
c0ldelement 1 year ago
@c0ldelement
That's one of my few screw-ups that was clean enough to include in a video.
TheHomeScientist 1 year ago
@TheHomeScientist very nice it at a nice humorous touch to it
c0ldelement 1 year ago
Oh im sure a better way is to destill that stuff. you have a better concentration (about 20%) and it`s faster.
olympicfan2 1 year ago
@olympicfan2
Sure, if you have the necessary equipment and are comfortable working around boiling hydrochloric acid, distillation will let you get very pure 20.2% acid. But for most purposes more dilute acid is fine and using the method in the video is a very easy way to get very pure acid at reasonable concentrations.
TheHomeScientist 1 year ago
so if i try to purify the 5% stuff I will end up with 2,5% pure hcl?
discaras 1 year ago
Hey Home scientist will this method concentrate it or just purify it?and another question I have around 5 % hcl using your method the concentration I will get can be 35 percent purity?.if it is needed I can repeat the process by adding new hcl in the unpure hcl container
discaras 1 year ago
@discaras
The concentration in both containers is the same once equilibrium is reached. If you start out with 100 mL of 10 M acid and 100 mL of water, you end up with 100 mL of 5 M acid in each container. You can keep replacing the impure acid with more 10 M acid and you'll eventually end up with both containers holding acid that's a fraction under 10 M.
TheHomeScientist 1 year ago
@deamond666123
Sure, at the expense of lowering the concentration.
TheHomeScientist 1 year ago
How about adding some (just SOME) sulphuric acid in the first container? maybe the reciving container would get higher concentration of hydrochloric acid than the first container ????
adriiPortillo 1 year ago
@adriiPortillo
No, alas. That will have no effect.
TheHomeScientist 1 year ago
Can't you just use the technical grade in most experiments.
mewrox99 1 year ago
@mewrox99
Yes, for most purposes the technical grade HCl works fine. Because of the production process, the only contaminants normally present are those in the tap water used to absorb the HCl gas. Depending on where it's made, that tap water may be pretty pure.
TheHomeScientist 1 year ago
hey if i use 100 ml of 31% and 50 ml of distiled water would that give a higher concentration than if i used 100 ml of water?
jordehwa 1 year ago
The two containers of liquid achieve equilibrium when the concentration of HCl in both containers is identical. So, for example, if you started with 100 mL of 31% HCl and 100 mL of distilled water, you'd end up with both containers being 15.5% (less some loss to the air). With 100 mL of 31% HCl and 1 mL of distilled water, both containers would be very slightly less than 31%.
TheHomeScientist 1 year ago
I have tried this on a toilet cleaner that says had 20% HCL but after a month I found that the distilled water has no change in weight and ph. help me please?
yahoorif 2 years ago
That's very strange. HCl is very volatile and should have outgassed from the toilet cleaner and been absorbed by the distilled water. I used relatively pure muriatic acid from the hardware store. Perhaps there's something in the toilet cleaner that's interfering.
TheHomeScientist 2 years ago
@TheHomeScientist well its says that its contain: 20% Hydrochloric acid , and trimethyltallow ammonium chloride. thats all.
yahoorif 2 years ago
I don't know. I'm not familiar with that compound, although it sounds like a quaternary ammonium surfactant. A 20% HCl solution should have a noticeable sharp HCl odor from outgassing. Does your toilet cleaner have that odor?
TheHomeScientist 2 years ago
@TheHomeScientist yeah , its have a sharp odour.
yahoorif 2 years ago
I have no idea what the problem is.
TheHomeScientist 2 years ago
@TheHomeScientist yeah , anyway thanks for you help.
yahoorif 2 years ago
So what if your acid happens to be weaker than muriatic and is a mixture of sulfuric acid and HCl?
HazMatLabz 2 years ago
You can still get pure hydrochloric acid, because HCl has a very high vapor pressure and H2SO4 a very low vapor pressure. All of the sulfuric acid will remain in the first container, and the second container will contain pure hydrochloric acid.
TheHomeScientist 2 years ago
very nice. i usually synthesize my chems to save money so this is helpful.
TheBombBros 2 years ago
Any way to concentrate the pure acid?
coolliger 2 years ago
Read the other comments. You can get it up to about 20% HCl by boiling off water. Alternatively, you can use a larger volume of technical acid and a smaller volume of water to get pure acid of higher molarity.
TheHomeScientist 2 years ago
I thought boiling HCl made it weaker, or is this only in high concentrations?
coolliger 2 years ago
Exactly. HCl and water form a low-boiling azeotrope at about 20.2% HCl. If you boil acid of a lower concentration, water boils off until the HCl concentration rises to 20.2%. If you boil more concentrated acid, HCl boils off until the concentration falls to 20.2%.
TheHomeScientist 2 years ago
I understand the quality is better at howes but the price is better a lome depot! Great tutorial, thanx!
ricktoven2 2 years ago
reagent grade just means almost no impurities right?
jsmithmilitary 2 years ago
Yes. The exact type and percentage of impurities in reagent grade chemicals varies depending on the chemical. Technically, a reagent-grade chemical is one that has been assayed to test for the types of impurities common to that chemical (and production method, if different methods are used). The assay lists the impurities and their percentages. An ACS reagent-grade chemical is one that the ACS has published standards for and that meets those standards.
TheHomeScientist 2 years ago
ahah Howe's or Lome Depot.
FIFAMAN07C3 2 years ago 20
if you used less water can you make a more concentrated and still pure hcl?
panzuman 2 years ago
Sure, at the cost of using a lot more raw acid. The HCL vapor pressure in the two containers reaches equilibrium when the molarity of the acid in the two containers is the same.
TheHomeScientist 2 years ago
oh! i did not catch that i though it was just the waters natural ability to absorb gasses which brings me to another question after you let it sit can you put it in the fridge so that way the water could better absorb the gasses?
panzuman 2 years ago
No need. The system will equilibrate fine at room temperature.
TheHomeScientist 2 years ago
i understand that but could you dissolve more into both and "raise" the equilibrium?
panzuman 2 years ago
At equilibrium, the molarity of the acid in both containers will be identical, regardless of the volume of liquid in each container. Think of it this way: if you start with 100 mL of 10 M acid and add 100 mL of water, you end up with 200 mL of 5 M acid. That's true whether you add the water directly to the acid or keep it in a separate container. Same if you add only 11 mL of water. You end up with 111 mL of 9 M acid, whether you add the water directly to the acid or use a second container.
TheHomeScientist 2 years ago
Comment removed
TheScienceiscool 2 years ago
No. Typical soil contains very low nitrate concentrations unless it has recently been heavily treated with nitrate fertilizer. You're thinking about the way potassium nitrate was originally extracted from soil and straw that had been soaked with urine. They had to treat a lot of soil to get a little bit of saltpeter. In practical terms, this isn't a reasonable way to get nitrates. It's much easier to obtain them from other sources such as cold packs, fertilizer, stump remover, etc.
TheHomeScientist 2 years ago
No, it's not possible. Depending on the type of wood burned, wood ash contains varying amounts of sodium and potassium carbonates and hydroxides with smaller amounts of sulfates and other salts. Like most nitrates, potassium nitrate is a strong oxidizer, and wouldn't survive the flames without reacting with the fuel.
TheHomeScientist 2 years ago
Is the same method possible with 10% HCl?
FOATE 2 years ago
Sure, although it obviously limits the concentration of HCl you can get in the purified product.
TheHomeScientist 2 years ago
Ah I see, but the R labeled product can later on be purified further with the same method am I correct?
What would happen if you'd use 200 mL HCl and 100 mL water? Would you end up with more concentrated HCl, less, or the same?
FOATE 2 years ago
Hello, TheHomeScientist, i have a question, can hydrogen peroxide be concentrated in a similar way? Not exactly the same way, but similar, i would have two containers, one with dilute hydrogen peroxide and other with anhydrus calcium chlorhidre.
adriiPortillo 2 years ago
I don't know. I've never tried it. But you'd use up a lot of anhydrous CaCl2, because drugstore H2O2 is about 97% water, and the dehydration would take forever.
It's easier just to buy more concentrated H2O2. You can buy 6% or 12% H2O2 from a beautician supply store, or just search google for "food grade hydrogen peroxide" for a local source of 30% or 35% H2O2.
TheHomeScientist 2 years ago
I actually have access to 50% hydrogen peroxyde, but i want it up to at least 80% as it will be suitable for liquid hobby rocket propellant. I was actually wondering if H2O2 was reactive with calcium chlorhidre. boiling off the water of H2O2 just decomposes it..
by the way, very good videos. 5*.
adriiPortillo 2 years ago
Please don't do that, even if you can somehow get your hands on some. Even 30% H2O2 is a dangerous oxidizer, let alone 50%. And with 80%, you might as well be dealing with nitroglycerin. The 80% stuff will oxidize stuff spontaneously that you don't even think of as combustible. Bad accidents are commonplace with high percentage H2O2.
TheHomeScientist 2 years ago
not to worry, i know all of the dangers involved, but i must tell you is not an explosive by itself. I know that it may generate the dangerous organic peroxides or just set things on fire with only the touch of it. But I know you know a more than me, so ok, i'll stay away of it.
adriiPortillo 2 years ago
I've seen that before. my teacher was pouring about 85% H2O2 on a cotton. a few minutes later, the cotton ignites by its self. its shock the whole class.
yahoorif 2 years ago
I've read about that method on a forum once. Someone took 32% H2O2 and put it in a dessicator with CaCl2 as the hygroscopic. He said it didn't work, probably because O2 is released from the H2O2 (forming H2O) over time, so he ended up with less concentrated H2O2.
Hope this helps.
FOATE 2 years ago
lol the end is funny "you can buy it at hoes" good stuff im getting your book
jsmithmilitary 2 years ago
howes and lome depot? ahaha
Chisco1389 2 years ago
You floored me when you just put the acid and water containers in the big container and let them sit to get the high grade acid!!! Thats great!! On of the things I love about chemistry is that it gets you to think and solve problems
twycross3 2 years ago
Yeah, it wasn't until my first-year organic prof explained what the word "elegant" really meant that I got it. I thought elegant meant fashionable, expensive, whatever. What it really means is simple but effective. An elegant synthesis requires the fewest possible steps with the simplest possible reagents at room temperature, but provides yields near theoretical. As a means of purifying acid, this process definitely meet the requirements for being called elegant.
TheHomeScientist 2 years ago
No, any water will work, but for the purest product you should use distilled or deionized water.
TheHomeScientist 2 years ago
You can concentrate hydrochloric acid to 20.2% (w/w) by boiling. HCl forms a negative azeotrope with water at 20.2% HCl by mass. If you boil a hydrochloric acid solution that's less than 20.2% concentration, water will boil off until the solution reaches 20.2%. If you boil hydrochloric acid that's greater than 20.2% HCl by mass, HCl will boil off until the concentration reaches 20.2%.
TheHomeScientist 2 years ago
If I stock up on muriatic acid, and store it in a plastic mini-shed outside in my backyard, will the seasonal variations in temperature cause it to degrade faster? I live in the northern tier of the U.S. and rarely is it 20º C often.The shed supposedly does keep out rain and moisture though.
HomeScienceNow 2 years ago
I really don't know, although I suspect it's a bad idea to store the stuff in an environment that isn't at least somewhat temperature controlled.
TheHomeScientist 2 years ago
Thanks, Robert. I recently had insulated garage doors installed, so I may store the jugs in the garage and just run with it.
HomeScienceNow 2 years ago
I could store some outside, in the shed, and some in the garage. Then do tests of samples from both for any color or pH change.
HomeScienceNow 2 years ago
10.2 molar????? holy shit, i thought they diluted muriatic acid.
freakin1random 2 years ago
A lot of it is diluted. As I mentioned elsewhere, I've seen muriatic acid in hardware stores at 10%, 14%, 28%, and the 31.45% that I used.
TheHomeScientist 2 years ago
So what would be the new acid's concentration be?
coolliger 2 years ago
Half the concentration of the original acid. In my case, I was using about 10.2 M muriatic acid, so the product was about 5.1 M.
TheHomeScientist 2 years ago