Thanks alot, this video was straight to the point and clearly done, very useful for reminding me of how to do titrations. I've got an exam on a titration experiment i have to do tommorow morning
nice demonstration, but i think you had an overshooting since the color of your end point is dark pink which should only be light pink. this will result to a slight increase in the computed HCl concentration in your unknown.
could you work out the concentration of the acid by taking a 100ml solution of hcl and a 100ml solution of water and weighing them and use the diffrence in weght to work out the concentration
@crapbag1997 Yes that's right, measuring density is another common way of finding concentration. If you can find a table of density vs concentration, this would be a quick way to do it. It might be slightly off from your actual solution though, if there are a lot of impurities.
@mrhomescientist thank you i have been doing math all day trying to find a formula see i'm only realy a diy chemist so i am knew to calculating acid percrentages and i would like it if you sent me a message if you came across a table thanks
@crapbag1997 Just google 'hydrochloric acid density table,' there's a good one about the 4th link down. There's lots of information out there, Google is your friend!
@megamarko94 Mine is 1%, but the concentration won't make a difference. It will still change color at the same pH. You just won't have to use quite as much of your 3% to get the same intensity of color I had.
@98JMA Yep, you're right. I forgot there was a difference - the equivalence point is where the number of moles of base equals the number of moles of acid, and the end point is where the color changes. The end point is a close estimation of the equivalence point. Thanks for pointing that out.
@megamarko94 The 10 comes from converting the mL in density (g/mL) to the L in molarity (mol/L), and is from the equation's derivation.
This is a general equation, and works for any substance you want to know the concentration of. It's very simple to rearrange so that weight% is by itself on one side of the equation.
@megamarko94 To go from weight % to molarity, I used the formula
molarity = (10*weight%*density) / molar mass
You can solve that for weight% to do what you wanted. I measured the density of my particular solution myself, but you might be able to look up ballpark numbers on the web someplace.
@spotlightman1234 Thanks! Just out of frame is a much larger jar with another pound in it under oil. I'll have to have some fun with that in a future video :)
wouldn't wanna spill that HCl on yourself, 9.5M HCl is strong isn't it?
VenomXRaptor 2 days ago
Thanks alot, this video was straight to the point and clearly done, very useful for reminding me of how to do titrations. I've got an exam on a titration experiment i have to do tommorow morning
MrPorflexpk 2 weeks ago
Nice video. It was clear, and I was able to follow with what you were saying. Thanks!
OkReadThis 2 weeks ago
nice demonstration, but i think you had an overshooting since the color of your end point is dark pink which should only be light pink. this will result to a slight increase in the computed HCl concentration in your unknown.
bingibale 3 weeks ago
could you work out the concentration of the acid by taking a 100ml solution of hcl and a 100ml solution of water and weighing them and use the diffrence in weght to work out the concentration
crapbag1997 6 months ago
@crapbag1997 Yes that's right, measuring density is another common way of finding concentration. If you can find a table of density vs concentration, this would be a quick way to do it. It might be slightly off from your actual solution though, if there are a lot of impurities.
mrhomescientist 6 months ago
@mrhomescientist thank you i have been doing math all day trying to find a formula see i'm only realy a diy chemist so i am knew to calculating acid percrentages and i would like it if you sent me a message if you came across a table thanks
crapbag1997 6 months ago
@crapbag1997 Just google 'hydrochloric acid density table,' there's a good one about the 4th link down. There's lots of information out there, Google is your friend!
mrhomescientist 6 months ago
u do know that ur taking away solution with ur stirring rod
ph4ntom012 8 months ago
i love i love i love, cramming for a prac test, so happy i found this
MegaShaedow 8 months ago
Nice beard. I think I might subscribe to your videos. (for the science, not the beard.)
MossOwnsYou 9 months ago
@MossOwnsYou Hah thanks! Sounds like I need to think of some beard-related experiments...
mrhomescientist 9 months ago
Phenolphthalein solution 1% or 3% for titration will I get wrong results if I use 3%.
megamarko94 10 months ago
@megamarko94 Mine is 1%, but the concentration won't make a difference. It will still change color at the same pH. You just won't have to use quite as much of your 3% to get the same intensity of color I had.
mrhomescientist 10 months ago
I think you mean that the phenolphthalein turns pink once the END POINT is observed, not the EQUIVALENECE point.
98JMA 1 year ago
@98JMA Yep, you're right. I forgot there was a difference - the equivalence point is where the number of moles of base equals the number of moles of acid, and the end point is where the color changes. The end point is a close estimation of the equivalence point. Thanks for pointing that out.
mrhomescientist 1 year ago
What does 10 stands for in formula.
Can this equation work for other acids.
How would my formula look like if I want weight % not molarity Plz write it.
megamarko94 1 year ago
@megamarko94 The 10 comes from converting the mL in density (g/mL) to the L in molarity (mol/L), and is from the equation's derivation.
This is a general equation, and works for any substance you want to know the concentration of. It's very simple to rearrange so that weight% is by itself on one side of the equation.
mrhomescientist 1 year ago
Great channel just keep making videos
megamarko94 1 year ago
This has been flagged as spam show
How can I convert molarity to weight %
megamarko94 1 year ago
How can I convert molarity to weight %
megamarko94 1 year ago
@megamarko94 To go from weight % to molarity, I used the formula
molarity = (10*weight%*density) / molar mass
You can solve that for weight% to do what you wanted. I measured the density of my particular solution myself, but you might be able to look up ballpark numbers on the web someplace.
mrhomescientist 1 year ago
How can I connvert molarity to weight %
I don't get it
megamarko94 1 year ago
Nice experiment it would be better if you can use Methyl Orange too. I would love to watch that.
Nickof24 1 year ago
i like the sodium in the background very fitting for the NaOH being used
spotlightman1234 1 year ago
@spotlightman1234 Thanks! Just out of frame is a much larger jar with another pound in it under oil. I'll have to have some fun with that in a future video :)
mrhomescientist 1 year ago
@mrhomescientist omg a whole pound! jeez
spotlightman1234 1 year ago