Question

Please help!!! So confused...What are the molar concentrations of the ions in 0.11 M aluminum sulfate?

Answer 1

@january123 @jackoo @mr.420 @dan815 @Luigi0210 @hayhayman @lordofpens @Nerdgirl @charlie7770 @G-unit @geekgirl1000 @ashton_gates2131

Answer 2

@HackberryAbby18 I do actually! lol

Answer 3

let me see what I can do okay :D

Answer 4

Okay!!

Answer 5

I hope this can help : but no worries I am still looking :D

https://ec.gc.ca/lcpe-cepa/default.asp?lang=En&n=491F0099-1&offset=8

Answer 6

Thank-you, ill read it!

Answer 7

Do you know the molecular formula for aluminum sulfate @glamourariss?

Answer 8

Al2(SO4)3 If I am not mistaken. :) @matt101

Answer 9

That's right! But remember, when this compound is dissolved, it dissociates into all the ions it's made of. So even though the concentration of Al2(SO4)3 is 0.11 M as the question says, the concentrations of the ions will be different.

Al2(SO4)3 contains two Al- ions and three SO4(2-) ions. So, for every mole of Al2(SO4)3 that dissolves, you actually produce TWICE as many moles of Al- (making it twice as concentrated), and THREE TIMES as many moles of SO4(2-) (making it three times as concentrated).

So if you have 0.11 M Al2(SO4)3, what are the concentrations of the individual ions - Al- and SO4(2-)?

Answer 10

So would you times each (.11) by its ions? Like .11 times 2 and so forth?

Answer 11

Yup!

Answer 12

Woot woot! Makes sense. Thanks so much, I'm a Bio major and I suck at chem. I decided to take this class online solely based on the Professor but instantly knew it was a bad idea-i'm teaching myself, so here I am. I only had 3 tries and was on my last attempt. @matt101

Answer 13

No worries - glad I could help. If you have any other questions just tag me in your posts and I'll have a look!