copper concentration (1 Viewer)

[Steven12]

i had something like 0.03mol per litre

u guys?

 

[The Bograt]

Yeah I think I got the same, but I had more decimal places so I don't know exactly

 

[Steven12]

does it matter, like do you have to round it to a really accurate decimal, i mean as long as you show the working out...

 

[xeriphic]

well I can't exactly remember but I think same

 

[tomato_sauce217]

OMG//
are u sure it's 0.03 moles/Litre???
i had that figure some where in the anwer because like.... initially it was that... den it was displaced and some copper ions are gone.. i calculated.. it's a diff answer

 

[L45er]

Yeh i got 0.030mol/L and i checked it numerous times...

 

[sub]

i think i got something like 0.007 ish...not sure...maybe it was a 3?
but yeah that sounds abt right. maybe too many zeroes too...haven't checked and dont wanna either.

 

[scruffy012]

yeah i dunno what i got but it was something similiar, 0.003, i hope i got it right.......

scruffy

 

[Sanchez__]

From what I remember, initial conc of cu was 0.0125. I think the final conc turned out at about 0.007 but not sure on that.

 

[sub]

From what I remember, initial conc of cu was 0.0125. I think the final conc turned out at about 0.007 but not sure on that.

hey thats what i got...hope im right.

 

[Zeppelin]

Yeah, I got 0.029... All you had to do was calucluate the concentration of the extracted copper, and subtract it from the initial concentration. I got it, but it was the biggest fluke. I can't believe how well I did!

 

[tina_goes_doo]

Yeah i got 0.03 too. Did it the same way as zepplelin but had stuff with moles and crap. Then divided it but the volume to get the concentration.

 

[babygoose!]

yeh i had something like 0.03 as well...good to hear so many of you had the same answer cos i wasnt quite sure if i was right

 

[tina_goes_doo]

I was certain i didn't have it right! I thought i knew the calculations but....it was all a lie!!

 

[xprshn]

OMg quit shattering my hopes !!.. i got 0.04 . awww

What about me?
It isn't fair.. i've had enough now i want my share
Can't you see.. I wanna live..

 

[lucyinthehole]

i got some answer in the most roundabout, non scientific way. just kinda followed my crazy logic, like "if this is this, then this is that". i think i got something close to the answers here so.... *fingers crossed* and i only came back to that in the last 5 minutes. couldn't figure it out before that.

 

[mervvyn]

i got 0.030 mol/L, you had to round up from 0.0295 or something cos of sig figs. 0.0125 was the inital number of moles of copper i think.

 

[lukebennett]

i just calculated the number of moles in the original solution then calculated the nuber of moles which was reduced. took that away from the initial and then divided that by the volume of the liquid.
i had 0.007 in the end. then you had to divide this by the volume to get the answer

 

[tina_goes_doo]

I thought i did do it your way but i got 0.03.

 

[smegthehead]

i can't remember what my answer was, but i remember that i found the number of moles of displaced copper, subtracted that from the number of moles of copper originally in the solution, then used the moles=(molarity x volume)/1000 equation to find the concentration