Quote:
Originally Posted by ilvtofu
I don't have much of a chem background but i did do chem 12.... twice...
0.0222mols/L =0.00222 mols/100mL
=0.00222mols/3.0mL because there were no mols in the 97ml of water added.
so... 0.00222mols/3.0ml x 1000ml/3ml = 0.74M?
But based on logic I think just calculate the molarity based off that?
I am probably wrong :/ oh wellz, google the question it seems pretty typical haha I feel really dumb now, but there I took a stab at it
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DING DING DING!
WE HAVE A WINNAAHHHHH!
Thank you!
Now, one left!
Quote:
Originally Posted by CRS
Because I'm apparently retarded now by not taking chem right after grade 12...
Assuming a density of 1.055 g/mL, what is the mass % NaOCl in a full-strength bleach solution that is 0.62 M NaOCl?
What I figured to do was...
0.62M NaOCl x 74.441g/1mol NaOCl = 46.15342g NaOCl
From here I have no idea what to do with the density.
I thought of doing this....
46.15gNaOCl x 1mL/1.055g = 43.7ml
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Done.
Since density is 1.055g/mL it means it is 1055g/L
Then is simply 46.15/1055 which is then 4.4%