I am truly sorry for the double post, i should have known "help" is not good in the title:
So i just did a gravimetric experiment where we took an unknown mass of a compound containing nickel and with the data gathered and some formulas to work with,
Ni^2+ (aq) + 2 C4H7O2N2H (alc) =====> Ni (C4H7O2N2)2 (s) + 2H^+ (aq)
Let me list my data first:
Mass of original sample: 1.0601 g
Mass of precipitate
9A: 0.2857 g
9B: 0.2815 g
And im asked to find the percentage of nickel in the unknown sample, which would be the 1.0601 g
So what i did first was took the mass of 9A's precipitate and converted it to moles,
0.2857 g / 288.9158 g /mol = 9.8887 x 10^-4 mol Ni(C4H7O2N2)2
From here, i converted that value into moles of nickel which would be the same since:
9.8887 x 10^-4 mol Ni(C4..)2 x 1 mol Ni divided by 1 mol of Ni(C4..)2 = 9.8887 x 10^-4 mol Ni
From here i can calculate the mass by taking the mass of the nickel and multiplying it by the molar mass of nickel:
9.8887 x 10^-4 mol Ni * 58.693 g / mol = 0.058039 g Ni
And then i divided it by the unknown sample's mass to obtain:
0.05803 g / 1.0601 g *100% = ~5.50%
2. Then the second part asks which of these choices my sample could be:
NiCl2*6H2O, NiSO4*6H2O, NiSO4*7H20, NiBr2*6H2O
Now what i decided to do was compare the percentages of nickel within each compound, I thought of a couple ways of doing this:
1. Take the molar mass of nickel and divide it by the total molar mass of the given compounds
2. Find equations like taking NiCl2*6H2O and then adding the alc shown above and then from there balance it and then here i thought which mass i would use, the unknown or the precipitate?
I gave it some thought and im still kinda stump on which approach would be appropriate
All feedback and help is greatly appreciated!
Thank you!