Question

1. Calculate the mass of each compound required to make 25mL of the following solutions:
(a) 0.10 M Ni(NO3)2 • 6H2O
(b) 1.0 M NaClO4 • H2O
(c) 0.11 M trien (C6H18N4)

2. Calculate the concentrations of Ni2+ and trien in a solution prepared by mixing equal volumes of solutions 2(a) and 2(c).

***Note: Ni(trien) = nickel(II) triethylenetetramine

I don't know how to start this problem or what to do with the "• H2O" on the end. Do I include that in my calculations? More detailed explanation the better, thanks!

Answer 1

1a. mols needed = M x L
Then mols = grams/molar mass. You know molar mass and mols, solve for grams.

Same concepts for 2 but not worked same way.

Answer 2

So for part 2 I assume I add he volumes for 50mL? And then do I find just the moles of Ni2+? So one mole of Ni per 2 moles of NO3?
I just don't understand how to calculate the concentration of a single element using two different compounds.