How would you prepare 1.00L of a 0.50M solution of each of the following?
a) NiCl2 from the salt NiCl2 . 6H20
I know I have to find the molar mass, as advised by other people, but the problem is that I don't know whether or not to include the 6H2O into it if the question said NiCl2 from the salt NiCl2 . 6H20.
Thank you so much in advance if you can help me out with this question.
2007-08-15 08:56:59 · 2 answers · asked by Andrew 2 in Science & Mathematics ➔ Chemistry
My only gripe with this is that it says NiCl2 from the salt NiCl2 . 6H20, so something tells me I disregard the .6H20.
2007-08-15 09:09:00 · update #1
Yes, you need to include the molecular weight of 6H2O in the formula weight of the nickel chloride hydrate.
Get 1 mol of NiCl2 and dissolveit up to 1L solution.
0.50molNiCl2 x 1molNiCl2*6H2O/1molNiCl2 x 237gNiCl2*6H2O/1molNiCl2*6H2O = 118g NiCl2*6H2O needed
2007-08-15 09:01:30 · answer #1 · answered by steve_geo1 7 · 1⤊ 0⤋
When you weigh out the sample, you are weighing NiCl2.6H2O. One mole of NiCl.6H2O will contain one mole of NiCl2.
Calculate the MW of NiCl2.6H2O and weigh 0.5 x MW grams..
2007-08-15 09:54:26 · answer #2 · answered by skipper 7 · 0⤊ 0⤋