What mass of $"nickel(II) chloride hexahydrate"$ is present in a $250mL$ volume of $1.00mol*L^-1$ concentration?

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Answer 1 · 2018-01-08T18:12:16

By definition, $"molarity"="moles of solute"/"volume of solution"$ ...we require a mass of approx. $75*g$

Here you specify a $"molarity"=1.00*mol*L^-1$ with respect to $Ni(NO_3)_2*6H_2O$ and a volume of $250*mL-=0.250*L$ ...

And so we require a molar quantity of....

$"moles of solute"="molarity"xx"volume"$

And note that the given product has units of $mol*L^-1xxL-="moles"$ as required....

And so .........

$"moles of nickel salt hydrate"=1.00*mol*L^-1xx0.250*L=0.250*mol$

And to get the mass we take the product....

$0.250*molxxunderbrace(290.79*g*mol^-1)_"molar mass of metal hydrate"=??*g$

What mass of "nickel(II) chloride hexahydrate""nickel(II) chloride hexahydrate" is present in a 250*mL250*mL volume of 1.00*mol*L^-11.00*mol*L^-1 concentration?