What is molarity of K^+ in a solution that contains63.3ppm of K_3Fe(CN)_6.?(atomic masses are: K=39.1, Fe=56, C=12 , N=14)

1 Answer
anor277
Mar 21, 2018

Not high....

Explanation:

#"1 ppm"-=1*mg*L^-1#...and at these concentrations, we really do not have to consider solution density...

And so with respect to #K_3[Fe(C-=N)_6]#...we gots a concentration of #((63.3xx10^-3*g)/(329.24*g*mol^-1))/(1*L)=1.92xx10^-4*mol*L^-1#...

And so ...........

#[K^+]=3xx1.92xx10^-4*mol*L^-1=5.76xx10^-4*mol*L^-1#

Related questions
See all questions in Solving Using PPM (Parts Per Million)
Impact of this question
8933 views around the world
You can reuse this answer
Creative Commons License