A student wishes to reduce the zinc ion concentration in a saturated zinc iodate solution to 1 xx 10^-61×10−6 M. How many moles of solid KIO_3KIO3 must be added to 1.00 L of solution? [K_(sp) Zn(IO_3)_2 = 4 xx 10^-6KspZn(IO3)2=4×10−6 at 25°C)?

1 Answer
anor277
Jun 1, 2018

So this is a K_"sp"Ksp problem, for which you have provided the relevant data...

Explanation:

We address the equilibrium...

Zn(IO_3)_2(s) rightleftharpoonsZn^(2+)+2IO_3^(-)Zn(IO3)2(s)⇌Zn2++2IO−3...

for which K_"sp"=[Zn^(2+)][IO_3^(-)]^2-=4.0xx10^-6Ksp=[Zn2+][IO−3]2≡4.0×10−6...

We will be requiring that Zn^(2+)-=1.0xx10^-6*mol*L^-1Zn2+≡1.0×10−6⋅mol⋅L−1 by the terms of the question...and thus we solve for [IO_3^(-)][IO−3] in the given equation.....

[IO_3^(-)]=sqrt(K_"sp"/[[Zn^(2+)]])=sqrt((4.0xx10^-6*mol*L^-1)/(1.0xx10^-6*mol*L^-1))[IO−3]=√Ksp[Zn2+]=√4.0×10−6⋅mol⋅L−11.0×10−6⋅mol⋅L−1

sqrt4=2*mol√4=2⋅mol...I must be clever cos I did this all in my nut!

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