- #1
higherme
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The question:
How many grams of Ba(IO3)2 can be dissolved in 700mL of a 0.100M KIO3 solution at 25C? use activity coefficients for this. (Ksp of Ba(IO3)2 =1.57E-9)
my answer:
I used this equation: Ksp = (concentration) * (activity coefficient)
well i found out that my ionic strength of KIO3 is 0.100M and from a chart, i found the respective activity coeff for Ba2+ and IO3-.
Ba2+ ---> 0.38
IO3^- ----> 0.775
Ba(IO3)2 <----> Ba2+ + 2IO3^-
I 0 x 0.100M
C +x +2x
E x 0.100M+2x
using the equation above,
Ksp = [Ba2+]*(activity coeff of Ba) * [IO3^-]^2 * (activity coeff of IO3^-)^2
1.57E-9 = (x)(0.38) * (0.100+2x)^2 * (0.775)^2
so i solve for X and that would be the concentration of Ba(IO3)2 in mol/L
BUT, to solve for X, i found it complicated because there would be 3 solutions for X aren't there?? since it's X^3... so i am confused on what to do.
help appreciated, Thanks.
How many grams of Ba(IO3)2 can be dissolved in 700mL of a 0.100M KIO3 solution at 25C? use activity coefficients for this. (Ksp of Ba(IO3)2 =1.57E-9)
my answer:
I used this equation: Ksp = (concentration) * (activity coefficient)
well i found out that my ionic strength of KIO3 is 0.100M and from a chart, i found the respective activity coeff for Ba2+ and IO3-.
Ba2+ ---> 0.38
IO3^- ----> 0.775
Ba(IO3)2 <----> Ba2+ + 2IO3^-
I 0 x 0.100M
C +x +2x
E x 0.100M+2x
using the equation above,
Ksp = [Ba2+]*(activity coeff of Ba) * [IO3^-]^2 * (activity coeff of IO3^-)^2
1.57E-9 = (x)(0.38) * (0.100+2x)^2 * (0.775)^2
so i solve for X and that would be the concentration of Ba(IO3)2 in mol/L
BUT, to solve for X, i found it complicated because there would be 3 solutions for X aren't there?? since it's X^3... so i am confused on what to do.
help appreciated, Thanks.