In: Chemistry
HClO / KClO buffer system is
to be constructed that is also 0.043 M in
Zn2+.
What is the minimum [HClO] /
[ClO-] that must be maintained to keep
a precipitate of zinc hydroxide from forming?
[Zn2+] = 0.043 M
Zn+2 + 2OH- Zn(OH)2(s)
Ksp of Zn(OH)2 = 5 x 10-17
Ksp = [Zn2+][OH-]^2
5 x 10-17 = 0.043 * [OH-]^2
[OH-] = 3.41 x 10^-8 M
Hence this is the minimum concentration of OH- that is required to precipitate Zn(OH)2.
pOH = - log (3.41 x 10^-8)
= 7.46
pH = 14 - 7.46
= 6.54
Hence, 6.54 is the maximum pH that will precipitate Zn(OH)2.
For a buffer system we have:
pH = pKa + log [ClO-] / [HClO]
6.54 = 7.53 + log [ClO-] / [HClO]
log [ClO-] / [HClO] = - 0.99
[ClO-] / [HClO] = 0.1023
[HClO] / [ClO-] = 1 / 0.1023
[HClO] / [ClO-] = 9.77
Hence, [HClO] / [ClO-] = 9.77 is the minimum value that must be maintained to keep a precipitate of zinc hydroxide from forming.