Hg2(IO3)2의 몰용해도. concentrations of Hg2^2+ and IO3^-
Mercury(I) is a diatomic ion (Hg2^2+, also called mercurous ion)
with a charge of +2. Mercury(I) iodate dissociates as follows:
Hg2(IO3)2(s) ⇌ Hg2^2+(aq) + 2IO3^-(aq)
Ksp = [Hg2^2+] [IO3^-]^2 = 1.3×10^(-18)
Hg2(IO3)2의 몰질량 = 750.99 g/mol
a) Find the concentrations of Hg2^2+ and IO3^-
in a saturated solution of Hg2(IO3)2(s)
if there are no other significant species
such as the ion pair Hg2^2+•IO3^-.
b) Find [Hg2^2+] in a 0.010 M solution of KIO3
saturated with Hg2(IO3)2(s).
Hg2(IO3)2(s) ⇌ Hg2^2+(aq) + 2IO3^-(aq)
Ksp = [Hg2^2+] [IO3^-]^2
= (s) (2s)^2 = 4s^3
= 1.3×10^(-18)
( s = Hg2(IO3)2의 몰용해도 )
( 참고 https://ywpop.tistory.com/8434 )
s = [Ksp / 4]^(1/3)
= [(1.3×10^(-18)) / 4]^(1/3)
= 6.875×10^(-7) M
[Hg2^2+] = s = 6.88×10^(-7) M
[IO3^-] = 2s = 2×(6.88×10^(-7) M)
= 1.376×10^(-6) M
= 1.38×10^(-6) M
KIO3(aq) → K^+(aq) + IO3^-(aq)
[KIO3] = [IO3^-] = 0.010 M
Ksp = [Hg2^2+] [IO3^-]^2
= (s) (2s + 0.010)^2
≒ (s) (0.010)^2
= 1.3×10^(-18)
s = (1.3×10^(-18)) / (0.010)^2
= 1.3×10^(-14) M
---> [Hg2^2+] in a 0.010 M solution of KIO3
[ 관련 글 https://ywpop.tistory.com/12688 ] PbI2의 몰용해도
[키워드] Hg2(IO3)2의 몰용해도 기준, Hg2(IO3)2의 Ksp 기준
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