Hg2(IO3)2의 몰용해도. concentrations of Hg2^2+ and IO3^-

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

 

[ 블로그스팟 https://ywpop.blogspot.com/2024/09/hg2io32-concentrations-of-hg22-and-io3.html ]

 

 

 

[키워드] Hg2(IO3)2의 몰용해도 기준, Hg2(IO3)2의 Ksp 기준