Hg₂ Cl₂ (s) Hg2 (aq) + 2Cl(aq) = Ksp = 1.20 × 10–18 Determine the concentrations of Hg2+ and Cl¯ in a saturated solution of Hg₂Cl₂ in pure water (assume μ = 0 M). [Hg2+] = [Hg2+] = 6.7 X10-7 [Hg²+] = Determine the concentrations of Hg2+ and Cl- in a saturated solution of Hg₂Cl₂ in a solution with an ionic strength of 0.010 M 8.26 X10-7 M 1.1 X10-6 M [CI] = 1.338 x10-6 M [CI] = Determine the concentrations of Hg2+ and Cl¯ in a saturated solution of Hg₂Cl₂ in a solution with an ionic strength of 0.10 M. M 16.52 x10-7 [CIT] = M M
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![Hg₂ Cl₂ (s) Hg2+(aq) + 2 Cl¯(aq)
Ksp = 1.20 × 10–18
+
Determine the concentrations of Hg2 * and CI in a saturated solution of Hg₂Cl₂ in pure water (assume μ = 0 M).
[Hg2+] = 6.7 X10-7
[Hg²+] =
8.26 X10-7
[Hg²+] =
M
Determine the concentrations of Hg2+ and Cl¯ in a saturated solution of Hg₂Cl₂ in a solution with an ionic strength of 0.010 M
1.1 X10-6
M
[CI] =
M
[Cl] =
1.338 ×10-6
Determine the concentrations of Hg2+ and Cl¯ in a saturated solution of Hg₂Cl₂ in a solution with an ionic strength of 0.10 M.
[Cl] =
M
16.52 X10-7
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60233bc8-b7a4-4cb1-97f6-a0fef93353db%2F3397e020-0e3a-437f-ac2e-47d43e6af5cd%2Fancvdet_processed.jpeg&w=3840&q=75)
To determine the concentration of Hg22+ and Cl- in pure water and at ionic strength of 0.010 M and 0.10 M.
Given Ksp = 1.20 x 10-18
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