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12 Dec 2019

1.Calculate the pH needed to start precipitation of tin (II) sulfide from a solution containing 0.0049 M of the tin (II) ion. The sulfide ion is produced in a solution saturated with H2S via the following equilibrium: [H+]2 [S2−] = 1.1 x 10−22. (Ksp = 1.3 x 10−23 for tin (II) sulfide)

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Collen Von
Collen VonLv2
13 Dec 2019

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Related questions

1. A solution is prepared so that the concentrations of manganese(II) nitrate, zinc(II) nitrate, mercury(II) nitrate, and copper(II) nitrate are all 0.100 M. If the solution is slowly titrated with 0.100 M sodium sulfide, which metal sulfide will precipitate first?

zinc sulfide, Ksp = 1.8???10?25

copper(II) sulfide, Ksp = 5.4???10?37

manganese(II) sulfide, Ksp = 2.4???10?14

mercury(II) sulfide, Ksp = 1.8???10?53

2. Calculate molar solubilities, concentrations of constituent ions, and solubilities in grams per liter for the following compounds at 25°C:

[Sn2+] =

[S2?] =

solubility = g SnS/Liter

[Cd2+] =

[PO43?] =

solubility = g Cd3(PO4)2/Liter

tin(II) sulfide, SnS, Ksp = 9.00???10?27

cadmium(II) phosphate, Cd3(PO4)2, Ksp = 2.50???10?33











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