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What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? consider a solution that is 2.3×10−2 m in fe2+ and 2.0×10−2 m in mg2+?

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ChemistryHelper2024
Ksp for FeCO₃ is 3.07 x 10⁻¹¹
Ksp for MgCO₃ is 6.82 x 10⁻⁶
So Fe²⁺ will precipitated first as solubility product of FeCO₃ is lower than solubility product of MgCO₃
Ksp FeCO₃ = [Fe²⁺][CO₃²⁻] 
3.07 x 10⁻¹¹ = (2.3 x 10⁻²) [CO₃²⁻]
[CO₃²⁻] = 1.33 x 10⁻⁹ M to precipitate Fe²⁺ ions

Ksp MgCO₃ = [Mg²⁺][CO₃²⁻]
6.82 x 10⁻⁶ = (2.0 x 10⁻²) [CO₃²⁻]
[CO₃²⁻] = 3.4 x 10⁻⁴ M to precipitate the Mg²⁺ ions

Ksp FeCO₃ = [Fe²⁺][CO₃²⁻]
3.07 x 10⁻¹¹ = [Fe²⁺] (3.4 x 10⁻⁴)
[Fe²⁺] = 9 x 10⁻⁸ M when Mg²⁺ ions precipitate


mahima6824soni

The remaining concentration is                      [tex][Fe^2^+] = 9 \times 10^-^8 M\; when\; Mg^2^+ ions \; precipitate[/tex]

What is a cation?

A cation is an ion that contains a positive charge. It gains a positive charge by donating an electron.

The equilibrium concentration for [tex]FeCO_3 = 3.07 \times 10^-^1^1[/tex]

The equilibrium concentration for [tex]MgCO_3 = 6.82 \times 10^-^6[/tex]

[tex]Fe^2^+[/tex] will precipitate first

[tex]FeCO_3 = [Fe^2^+][CO_3^2^-][/tex]

[tex]3.07 \times 10^-^1^1 = (2.3 \times10^-^2) [CO_3^2^-][/tex]

[tex][CO_3^2^-] = 1.33 \times 10^-^9 M[/tex] to precipitate [tex]Fe^2^+[/tex] ions

[tex]MgCO_3 = [Mg^2^+][CO_3^2]\\6.82 \times 10^-^6 = (2.0 \times 10^-^2) [CO_3^2-]\\[CO_3^26-] = 3.4 \times 10^-^4 M to\; precipitate\; the \;Mg^2^+ ions[/tex]

[tex]FeCO_3 = [Fe^2^+][CO_3^2^-][/tex]

[tex]3.07 \times 10^-^11= [Fe^2^+] (3.4 \times 10^-^4)[/tex]

[tex][Fe^2^+] = 9 \times 10^-^8 M\; when\; Mg^2^+ ions \; precipitate[/tex]

The remaining concentration is 9 × 10⁻⁸ M.

Learn more about cations

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