Respuesta :
CuBr is soluble in pure water at a solubility of 0.2583 g/L, while CoBr₂ is soluble at a solubility of 7.50 × 10⁻⁶ g/L
Given,
The equation of reaction as; CuBr₂ → Cu²⁺ + 2Br⁻
In pure water, the Ksp of the solution is 6.27 * 10^-9
Ksp = [Cu²⁺] [Br⁻]²
Ksp = x³
Let's substitute and solve
x³ = 6.27 × 10⁻⁹
x = [tex]\sqrt[3]{6.27 * 10^{-9} }[/tex]
x = 0.0018
The molecular weight of CuBr₂ is 143.5 g/mol
The solubility of CuBr₂ is
0.0018 × 143.5 = 0.2583 g/L
The solubility in 0.0060M of CoBr₂
The equation of dissociation is given as
CoBr₂ → Co²⁺ + 2Br⁻
0.012 0 0
0 0.120 2 * 0.0060 = 0.012M
The dissociation of copper bromide is
CuBr₂ → Cu²⁺ + Br⁻
c 0 0.012
c - s s s + 0.012
The Ksp of this reaction is
[Ksp] = [Co²⁺] [Br⁻]
The Ksp of CuBr₂ = 6.27 × 10⁻⁹
6.27 × 10⁻⁹ = s(s + 0.012)
s + 0.012 = 0.012
0.012 > > > s
6.27 × 10⁻⁹ = s × 0.012
s = 6.27 × 10⁻⁹ / 0.012 = 5.225 × 10⁻⁷ mol / l
Let's convert this into g/L
s = 5.225 × 10⁻⁷ × 143.5 = 7.50 × 10⁻⁶ g/L
Therefore,
The solubility of CuBr in pure water is 0.2583 g/L and the solubility in CoBr₂ is 7.50 × 10⁻⁶ g/L
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