What concentration of [tex] \text{SO}_3^{2-} [/tex] is in equilibrium with [tex] \text{Ag}_2\text{SO}_3 \text{(s)} [/tex] and [tex] 3.60 \times 10^{-3} \, \text{M} \, \text{Ag} [/tex]? The [tex] K_{sp} [/tex] of [tex] \text{Ag}_2\text{SO}_3 [/tex] is [tex] 1.5 \times 10^{-14} [/tex].
Answer (2)
Ag₂SO₃ ⇔ 2Ag⁺ + SO₃²⁻
Ksp = [Ag⁺]²[SO₃²⁻] [SO₃²⁻] = x
1.5 10⁻¹⁴ = (3.6 10⁻³)² * x 1.5 10⁻¹⁴ = 12.96 10⁻⁶ * x x = 1.5 10⁻¹⁴/12.96 10⁻⁶ x=0.12 10⁻⁸= 1.2 10⁻⁹M
The concentration of sulfate ions SO 3 2 − in equilibrium with solid silver sulfite Ag 2 SO 3 and a silver concentration of 3.60 × 1 0 − 3 M is calculated to be approximately 1.16 × 1 0 − 9 M . This is obtained using the solubility product constant K s p = 1.5 × 1 0 − 14 .
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