In a sautrated solution of the sparingly soluble strong electrolyte AgIO3 (Molecular mass = 283) the equilibrium which sets in is AgIO3(s) $\leftrightharpoons$ Ag+(aq) + $IO_3^-$ If the solubility product constant Ksp of AgIO3 at a given temperature is 1.0 $\times$10−8, what is the mass of AgIO3 contained in 100 ml of its saturated solution?

Question

In a sautrated solution of the sparingly soluble strong electrolyte AgIO₃ (Molecular mass = 283) the equilibrium which sets in is
AgIO_3(s) $\leftrightharpoons$ Ag⁺(aq) + $IO_3^-$
If the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 $\times$10⁻⁸, what is the mass of AgIO₃ contained in 100 ml of its saturated solution?

28.3 × 10⁻² g

2.83 × 10⁻³ g

1.0 × 10⁻⁷ g

1.0 × 10⁻⁴ g

Solution

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