A solution containing Pb^{2+} and a solution containing IO_3^- are poured together and quickly...


A solution containing {eq}Pb^{2+} {/eq} and a solution containing {eq}IO_3^- {/eq} are poured together and quickly mixed. After mixing, the solution contains 0.0030 M {eq}Pb^{2+} {/eq} and 0.040 M {eq}IO_3^- {/eq}. Immediately {eq}Pb(IO_3)_2 {/eq}(s), which has Ksp={eq}2.5 \times 10^{-13} {/eq}, begins to precipitate. Calculate the free concentrations of {eq}Pb^{2+} {/eq} and {eq}IO_3^- {/eq} after the precipitation reaction comes to equilibrium.

Calculation of Ions from the Dissolution of Sparingly Soluble Salt at Equilibrium

Insoluble salts form an equilibrium condition in an aqueous medium. The equilibrium reaction liberates some ions that can be quantified using the solubility constant of the salt.

Answer and Explanation: 1

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The concentration of the ions are:

$$\begin{align*} &Pb^{2+} = 0.074 \ M \\ &IO_3^- = 0.185 \ M \\ \end{align*} $$


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Solubility Equilibrium: Using a Solubility Constant (Ksp) in Calculations


Chapter 11 / Lesson 5

Learn about solubility product constant. Understand the definition of Ksp, the Ksp formula, how to calculate Ksp, and how to find molar solubility from Ksp.

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