Question

Use the following data to calculate the KspK_{\mathrm{sp}} value for each solid. The solubility of Li2CO3\mathrm{Li}_{2} \mathrm{CO}_{3} is 7.4×102 mol/L.7.4 \times 10^{-2}\ \mathrm{mol} / \mathrm{L}.

Solutions

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The reaction is

Li2CO3(s)2Li+(aq)+CO32(aq)Li_2CO_3(s) \rightleftharpoons 2Li^+(aq) + CO_3^{2-}(aq)

Let s = solubility of Li2CO3Li_2CO_3

From the balanced equation, the following relationship can be obtained

[Li+]=2s[Li^+]=2s

[CO32]=s[CO_3^{2-}]=s

Ksp=[Li+]2[CO32]=(2s)2(s)=4s3=4(7.4×102)3K_{sp}=[Li^+]^2[CO_3^{2-}]=(2s)^2(s)=4s^3=4(7.4\times10^{-2})^3 Ksp=1.62×103K_{sp}=1.62\times10^{-3}

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