Question

An experimental cell is set up such that one half-cell contains a solid silver electrode dipping into a saturated solution of silver oxalate. The oxalate ion comes from added sodium oxalate so that equilibrium concentration of oxalate ions is 0.33M. This half-cell is connected to a standard hydrogen electrode (SHE) half cell. The measured potential for this cell is 0.453V. What is the experimental value of the solubility product constant for silver oxalate?

Answer 1

Answer on the question 77504 Chemistry / Inorganic Chemistry

$$0.453\,\mathrm{V} = 0.799\,\mathrm{V} + \frac{0.059}{1}\,\mathrm{lg}[\mathrm{Ag}^{+}]$$ $$0.059\,\mathrm{lg}[\mathrm{Ag}^{+}] = 0.453 - 0.799$$ $$\mathrm{lg}[\mathrm{Ag}^{+}] = -5.86$$ $$[\mathrm{Ag}^{+}] = 1.38 \cdot 10^{-6}$$ $$K_{\mathrm{sp}} = [\mathrm{Ag}^{+}]^{2} \cdot [\mathrm{C}_{2}\mathrm{O}_{4}^{2-}] = (1.38 \cdot 10^{-6})^{2} \cdot 0.33 = 6.3 \cdot 10^{-13}$$

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