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The solubility product of silver sulphate is 2.3 × 10-5. Calculate the concentration of Ag+ in the saturated solution of salt containing 1.8 × 10-2 moles/dm3 of SO42- ions. |
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Answer» Ksp = 2.3 x 10-5 [SO4-] = 1.8 x 10-2 Ag2SO4 \(\rightleftharpoons\) 2Ag+ + SO4-2 Ksp = [Ag+]2[SO4-2] \(\therefore\) [Ag+]2 = \(\frac{K_{sp}}{[SO_4^{-2}]}\) [Ag+]2 = \(\frac{2.3\times10^{-5}}{1.8\times10^{-2}}\) = 1.28 x 10-3 or [Ag+]2 = 12.8 x 10-4 [Ag+] = \(\sqrt{12.8\times10^{-4}}\) = 3.58 x 10-2 M or [Ag+] = 0.0358 M |
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