A mixture is prepared by combining 11.34 mL of 2.36 x 103 M Fe(NO3)3 with 10.00 mL of 1.66 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the[FESCN2*] at equilibrium is found to be 2.20 x 10-4 M.Complete the following ICE tableFe3+SCN1tFESCN2+initial (M)(A)(B)(C)0change (M)(D)(E)(F)equilibrium (M)(G)(H)(1)What is the value of K?

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 64QRT

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2. An iron ore was analyzed by dissolving a 1.1324 g sample in concentrated HC. The resulting solution was diluted with water, and the iron(III) was precipitated as hydrous oxide Fe,03 .XH20 by the addition of NH3. After filtration and washing, the residue was ignited at a high temperature to give 0.5394 g of pure Fe,03 (FW = 159.69). Calculate (a) the percent Fe (FW = 55.847) and (b) the percent Fe;04 (FW = 231.54) in the sample.
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For the aqueous [Hg14] complex K₁=6.76 × 10²⁹ at 25 °C. 2+ Suppose equal volumes of 0.0066M Hg(NO3), solution and 0.78M KI solution are mixed. Calculate the equilibrium molarity of aqueous Hg²+ ion. Round your answer to 2 significant digits. M x10 X ? Ś
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