2.5 grams of a metallic sample containing an unknown amount of zinc is dissolved in 500...

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Chemistry

2.5 grams of a metallic sample containing an unknown amount ofzinc is dissolved in 500 ml of acidic water, releasing the zincinto the water as Zn²⁺ ions. A 10.00 ml aliquot of thissolution is extracted with 10 ml of CCl₄ containing anexcess of 8-hydroxy quinoline. The CCl₄ and aqueousphases separate and 8-hydroxy quinoline forms a fluorescent complexwith Zn²⁺ ions that partitions entirely into theCCl₄ phase. The CCl₄ phase is separated andthen diluted to 25 ml. This solution gives a fluorescence intensityof 155 (arbitrary units). A similar procedure is done with 10.00 mlof the unknown zinc solution plus 8.00 ml of an aqueous 2.50 ppmZn²⁺ solution, and the final fluorescence intensity is247. Calculate the Zn²⁺ concentration in the original500 ml solution and the amount of zinc in the original solid.

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Ans Given Fluorescence intensity of unknown Zn2 solution 155 units Fluorescence intensity of unknown Zn2 Standard solution 247 units Increase in fluorescence intensity 247 155 unit 92 units Conclusion Increase in Fluorescence intensity of 92 units is due to addition of 80 mL of standard Zn2 solution of See Answer

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