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FeSO(4)+NO+H(2)O to...

`FeSO_(4)+NO+H_(2)O to`

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`FeSO_(4)+NO+5H_(2)O to [Fe(NO)(H_(2)O)_(5)]^(2+)SO_(4)^(2-)`
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What is the molarity of a FeSO_(4) . 7H_(2) O solution having 5.56 of it dissolved in 250 mL of water ? ( molar mass =278)

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25 grams of a sample of ferrous sulphate is dissolved in dilute sulphuric acd. By adding water, its volume is made up to 1 litre. 25 mL of this solution requries 20 mL of N//10 KMnO_(4) solution for oxidation. Calculate the percentage of FeSO_(4) . 7H_(2)O in the sample. Strategy: Percentage of FeSO_(4).7H_(2)O =("mass"_("ferrous sulphate"))/("mass of sample")xx100% To get the mass of ferrous suphate, we need to calculate equivalents of ferrous sulphate. By law of equivalrnce, the milli equivalents of KMnO_(4) must be equal to the miliequivalents of ferrous sulphate. We can find the milliequivalents of KMnO_(4) by taking the product of millilitres of solution and its normality.

In 2.6 gm of FeSO_(4).6H_(2)O (At wt of fe =56):