A sample containing potassium chloride and inert material wasanalyzed by the Moh

Question

A sample containing potassium chloride and inert material wasanalyzed by the Mohr method. A portion of the solid weighing 0.2500g was dissolved and titrated with 0.07575 M AgNO3solution to a brick-red silver chromate end point. If the titrationconsumed 43.22 mL of the AgNO3 solution, what is theweight percent chloride (35.45 g/mol) in the sample? What is theweight percent KCl (74.55 g/mol) in the sample?

The answer should be 46.44% Cl & 97.64% KCl, but I really needto know how to solve it, any help would be appreciated. Thanks.

Explanation / Answer

Ag^+ (aq) + Cl^-(aq) ..............> AgCl(s) At equilivelence point: moles of Ag^+ = moles of Cl^- (0.07575M)(43.22mL) = moles of Cl^- moles of Cl^- = 3.2739m mol Mass of Cl^- present = 3.2739m mol * (35.45g / mol) =0.1161g Hence, mass percent of Cl^- = (0.1161 g / 0.2500g)*100 =46.44% Mass of KCl = (3.2739m mol)(74.55g/mol) = 0.2441g Hence, mass percent = (0.2441g / 0.2500g )*100 =97.64%

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