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A fajans titration of a 0.9628 g sample containing chloride required 31.32 ml of 0.1001 M...

A fajans titration of a 0.9628 g sample containing chloride required 31.32 ml of 0.1001 M AgNO3. Express the result of this analysis in terms of the percent AlCl3 (FW= 133.34) in the sample.

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Expert Solution

no of mole of AgNo3 added = 31.32/1000*0.1001 = 0.00313 mole

AgNO3(aq) + Cl^-(aq) ----> AgCl(s) + NO3^- (aq)

no of mole of Cl^- present in solution =  no of mole of AgNo3 added = 0.00313 mole

no of mole of AlCl3 present = 0.00313/3 = 0.00104 mole

mass of AlCl3 present   = n*Mwt

                                   = 0.00104*133.34

                                   = 0.14 g

% of AlCl3 present in sample = weight of AlCl3 / sample weight * 100

                                                        = 0.14/0.9628*100

                                                     = 14.54%

queen_honey_blossom answered 1 year ago
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