Question
In: Chemistry
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.
Solutions
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%
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