Question

a mixture of AgCl and AgBr undergoes a loss in wt. by 5% if it is exposed to clorination . the % of AgCl in the mixture was.

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Answer 1

Hi dear

A precipitate of AgCl and AgBr has the mass 0.4066 g. On heating a current of chlorine, the AgBr is converted to AgCl and the mixture loses 0.0725 in mass. The % of mass in the original mixture is (as the nearest integer) :

A6

Solution

Let the mass of AgCl and AgBr in the sample be a and b g respectively,

∴a+b=0.4066...(i)

On passing a current of Cl2 through mixture, AgBr changes to AgCl according to equation :

AgBr−→−Cl2AgCl; whereas AgCl remains unaffected.

∵ 188 g AgBr changes to 143.5 g AgCl.

b g AgBr changes to 143.5×b188 g AgCl

Total mass of AgCl after reaction = initial mass - mass loss

a+143.5×b188=0.4066−0.0725...(ii)

Solving equations (i) and (ii), a=0.1007g,b=0.3059g

Mass of Cl in 0.1007 g AgCl =35.5×0.1007143.5=0.025

% of Cl in mixture =(0.025×100)/0.4066=6.15%

So, answer is 6.

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