In the crystallisation of `71.75` grams of `AgCl`, in molten state `1 xx 10^(4)` mole of cadmium chloride is added to cause impurity defect. Calculate (a) the number of `Ag^+` ions present, (b) the number of Cd2+ ions present and (c) the number of lattice vacancy defects.

Explanation

Number of moles of `Ag^+= ` number of moles of `AgCl = (71.75) /( 143.5) = 0.5`
Original number of `Ag^(+)` ions in the given crystalline substance
`=0.5 xx 6.023 xx 10^(23) = 3.011 5 xx 10^(23)`
Number of `Cd^(2+)` ions added
`=1 xx 10^(-4) xx6.023 xx 10^(23) = 6.023 xx 10^(19)`
Number of `Ag^(+)` ions removed
`=2 xx 6.023 xx 10^(19) = 1.2046 xx 10^(20)`
Number of lattice vacancies created in the given crystal
`=6.023 xx 10^(19) `
Number of `Ag^+` ions present in the defected crystal
`=3.0115 xx 10^(23) -1.2046 xx 10^(20) =3.0103 xx 10^(23)`