Answer:
The mass of PbCl₂ is 45.88 grams and the mass of AgCl is 16.48 grams.
Explanation:
As mentioned in the given question, the addition of 0.275 L of 1.62 M KCl is done in a solution that comprise Ag⁺ and Pb²⁺ ions so that all the ions get precipitated. Therefore, the moles of KCl present is,
Moles of KCl = 0.275 L × 1.62 M = 0.445 moles
Now the reaction will be,
Ag⁺ + Pb²⁺ + KCl ⇒ AgCl + PbCl₂ + 3K⁺
Now let us assume that the formation of x moles of AgCl and y moles of PbCl₂ is taking place.
Therefore, mass of AgCl will be x × molecular mass, which will be equal to x × 143.32 grams = 143.32 x grams
Now the mass of PbCl2 formed will be,
y × molecular mass = y × 278.1 grams = 278.1 y grams
Now the total precipitate will be,
62.37 grams = 143.32 x + 278.1 y -----------(i)
Now as AgCl and PbCl₂ requires 1:2 ratio of KCl, this shows that x moles of AgCl will require x moles of KCl and y mol of PbCl₂ will require 2*y moles of PbCl₂. Therefore,
x + 2y = total mass of KCl
x + 2y = 0.445 moles ------ (ii)
On solving equation (i) and (ii) we get,
x as 0.115 and y as 0.165
Now the mass of AgCl will be,
143.32 × 0.115 = 16.48 grams
The mass of PbCl₂ will be,
278.1 × 0.165 = 45.88 grams.
