17 g of AgNO 3 solution is mixed with 400 ml of 0.2 M HCl solution then how many gram of AgCl will be precipitated: [ Ag =108, Cl =35.5, N =14, O =16]

Question

17 g of AgNO 3 solution is mixed with 400 ml of 0.2 M HCl solution then how many gram of AgCl will be precipitated: [ Ag =108, Cl =35.5, N =14, O =16] (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/8e992ce46693ec464d790f62db7dd01b-.png" /> ∴ moles =(80/1000) × 143.5=11.48

Q. $17 g$ of $A g N O_{3}$ solution is mixed with $400 m l$ of $0.2$ $M H Cl$ solution then how many gram of $A g Cl$ will be precipitated: $[A g = 108, Cl = 35.5, N = 14, O = 16]$

$∴$ moles $= \frac{80}{1000} \times 143.5 = 11.48$

Q. 17g of AgNO3​ solution is mixed with 400ml of 0.2 MHCl solution then how many gram of AgCl will be precipitated: [Ag=108,Cl=35.5,N=14,O=16]

∴ moles =100080​×143.5=11.48

Q. $17 g$ of $A g N O_{3}$ solution is mixed with $400 m l$ of $0.2$ $M H Cl$ solution then how many gram of $A g Cl$ will be precipitated: $[A g = 108, Cl = 35.5, N = 14, O = 16]$

$∴$ moles $= \frac{80}{1000} \times 143.5 = 11.48$