What is the mass of the precipitate formed when 50 mL of 16.9 % solution of AgNO 3 is mixed with 50 mL of 5.8 % NaCl solution ? ( Ag =107.8, N =14, O =16, Na =23, Cl =35.5)

Question

What is the mass of the precipitate formed when 50 mL of 16.9 % solution of AgNO 3 is mixed with 50 mL of 5.8 % NaCl solution ? ( Ag =107.8, N =14, O =16, Na =23, Cl =35.5) (A) 7 g (B) 14 g (C) 28 g (D) 3.5 g

Tardigrade Admin · Accepted Answer

16 ⋅ 9 g AgNO 3 is present in 100 mL solution. ∴ 8.45 g AgNO 3 is present in 50 mL solution 5.8 g NaCl is present in 100 mL solution ∴ 2.9 g NaCl is present in 50 mL solution AgNO 3+ NaCl longrightarrow AgCl + NaNO 3 (8 ⋅ 45/170) mol (2.9/58.5) =0 ⋅ 049 mol =0 ⋅ 049 mol arrow 00 after reaction00 arrow 0 ⋅ 049 mol 0 ⋅ 049 mol mass of AgCl precipitated =0.049 × 143.5 g =7 g Ag Cl

Q. What is the mass of the precipitate formed when 50mL of 16.9% solution of AgNO3​ is mixed with 50mL of 5.8%NaCl solution ? (Ag=107.8,N=14,O=16,Na=23,Cl=35.5)

7 g

14 g

28 g

3.5 g

Q. What is the mass of the precipitate formed when $50 m L$ of $16.9%$ solution of $A g N O_{3}$ is mixed with $50 m L$ of $5.8% N a Cl$ solution ?
$(A g = 107.8, N = 14, O = 16, N a = 23, Cl = 35.5)$