What is the mass of the precipitate formed when 50 mL of $16.9\mathrm{\%}$ solution of $\mathrm{A}\mathrm{g}\mathrm{N}{\mathrm{O}}_3$ is mixed with 50 mL of $5.8\mathrm{\%}$ NaCl solution?

(Ag = 107.8, N = 14, O = 16, Na = 23, Cl = 35.5)

• A

  28 g
• B

  3.5 g
• Correct answer
  C

  7 g
• D

  14 g

Solution

$16.9\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{A}\mathrm{g}\mathrm{N}{\mathrm{O}}_3$ is present in 100 mL solution.

$\therefore 8.45\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{A}\mathrm{g}\mathrm{N}{\mathrm{o}}_3$ is present in 50 mL solution

5.8 g NaCl is present in 100 mL solution

$\therefore 2.9\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{N}\mathrm{a}\mathrm{C}\mathrm{l}$ is present in 50 mL solution



Mass of AgCl

$=0.049\times 143.5\mathrm{ }\mathrm{g}$

$=7\mathrm{ }\mathrm{g}\mathrm{ }\mathrm{A}\mathrm{g}\mathrm{C}\mathrm{l}$

Hence, the correct answer is option: 'C'.