Question

A solution containing 0.1 mol of a metal chloride $MC{l}_x$ required 500 ml of 0.8 m $AgN{O}_3$ solution for complete reaction $MC{l}_x+xAgN{O}_3\to xAgCl+M(N{O}_3{)}_x$. Then the value of x is :

• A. 1
• B. 2
• C. 4
• D. 3

Answer 1

Answer: (C)

4

$no.molesofAgN{O}_3=volme\ast Molarity=0.5\ast 0.8=0.4$
0.1 mol of a metal chloride $MC{l}_x$ required 0.4 mols of $AgN{O}_3$ to complete the reaction.
Then the mole ratio between $MC{l}_x:AgN{O}_3=1:x=1:4$
$\therefore x=4$