An excess of `AgNO_3` is added to `100mL` of a `0.01M` solution of dichlorotetraaquachromin (III) chloride. The number of moles of `AgCl` precipitated would be:

Options

A. (a) `0.002`
B. (b) `0.003`
C. (c) `0.01`
D. (d) `0.001`

Answer

D

Explanation

`AgNO_3+[Cr(H_2O)_4Cl_2]ClrarrAgCl+[Cr(H_2O)_4Cl_2]NO_3`
millimole of `AgNO_3` added is
`100xx0.1=1`
`:.` Mole of `AgCl=1xx10^-3=0.001`
(As `AgNO_3` causes ppt of `AgCl` so `AgCl` ppt is `10^-3` moles.)