What is the mass of precipitate formed when 50 ml of 8.5% solution of `AgNO_3` is mixed with 100 ml of 1.865% potassium chloride solution?

Options

A. 3.59 g
B. 7 g
C. 14 g
D. 28 g

Answer

A

Explanation

`AgNO_3 + KCl to KNO_3 + AgCl`
50 mL of 8.5% solution contains 4.25 g of `AgNO_3`
Number of moles of `AgNO_3` present in 50mL of 8.5% of `AgNO_3`
Number of moles of `AgNO_3` present in 50 mL of 8.5% `AgNO_3` solution.
=Mass/Molar mass = 4.25/170
= 0.05 moles
Similary, number of moles of KCl present in 100 mL of 1.865% KCl solution.
`=1.865 //74.5 =0.025` moles
So total amount of AgCl formed is 0.025 moles (based on the stoichiometry )
Amount of AgCl present in 0.025 moles of AgCl
=No. of moles `xx` molar mass
`=0.025 xx 143.5 = 3.59 g`