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. 3.59g
B. 77g
C. 14g
D. 28g

Answer

A

Explanation

`AgNO_(3) + KCl to KNO_(3) + AgCl`
50 mL of 8.5% solution contains 4.25 g of `AgNO_(3)`
No. of moles of `AgNO_3` present in 50 mL of 8.5% `AgNO_3` solution
= Mass / Molar mass = 4.25 / 170
= 0.025 moles
Similarly, No of moles of KCI present in 100 mL of 1.865% KCI solution
= 1.865/74.5 = 0.025 moles
So total amount of AgCI formed is 0.025 moles (based on the stoichiometry)
Amount of AgCI present in 0.025 moles of AgCI
= no. of moles `xx` molar mass = `0.025 xx 143.5 = 3.59 g`