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?

What is the mass of precipitate formed when 50 ml of 8.5% solution of

1.	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?
Answer» 3.59g 77g 14g 28g SOLUTION :`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`