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» 3.59 G 7 g 14 g 28 g Solution :`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`