Question

write the material balance chart for the reaction between 125 ml of 0.200 M Silver Nitrate and 75.0 ml of 0.200 M Hydrochloric acid

Answer 1

the reaction is

AgNO3(aq)+HCl (aq) ----->AgCl(s) + HNO3(aq)

1 moles of AgNO3 reacts with 1 mole of HCl to produce 1 mole of AgCl (s) and 1 mole of HNO3.

moles of AgNO3= molarity* volume in   L=0.2*125/1000=0.025 , moles of HCl = molarity*volume in L=0.2*75/1000 = 0.015

mass of reactants : AgNO3 = moles* molar mass =0.025*170 gm=4.25 gm, mass of HCl =moles of HCl* molar mass of HCl =0.015*36.5 gm =0.5475 gm

masses entering : AgNO3=4.25 gm, HCl=0.5475 gm

total mass entering =4.25+0.5475 =4.7975 gm

theoretical molar ratio of     AgNO3: HCl = 1:1 , actual molar ratio =0.025:0.015

hebce excess is AgNO3 and limiting reactant is HCl. moles of Ag Cl= moles of   HNO3=0.015

mass of AgCl formed = moles* molar mass of AgCl =0.015*143.3 =2.1495 gm, mass of HNO3= moles* molar mssd=0.015*63= 0.945 gm

moles of AgNO3 remaining = moles of AgNo3 supplied- moles of AgNO3 used= 0.025-0.015=0.01, mass of AgNO3= moles*molar mass =0.01*170=1.7 gm

mass of products (gm): AgCl= 2.1495, HNO3= 0.945, AgNO3 =1.7 gm

total mass of products= 2.1495+0.945+1.7 =4.7945 gm

law of conservation of mass states that mass can neither be created nor be created. in this case, mass entering = mass leaving under steady state conditions