Precipitation reaction

Question

Calculate the ksp value and the mass of precipitated Agcl when 10 mL of 0.01 Μ AgNO3 and 10 mL of 0.0001 Μ NaCl solutions are mixed?
Please explain step by step

Answer 1

AgCl ==> Ag⁺ + Cl^-

Ksp = [Ag+][Cl-] where [Ag+] and [Cl-] are the molar solubilities of AgCl which you need to look up under “solubility of silver chloride”. Plug that number in and solve for Ksp. 

 

Mass AgCl ppt formed:

find moles of Ag and moles of Cl present. Note: moles Cl will be limiting because conc of NaCl is musc lower than that of AgNO3. Convert to moles/L and subtract the molar solubility used in the previous step. Finally convert that value to grams using molar mass of AgCl.