An excess of AgNO₃ is added to 100 mL of a 0.05 M solution of tetraaquadichloridochromium (III) chloride. The number of moles of AgCl precipitated will be __________ 10⁻³ . (Nearest integer)

Step-by-step solution

The formula of tetraaquadichloridochromium (III) chloride is [Cr(H₂O)₄Cl₂]Cl . In this complex, there is one ionizable chloride ion present outside the coordination sphere. The dissociation reaction is: [Cr(H₂O)₄Cl₂]Cl [Cr(H₂O)₄Cl₂]^+ + Cl^- Number of moles of the complex = M V = 0.05 100 1000 = 0.005 moles. Since one mole of the complex yields one mole of chloride ions, the number of moles of Cl^- ions produced is 0.005 moles. When excess AgNO₃ is added, the chloride ions precipitate as AgCl : Ag^+ + Cl^- AgCl Num