The solubility product of AgCl is 1.8 × 10-10. Precipitation of AgCl will occur by mixing which of the following solutions are mixed in equal volumes?

Question

The solubility product of AgCl is 1.8 × 10-10. Precipitation of AgCl will occur by mixing which of the following solutions are mixed in equal volumes? (A) 10-8 M Ag+ and 10-8 M Cl- ions (B) 10-3 M Ag+ and 10-3 M Cl- ions (C) 10-6 M Ag+ and 10-6 M Cl- ions (D) 10-10 M Ag+ and 10-10 M Cl- ions

Tardigrade Admin · Accepted Answer

For precipitation, ionic product > solubility product In all other options, ionic product is less than solubility product.

Q. The solubility product of $A g Cl$ is $1.8 \times 1 0^{- 10}$ . Precipitation of $A g Cl$ will occur by mixing which of the following solutions are mixed in equal volumes?

$1 0^{- 8} M A g^{+}$ and $1 0^{- 8} M C l^{-}$ ions

$1 0^{- 3} M A g^{+}$ and $1 0^{- 3} M C l^{-}$ ions

$1 0^{- 6} M A g^{+}$ and $1 0^{- 6} M C l^{-}$ ions

$1 0^{- 10} M A g^{+}$ and $1 0^{- 10} M C l^{-}$ ions

For precipitation, ionic product $>$ solubility product In all other options, ionic product is less than solubility product.

Q. The solubility product of AgCl is 1.8×10−10. Precipitation of AgCl will occur by mixing which of the following solutions are mixed in equal volumes?

10−8MAg+ and 10−8MCl− ions

10−3MAg+ and 10−3MCl− ions

10−6MAg+ and 10−6MCl− ions

10−10MAg+ and 10−10MCl− ions