A solution contains 0.010 M each of Cl-, Br- and I-. Solid AgNO3 is added slowly (no volume change). K_sp: AgCl 1.8 x 10^-10, AgBr 5.0 x 10^-13, AgI 8.5 x 10^-17. Select the correct statement(s).

AgI precipitates first, followed by AgBr and then AgCl

AgCl begins to precipitate at [Ag+] = 1.8 x 10^-8 M

When AgBr just starts to precipitate, [I-] left is about 1.7 x 10^-6 M

AgI precipitates first, followed by AgBr and then AgCl

AgCl begins to precipitate at [Ag+] = 1.8 x 10^-8 M

When AgCl just starts to precipitate, [Br-] left is less than 10^-5 M

When AgBr just starts to precipitate, [I-] left is about 1.7 x 10^-6 M

JEE Main levelOne or more correct optionsDifficulty 2 of 3ia065

A solution contains $0.010 M$ each of $Cl X^{-}$ , $Br X^{-}$ and $I X^{-}$ . Solid $AgNO X_{3}$ is added slowly (no volume change). $K_{s p}$ : $AgCl$ $1.8 \times 1 0^{- 10}$ , $AgBr$ $5.0 \times 1 0^{- 13}$ , $AgI$ $8.5 \times 1 0^{- 17}$ . Select the correct statement(s).

A $AgI$ precipitates first, followed by $AgBr$ and then $AgCl$
B $AgCl$ begins to precipitate at $[Ag X^{+}] = 1.8 \times 1 0^{- 8} M$
CWhen $AgCl$ just starts to precipitate, $[Br X^{-}]$ left is less than $1 0^{- 5} M$
DWhen $AgBr$ just starts to precipitate, $[I X^{-}]$ left is about $1.7 \times 1 0^{- 6} M$

Start of precipitation needs

[Ag X^{+}] = K_{s p} /0.010

1.8 \times 1 0^{- 8}

M (

AgCl

5.0 \times 1 0^{- 11}

M (

AgBr

8.5 \times 1 0^{- 15}

M (

AgI

), so the order is

AgI

AgBr

AgCl

. At

[Ag X^{+}] = 1.8 \times 1 0^{- 8}

[Br X^{-}] = 2.8 \times 1 0^{- 5}

M, which is more than

1 0^{- 5}

M, so the third statement is false. At

[Ag X^{+}] = 5.0 \times 1 0^{- 11}

[I X^{-}] = 1.7 \times 1 0^{- 6}