For a saturated solution of Ag2CrO4 (K_sp = 1.1 x 10^-12) at 298 K, choose the correct statement(s).

K_sp = 4s^3, where s is the molar solubility

Adding solid K2CrO4 shifts the equilibrium towards the solid and lowers [Ag^+]

K_sp = 4s^3, where s is the molar solubility

Its solubility in 0.1 M AgNO3 is 1.1 x 10^-11 M

Adding solid K2CrO4 shifts the equilibrium towards the solid and lowers [Ag^+]

JEE Main levelOne or more correct optionsDifficulty 2 of 3ie195

For a saturated solution of $Ag X_{2} CrO X_{4}$ ( $K_{s p} = 1.1 \times 1 0^{- 12}$ ) at 298 K, choose the correct statement(s).

A $[Ag X^{+}]$ equals $2 [CrO X_{4} X^{2 -}]$
B $K_{s p} = 4 s^{3}$ , where $s$ is the molar solubility
CIts solubility in $0.1 M$ $AgNO X_{3}$ is $1.1 \times 1 0^{- 11}$ $M$
DAdding solid $K X_{2} CrO X_{4}$ shifts the equilibrium towards the solid and lowers $[Ag X^{+}]$

In pure water

[Ag X^{+}] = 2 s

and

[CrO X_{4} X^{2 -}] = s

, so

K_{s p} = 4 s^{3}

. Added chromate is a common ion and lowers

[Ag X^{+}]

. In

0.1 M

AgNO X_{3}

s = K_{s p} / (0.1)^{2} = 1.1 \times 1 0^{- 10} M

, not

1.1 \times 1 0^{- 11}