The molar mass of a sparingly soluble salt \( \left( MX _{2}\right) \) is \( 100 g mol ^{-1} .0 .4 g \) of the salt is required to prepare a saturated solution with water at \( 25^{\circ} C \). Choose the correct statement(s) from the following the molar solubility product constant \( \left(K_{s p}\right) \) of the salt is \( 256 \times 10^{-9} mol L^{-1} \) the molarity of the saturated solution of the salt is \( 0.4 M \) the salt will precipitate as \( MX _{2} \) (s), if \( 500 mL \) of \( 10^{-4} M ^{\prime} MCl _{2} \) ' solution is mixed with \( 500 mL \) of \( 10^{-4} M \) ' \( NX \) ' solution. \( \left[ MCl _{2}\right. \) and \( NX \) are completely ionized in water \( ] \) The molarity of \( X \) ions in the saturated solution is \( 0.008 M \)

Question

The molar mass of a sparingly soluble salt \( \left( MX _{2}\right) \) is \( 100 g mol ^{-1} .0 .4 g \) of the salt is required to prepare a saturated solution with water at \( 25^{\circ} C \). Choose the correct statement(s) from the following the molar solubility product constant \( \left(K_{s p}\right) \) of the salt is \( 256 \times 10^{-9} mol L^{-1} \) the molarity of the saturated solution of the salt is \( 0.4 M \) the salt will precipitate as \( MX _{2} \) (s), if \( 500 mL \) of \( 10^{-4} M ^{\prime} MCl _{2} \) ' solution is mixed with \( 500 mL \) of \( 10^{-4} M \) ' \( NX \) ' solution. \( \left[ MCl _{2}\right. \) and \( NX \) are completely ionized in water \( ] \) The molarity of \( X \) ions in the saturated solution is \( 0.008 M \)