314935 Assertion :
Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate \(\mathrm{AgBr}\) rather than \(\mathrm{AgCl}\).
Reason :
\(\mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgCl} < \mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgBr}\).

314936 When different types of salts have nearly same solubility product constant \(\left( {{{\text{K}}_{{\text{SP}}}}} \right)\) which is lesser than \({{\rm{K}}_{{\rm{SP}}}}\) value of one salt, then the most soluble salt is the one

314937 For a sparingly soluble salt \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\), the equilibrium concentrations of \({\mathrm{\mathrm{\mathrm{A}^{2+}}}}\) ions and \({\mathrm{\mathrm{\mathrm{B}^{-}}}}\)ions are \({\mathrm{\mathrm{1.2 \times 10^{-4} \mathrm{M}}}}\) and \({\mathrm{\mathrm{0.24 \times 10^{-3} \mathrm{M}}}}\), respectively. The solubility product of \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\) is

314938 On adding \(0.1 \mathrm{M}\) solution each of \(\left[\mathrm{Ag}^{+}\right],\left[\mathrm{Ba}^{2+}\right],\left[\mathrm{Ca}^{2+}\right]\) in a \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) solution, species first precipitated is \(\left[\mathrm{K}_{\mathrm{sp}}\right.\) of \(\mathrm{BaSO}_{4}=10^{-11}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{CaSO}_{4}=10^{-6}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}=10^{-5}\) ]

314935 Assertion :
Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate \(\mathrm{AgBr}\) rather than \(\mathrm{AgCl}\).
Reason :
\(\mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgCl} < \mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgBr}\).

314936 When different types of salts have nearly same solubility product constant \(\left( {{{\text{K}}_{{\text{SP}}}}} \right)\) which is lesser than \({{\rm{K}}_{{\rm{SP}}}}\) value of one salt, then the most soluble salt is the one

314937 For a sparingly soluble salt \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\), the equilibrium concentrations of \({\mathrm{\mathrm{\mathrm{A}^{2+}}}}\) ions and \({\mathrm{\mathrm{\mathrm{B}^{-}}}}\)ions are \({\mathrm{\mathrm{1.2 \times 10^{-4} \mathrm{M}}}}\) and \({\mathrm{\mathrm{0.24 \times 10^{-3} \mathrm{M}}}}\), respectively. The solubility product of \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\) is

314938 On adding \(0.1 \mathrm{M}\) solution each of \(\left[\mathrm{Ag}^{+}\right],\left[\mathrm{Ba}^{2+}\right],\left[\mathrm{Ca}^{2+}\right]\) in a \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) solution, species first precipitated is \(\left[\mathrm{K}_{\mathrm{sp}}\right.\) of \(\mathrm{BaSO}_{4}=10^{-11}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{CaSO}_{4}=10^{-6}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}=10^{-5}\) ]

314935 Assertion :
Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate \(\mathrm{AgBr}\) rather than \(\mathrm{AgCl}\).
Reason :
\(\mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgCl} < \mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgBr}\).

314936 When different types of salts have nearly same solubility product constant \(\left( {{{\text{K}}_{{\text{SP}}}}} \right)\) which is lesser than \({{\rm{K}}_{{\rm{SP}}}}\) value of one salt, then the most soluble salt is the one

314937 For a sparingly soluble salt \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\), the equilibrium concentrations of \({\mathrm{\mathrm{\mathrm{A}^{2+}}}}\) ions and \({\mathrm{\mathrm{\mathrm{B}^{-}}}}\)ions are \({\mathrm{\mathrm{1.2 \times 10^{-4} \mathrm{M}}}}\) and \({\mathrm{\mathrm{0.24 \times 10^{-3} \mathrm{M}}}}\), respectively. The solubility product of \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\) is

314938 On adding \(0.1 \mathrm{M}\) solution each of \(\left[\mathrm{Ag}^{+}\right],\left[\mathrm{Ba}^{2+}\right],\left[\mathrm{Ca}^{2+}\right]\) in a \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) solution, species first precipitated is \(\left[\mathrm{K}_{\mathrm{sp}}\right.\) of \(\mathrm{BaSO}_{4}=10^{-11}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{CaSO}_{4}=10^{-6}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}=10^{-5}\) ]

314935 Assertion :
Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate \(\mathrm{AgBr}\) rather than \(\mathrm{AgCl}\).
Reason :
\(\mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgCl} < \mathrm{K}_{\mathrm{sp}}\) of \(\mathrm{AgBr}\).

314936 When different types of salts have nearly same solubility product constant \(\left( {{{\text{K}}_{{\text{SP}}}}} \right)\) which is lesser than \({{\rm{K}}_{{\rm{SP}}}}\) value of one salt, then the most soluble salt is the one

314937 For a sparingly soluble salt \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\), the equilibrium concentrations of \({\mathrm{\mathrm{\mathrm{A}^{2+}}}}\) ions and \({\mathrm{\mathrm{\mathrm{B}^{-}}}}\)ions are \({\mathrm{\mathrm{1.2 \times 10^{-4} \mathrm{M}}}}\) and \({\mathrm{\mathrm{0.24 \times 10^{-3} \mathrm{M}}}}\), respectively. The solubility product of \({\mathrm{\mathrm{\mathrm{AB}_{2}}}}\) is

314938 On adding \(0.1 \mathrm{M}\) solution each of \(\left[\mathrm{Ag}^{+}\right],\left[\mathrm{Ba}^{2+}\right],\left[\mathrm{Ca}^{2+}\right]\) in a \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) solution, species first precipitated is \(\left[\mathrm{K}_{\mathrm{sp}}\right.\) of \(\mathrm{BaSO}_{4}=10^{-11}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{CaSO}_{4}=10^{-6}, \mathrm{~K}_{\mathrm{sp}}\) of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}=10^{-5}\) ]