In a saturated solution of AgCl, NaCl is added gradually. The concentration of `Ag^(+)` is plotted against the concentration of `Cl^(-)`. The graph appears as :

How much the concentration of Ag^(o+) ions in a saturated solution of AgCI diminish if such an amount of HCI is added to it that the concentration of CI^(Θ) ions in the solution becomes equal to 0.03M ? Also find the amount of AgCI precipitated at the given concentration. K_(sp) of AgCI = 1.8 xx 10^(-10) .

NaCl solution is added to a saturated solution of PbCl_(2). What will happen to the concentration of Pb^(+2) ions?

NaCl solution is added to a saturated solution of PbCl_(2). What will happen to the concentration of Pb^(+2) ions?

NaCI solution is added to a saturated solution of PbCI_2 . What will happen to the concentration of Pb^(+2) ions ?

NaCI solution is added to a saturated solution of PbCI_2 . What will happen to the concentration of Pb^(+2) ions ?

The shape of the curve obtained when substrate concentration is plotted against velocity of reaction

The shape of the curve obtained when substrate concentration is plotted against velocity of reaction

In a saturated aqueous solution of AgBr, concentration of Ag^(+) ion is 1xx10^(-6) mol L^(-1) it K_(sp) for AgBr is 4xx10^(-13) , then concentration of Br^(-) in solution is