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 ?

When a solid KCI is added to a saturated solution of AgCI "in" H_(2)O ,

Saturated solution of NaCl on heating becomes :

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag^(+) " and " Pb^(+) at a concentration of 0.10M. Aqueous HCl is added to this solution until be Cl^(-) concentration is 0.10M. What will be concentration of Ag^(+) " and " Pb^(2+) be at equilibrium ? ( K_(sp) " for AgCl " = 1.8xx10^(-10) K_(sp) " for " PbCl_(2) = 1.7xx10^(-5) )

Statement-1: No yellow precipitate is formed when an excess of a more concentrated (6M) solution of KI is added to a solution containing Pb^(2+) ions. Statement-2: Solution of [PbI_(4)]^(2-) on dilution with water produces yellow precipitate of PbI_(2) .

In a saturated solution of Ag_(2)CO_(3) , silver ion concentration is 2xx10^(-4) M. Its solubility product is :