Find the concentration of ion which is first precipitated at the point when the third ion starts precipitating, if $AgNO_3$ is added gradually to the solution that contains $0 .1\ M\  Cl^-, 0 .1\  M\ Br^-$ and $0. 1\ M\ I^-$

Given that

Salt            ||         $K_{sp}$

$AgCl$        ||        $2 \times {10^{ – 10}}$

$AgBr$       ||       $5 \times {10^{ – 13}}$

$Ag$           ||        $9 \times {10^{ – 17}}$

Solid Lead nitrate is dissolved in $1\,litre$ of water. The solution was found to boil at $100.15^{\circ}\,C$. When $0.2\,mol$ of $NaCl$ is added to the resulting solution, it was observed that the solution froze at $-0.8^{\circ}\,C$. The solutbility product of $PbCl _2$ formed is $………..\times 10^{-6}$ at $298\,K$. (Nearest integer) Given : $K _{ b }=0.5\,K\,kg\,mol ^{-1}$ and $K _{ f }=1.8\,kg\,mol ^{-1}$. Assume molality to be equal to molarity in all cases.

At temperature $T$ a compound $AB_2(g)$ dissociates according to the reaction with a degree of dissociation $'x'$ which is very small compared to unity. The value of $x$ is 

$2A{B_2}(g) \rightleftharpoons 2AB(g) + {B_2}(g)$

For a sparingly soluble salt ${A_p}{B_q},$ the relationship of its solubility product $({L_S})$ with its solubility $(S)$ is

Concentration of the $Ag^+$ ions in a saturated solution of $Ag_2C_2O_4$ is $2.2 \times 10^{-4}\, mol\, L^{-1} .$ Solubility product of $Ag_2C_2O_4$ is