[" Ouestion No."36],[" If the solubility products of AgCl and AgBr are "1.0times10^(-8)M" and "3.5times10^(-13)" respectivell,then the correct relation bemeen th "],[" 's') of these salts is."]

The solubility products of AgCl and Ag_2CrO_4 are 1.5 xx 10^(-10) and 9 xx 10^(-12) respectively. Which of the following statement is correct ?

Consider the cell Ag|AgBr(s)Br^(-)||AgCl(s)Cl^(-)|Ag at 298 K the solubility product of AgCl and AgBr are 1xx10^(-10) and 5xx10^(-13) respectively. What should be the ratio of concentration of Br^(-) and Cl^(-) by which emf of the cell becomes zero?

Solubility products of Ag_2 CrO_4 and AgCl are 9 xx 10^(-12) and 1 xx 10^(-10) respectively at 298. Concentration of Ag^(+) is more in the saturated solution of which salt?

Calculate the simultaneous solubility of AgSCN and AgBr. K_(sp) for AgSCN and AgBr are 1 xx 10 ^(-12) and 5 xx 10 ^(-13) respectively.

If the solubility of AgCl in 0.1 M NaCl is ( K_(sp) of AgCl = 1.2 xx 10^(-10) )

The solubility product of salt AB is 1 xx 10^(-8) In a solution in which concertration of A is 10^(-3) M . The AB will precipitate when the concentration of B becomes.

The solubility of AgCl (K_(ap) = 1.2 xx 10^(-10)) in a 0. 10 M NaCl solution is