`A_(3)B_(2)` is a sparingly soluble salt with molar mass `M(gmol^(-))` and solubility `x` gm `litre^(-1)`, the ratio of the molar concentration of `B^(3-)` to the solubilty product of the salt is `:-`
At a certain temperature ,the solubility of the salt M_m A_n in water is .s. moles per litre. The solubility product of the salt is
The electrochemical cell shown below is a concentration cell. M|M^(2+) (saturated solution of a sparingly soluble salt, MX_2 || M^(2+) (0.001 mol dm^(-3) ) |M The emf of the cell depends on the difference in concentration of M^(2+) ions at the two electrode The emf of the cell at 298 is 0.059 V The solubility product (K_(sp) , mol^(3) dm^(-9)) of MX_2 at 298 based on the information available the given concentraiton cell is (take 2.303 xx R xx 298 // F = 0.059 V )
The electrochemical cell shown below is a concentration cell. M|M^(2+) (saturated solution of a sparingly soluble salt, MX_2 || M^(2+) (0.001 mol dm^(-3) ) |M The emf of the cell depends on the difference in concentration of M^(2+) ions at the two electrode The emf of the cell at 298 is 0.059 V The value of DeltaG (kJ " mol"^(-1)) for the given cell is ( take 1F = 96500 C " mol"^(-1) )
The molar solubility in mol. lit^(-1) of a sparingly soluble salt MX_(4) , is S. The corresponding solubility product K_(sp) , is given by the relation
The solubility of A_(2)B=2xx10^(-3) "mol" L^(-1) . What is solubility product?
If the solubility of alum KAl(SO_4 )_2 is 2 xx 10^(-3) M, what its solubility product ?
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?
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
