Solubility of `BaF_(2)` in a solution of `Ba(NO_(3))_(2)`, will be represented by the concentration term:

The solubility of CaF_(2) in a solution of 0.1M Ca(NO_(3))_(2) is

The solubility of CaF_(2) in a solution of 0.1M Ca(NO_(3))_(2) is

The solubility product of a soluble salt A_(x)B_(y) is given by: K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y) . As soon as the product of concentration of A^(y+) and B^(x-) increases than its K_(SP) , the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in 0.1M NaCI or 0.1M AgNO_(3) solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases. Which of the following statement is wrong ? (1) K_(SP) of a salt depends upon temperature (2) K_(SP) of a salt has no units (3) The K_(SP) of salt A_(x)B_(y) can be given as: x^(x).y^(y)(S)^(x+y) (4) Solubility of BaF_(2) in a solution of Ba(NO_(3))_(2) can be given by (1)/(2)[F^(-)]

Solubility product of Ba(OH)_2 is 5.01×10^(-7) ,pOH of saturated solution of Ba(OH)_2 is

STATEMENT-1: Solubility product of BaF_(2) will increase on dilution. STATEMENT-2: Solubility of BaF_(2) will change on changing temperature.

STATEMENT-1: Solubility product of BaF_(2) will increase on dilution. STATEMENT-2: Solubility of BaF_(2) will change on changing temperature.

Solubility product of Ba(OH)_2 is 5.0.* 10^(-7) . pOH of saturated solution of Ba(OH)_2 is

Solid Ba(NO_(3))_(2) is gradually dissolved in a 10^(-4)M Na_(2)CO_(3) solution. At what concentration of Ba^(2+) will a precipitate begin to form ? ( K_(sp) for BaCO_(3)=5.1xx10^(-9) )

100 ml of 0.2"M H"_(2)SO_(4) solution is mixed with 400ml of 0.05"M Ba"_(3)(PO_(4))_(2) . Calculate the concentration of [Ba^(+2)] ion in resulting solution.