Calculate the concentration of silver ion, if water is saturated with AgCNS (K_(sp) =1 xx 10^(-12)) and AgBr (K_(sp) = 5 xx 10^(-13) ).
What is the molar solubility of Fe(OH)_2 (K_(sp) =8.0 xx 10^(-16) ) at pH 13.0 ?
The specific conductance of a saturated solution of a salt MX is 2.8 xx 10^(-7) Omega^(-1) cm^(-1) and the equivalent conductances at infinite dilution of M^(+1) and X^(-1) ions are 68 and 72 Omega^(-1) cm2 / equivalent respectively Hence, the K_(sp) of MX is found to be
What is the minimum pH required to prevent the precipitation of Zn^(+2) in a solution that is 0.01 M ZnCl_(2) and saturated with 0.1 M H_(2) S (Given : K_(sp) ZnS = 10^(-21) and Ka_(1) xx Ka_(2) of H_(2)S = 10^(-20) )
A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product (K_(sp)) . For the electrolyte, A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-) , with solubility S, the solubility product (K_(sp)) =x^(x)xxy^(y) xx s^(x+y) . While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its K_(sp) , value at a particular temperature, then precipitation occurs. The solubility of BaSO_(4) , in 0.1 M BaCl_(2) , solution is (K_(sp) , of BaSO_(4), = 1.5 xx 10^(-9))
Sparingly soluble salts maintains their solubility product value in their saturated solutions irrespective of the sources of the ions . what is the molar solubility of AgNO_3 in a 0.1 M H_2S solution buffered at pH= 2 (K_1 and K_2 " of " H_2S " are " 10^(4) and 10^(-8) respectively) (K_(sp) " of " Ag_2S = 4xx 10^(-13) ) (Note : No Ag_2S precipitate should be formed)
if 500 mL of 0.4 M AgNO_3 is mixed with 500 mL of 2M NH_3 solution the what is the concentration of Ag (NH_3 ) ^(+) in solution? [Given : K_(f_1) [Ag (NH_3) ^(+)] =10 ^(3) , K _(f_2) [Ag (NH_3)_2^(+) ]= 10^(4) ]
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
