Which of the following is most soluble? `Bi_(2)S_(3)` `(K_(sp)=1times10^(-70)) ``MnS(K_(sp)=7times10^(-16)) ``CuS(K_(sp)=8times10^(-45)) ``Ag_(2)S(K_(sp)=6times10^(-51)) `

Some chemists at wished to perpare a saturated solution of a silver compound and they wanted it to have the highest concentration of silver ion possible. Which of the following compound would they use ? K_(sp) (AgCI) = 1.8 xx 10^(-10), K_(sp) (AgBr) = 5.0 xx 10^(-13) , K_(sp) (Ag_(2)CrO_(4)) = 2.4 xx 10^(-12) ["Use" 3sqrt(0.6) = 0.84]

A 1 litre solution containing NH_(4)Cl and NH_(4)OH has hydroxide ion ion concentration of 10^-6) mol//litre. Which of the following hydroxides could be precipitated when the solution is added to 1 litre solution of 0.1 M metal ions? (I) Ba(OH)_(2)(K_(sp)=5xx10^(-3)) , (II) Ni(OH)_(2)(K_(sp)=1.6xx10^(-16)) (III) Mn(OH)_(2) (K_(sp)=2xx10^(-13)) , (IV) Fe(OH)_(2) (K_(sp)=8xx10^(-16))

What is the molar solubility of Fe(O)_(2) (K_(sp)=8.0xx10^(-16)) at pH 13.0 ?

What is the pH of a saturated solution of Cu(OH)_(2) ? (K_(sp)=2.6xx10^(-19)

Compare the solubility of Fe(OH)_(3) (K_(sp) = 4 xx 10^(-38)) and Ni(OH)_(2).(K_(sp) = 2 xx 10^(-16)) at pH = 5.0

Three suggestion are made for ways to removes silver ions from solution: a. Make the solution 0.01M in Nal . b. Buffer the solution at pH = 13 . c. Make the solution 0.01M Na_(2)S . What will be the equilibrium silver ion concentartion in each case? which course of action is most effective in removing Ag^(o+) ions? K_(sp) (AgI) = 8.5 xx 10^(-17), K_(sp) (AgOH) = 2 xx 10^(-8) , K_(sp) (Ag_(2)S) = 5.5 xx 10^(-51)

Assertion (A): A solution contains 0.1M each of pB^(2+), Zn^(2+),Ni^(2+) , ions. If H_(2)S is passed into this solution at 25^(@)C . Pb^(2+), Ni^(2+), Zn^(2+) will get precpitated simultanously. Reason (R): Pb^(2+) and Zn^(2+) will get precipitated if the solution contains 0.1M HCI . [K_(1) H_(2)S = 10^(-7), K_(2)H_(2)S = 10^(-14), K_(sp) PbS =3xx 10^(-29) K_(sp) NiS = 3 xx 10^(-19). K_(sp) ZnS = 10^(-25)]

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

If the solubility of Ag_(2)SO_(4) in 10^(-2)M Na_(2)SO_(4) solution be 2xx10^(-8)M then K_(sp) of Ag_(2)SO_(4) will be

On adding 0.1 M solution each of Ag^(+),Ba^(2+), Ca^(2+) ions in a Na_(2)SO_(4) solution, species first precipitated is (K_(sp)BaSO_(4)=10^(-11),K_(sp)CaSO_(4)=10^(-6),K_(sp) Ag_(2)SO_(4)=10^(-5))