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

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]

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

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

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 MgF_(2) in a 0.2 M solution of KF? (K_(sp)=8xx10^(-8))

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

At what ([Br^(-)])/(sqrt([CO_(3)^(2-)]) does the following cell have its reaction at equilibrium? Ag(s)|Ag_(2)CO_(3)(S)|Na_(2)CO_(3)(aq)||KBr(aq)|AgBr(s)|Ag(S) K_(SP)=8xx10^(-12) for Ag_(2)CO_(3) and K_(SP)=4xx10^(-13) for AgBr. (A). sqrt(1)xx10^(-7) (B). sqrt(2)xx10^(-7) (C). sqrt(3)xx10^(-7) (D). sqrt(4)xx10^(-7)

The solubility of AgCl in 0.1M NaCI is (K_(sp) " of AgCl" = 1.2 xx 10^(-10))

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)

It is given that 0.001 mol each of Cd^(2+) and Fe^(2+) ions are contained in 1.0L of 0.02M HC1 solution. This solutions is now saturated with H_(2)S gas at 25^(@)C . a. Determine whether or not each of these ions will be precipitated as sulphide? b. How much Cd^(2+) ions remains in the solution at equilibrium? K_(1)(H_(2)S) = 1.0 xx 10^(-7), K_(2) (H_(2)S) = 1.0 xx 10^(-14) : ltbRgt K_(sp) (CdS) = 8 xx 10^(-27): K_(sp) (FeS) = 3.7 xx 10^(-19) .