The solubility of `Fe(OH)_(3)` would be maximum in :

Calculate the molar solubility of Fe(OH)_(3) in a buffer solution that is 0.1M in NH_(4)OH and 0.1M in NH_(4)Cl (K_(b) of NH_(4)OH=1.8xx10^(-5) , K_(sp) of Fe(OH)_(3)=2.6xx10^(-39) )

The solubility product of Fe(OH)_3 at 298K is 1.1 xx 10^(-36) . Find its solubility in kgdm^-3 at the same temperature. (Given: At Wts. Fe = 56, O =16, H =1).

The solubility of Al(OH)_3 is 's' mol per litre, the solubility product of Al(OH)_ 3 is :

What is the solubility (in mol/L) of Fe(OH)_3 in a solution of pH= 8.0 ? [K_(sp)" for "Fe(OH)_3= 1.0 xx 10^(-36)]

If the solubility of Ca(OH)_(2) is sqrt3 , What is its solubility product ?

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

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 298 K, the K_(xp) value of Fe(OH)_(3) , in aqucous solution is 3.8 xx 10^(-38) . The solubility of Fe^(3+) ions will increase when