`Fe(OH)_(2)` is diacidic base has `K_(b1)=10^(-4)` and `K_(b2)=2.5xx10^(-6)` What is the concentration of `Fe(OH)_(2)` in 0.1 M `Fe(NO_(3))_(2)` solution?

0.1 M H_(2)S has K_(1)=10^(-5) & K_(2)=1.5xx10^(-12) . What will be the concentration of S^(-2) in the solution.

0.1 M H_(2)S has K_(1)=10^(-5) & K_(2)=1.5xx10^(-12) . What will be the concentration of S^(-2) in the solution.

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

What is the approximate OH^(-) ion concentration of a 0.150M NH_(3) solution? (K_(b)=1.75xx10^(-5))

The concentration of Fe^(2+) (10ml) required to oxidize 15ml of 0.1M K_2Cr_2O_7 solution is:

The K_(sp) of M(OH)_(2)" is "5 times 10^(-10)M^(3) . The molar solubility of M(OH)_(2) in a 0.1 M NaOH solution is

The solubility product of Fe(OH)_3 is 1xx10^(-36) What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 ?

The solubility product of Fe(OH)_3 is 1xx10^(-36) What is the minimum concentration of OH^- ions required to precipitate Fe(OH)_3 from a 0.001 M solution of FeCl_3 ?

For the reaction: 2Fe^(3+)(aq)+(Hg_(2))^(2+)(aq) hArr 2Fe^(2+)(aq) K_(c)=9.14xx10^(-6) at 25^(@)C . If the initial concentration of the ions are Fe^(3+)=0.5 M, (Hg_(2))^(2+)=0.5 M, Fe^(2+)=0.03 M and Hg^(2+)=0.03 M, what will be the concentration of ions at equilibrium.