Ionic Equilibrium

At 25oC, the dissociation constant of a base, BOH, is 1.0 \(\times\) 10\(-\)12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because

The solubility product of a sparingly soluble salt AX2 is 3.2 \(\times\) 10\(-\)11. Its solubility (in moles/L) is

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection. pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In\(-\)) forms of the ind...

The solubility product of AgI at 25oC is 1.0 \(\times\) 10\(-\)16 mol2 L\(-\)2. The solubility of AgI in 10\(-\)4 N solution of KI at 25oC is approximately (in mol L\(-\)1

Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. Then find out pKb of NH4OH

Which has highest pH?

Solubility of MX2 type electrolytes is 0.5 \(\times\) 10\(-\)4 mole/lit., then find out Ksp of electrolytes.

Correct relation between dissociation constants of a dibasic acid is

Solubility of M2S salt is 3.5 \(\times\) 10\(-\)6 then find out solubility product.

In HS\(-\), I\(-\), R \(-\) NH2, NH3 order of proton accepting tendency will be

Ionisation constant of CH3COOH is 1.7 \(\times\) 10\(-\)5 and concentration of H+ ions is 3.4 \(\times\) 10\(-\)4. Then find out initial concentration of CH3COOH molecules.

Which statement is wrong about pH and H+?

Conjugate acid of NH2\(-\) is