Ionic Equilibri...

The pH of a solution obtained by dissolving 5 × 10⁻⁴ moles of Ca(OH)₂ (strong electrolyte) to 100 ml solution at 298 K will be

One litre of a saturated solution of CaCO₃ is evaporated to dryness due to which 7.0 mg of residue is left. The solubility product for CaCO₃ is

The hydrolysis constant for ZnCl₂ will be

Where, K_b is effective dissociation constant of base Zn⁺⁺

M(OH)_x has K_SP 4 × 10^–12 and solubility 10^–4M. Then the value of x is

For a weak electrolyte α1 and α2 are in ratio of 1: 2, for a given concentration ka1 = 2 ×10−4 . What will be value of ka2 ?

Consider the reaction A⁻ + H₃O⁺ ⇌ HA + H₂O. The K_a value for acid HA is 1.0 × 10⁻⁶ . What is the value of K for this reaction.

The ionization constant of HCO₂H is 1.8 × 10⁻⁴ . What is the percent ionization of a 0.001 M solution?

At −50°C, the self−ionization constant (ion product) is How many amide ions are present per mm³ of pure liquid ammonia?

The degree of dissociation of anilinium acetate is

10 ml of 0.2 M acid is added to 250 ml of a buffer solution with pH = 6.34 and the pH of the solution becomes 6.32. The buffer capacity of the solution is