Ionic Equilibri...

A weak base B(OH)₂ has dissociation constant 10^-8 . The equilibrium constant for its reaction with excess of strong acid will be

A weak monobasic acid (0.1 M) has a pH of 3 at a particular temperature (25°C). When this acid is neutralized by strong base (NaOH), what is the value of equilibrium constant at equivalent point at 25°C?

The concentration of [OH^– ] left in a solution after mixing 50 ml of 0.2 M ACl₂ with 50 ml 0.4 m NaOH. [K_sp of A[OH]₂ = 1.2 × 10^–11]

A weak acid HA after treatment with 12 ml of 0.1 M strong base BOH has a pH of 5. At the end point, the volume of same base required is 20 ml, then K_a of acid is

The H⁺ ion concentration in 0.001 M CH₃COOH (K_a = 1.8 ×10^-5 ) is 1.34 ×10^-4 g ion/L. The H⁺ ion concentration if 0.164 g of CH₃COONa is added to a litre of 0.001 M CH₃COOH will be

The pH at which an acid indicator with K_a = 1 × 10⁻⁵ changes colours when indicator concentration is 1 × 10⁻⁵ M is

If K_b for fluoride ion at 25°C is 1.48 × 10⁻¹¹, the ionization constant of hydrofluoric acid in water at this temperature is

If 50 ml of 0.2 M KOH is added to 40 ml of 0.5 M HCOOH, the pH of the resulting solution is (K_a = 1.8 × 10⁻⁴ )

If the degree of ionization of water be 1.8 × 10^-9 at 298 K. Its ionization constant will be

When a solution of benzoic acid was titrated with NaOH, the pH of the solution, when half of the acid was neutralized, will be 4.2. Dissociation constant of the acid is