Ionic Equlibriu...

The compound whose 0.1 M solution is basic is?

Which of the following solution will have pH close to 1.0 ?

The ≈ pH of the neutralisation point of 0.1 N ammonium hydroxide with 0.1 N HCl is

If equilibrium constant of

CH₃COOH + H₂O  CH₃COO^- + H₃O⁺

Is 1.8 × 10^-5, equilibrium constant for

CH₃COOH + OH^-  CH₃COO^- + H₂O is

If 40 ml of 0.2 M KOH is added to 160 ml of 0.1 M HCOOH [K_a = 2 × 10^-4]. The pOH of the resulting solution is

A solution with pH 2.0 is more acidic than the one with pH 6.0 by a factor of :

The first and second dissociation constants of an acid H₂A are 1.0 × 10^-5 and 5.0 × 10^-10 respectively.

The overall dissociation constant of the acid will be:

An aqueous solution contains 0.01 M RNH₂ (K_b= 2 × 10^-6) & 10^-4 M NaOH.

The concentration of OH^- is nearly:

What volume of 0.2 M NH₄Cl solution should be added to 100 ml of 0.1 M NH₄OH solution to produce a buffer solution of pH = 8.7 ?            

Given : pK_b of NH₄OH = 4.7 ; log 2 = 0.3

The pK_a of a weak acid, HA, is 4.80. The pK_b of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be: