Test: Ionic Equilibrium - NEET MCQ

1 c.c. of 0.1N HCl is added to 99 CC solution of NaCl. The pH of the resulting solution will be

10 ml of  is mixed with 40 ml of . The pH of the resulting solution is

If pK_b for fluoride ion at 25°C is 10.83, the ionisation constant of hydrofluoric acid in water at this temperature is :

The pH of an aqueous solution of 1.0 M solution of a weak monoprotic acid which is 1% ionised is:

If K₁ & K₂ be first and second ionisation constant of H₃PO₄ and K₁ >> K₂ which is incorrect.

The degree of hydrolysis of a salt of weak acid and weak base in it's 0.1 M solution is found to be 50%. If the molarity of the solution is 0.2 M, the percentage hydrolysis of the salt should be

What is the percentage hydrolysis of NaCN in N/80 solution when the dissociation constant for HCN is 1.3 × 10^-9 and K_w = 1.0 × 10^-14

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:

The range of most suitable indicator which should be used for titration of X ^- Na⁺ (0.1 M, 10 ml) with 0.1 M HCl should be ( Given : k_b(X^-) = 10^-6 )

How many gm of solid NaOH must be added to 100 ml of a buffer solution which is 0.1 M each w.r.t. Acid HA and salt Na⁺ A^- to make the pH of solution 5.5. Given pK_a(HA) = 5 (Use antilog (0.5)= 3.16)

The solubility of A₂X₃ is y mol dm^-3. Its solubility product is

If K_sp for HgSO₄ is 6.4 × 10^-5, then solubility of this substance in mole per m³ is

Which of the following in most soluble in water ?

1 M NaCl and 1 M HCl are present in an aqueous solution. The solution is

The pK_a of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is:

The precipitate of CaF₂ (K_sp = 1.7 × 10^-10) is obtained when equal volumes of the following are mixed

pH of saturated solution of silver salt of monobasic acid HA is found to be 9.

Find the K_sp of sparingly soluble salt Ag A(s).

Given : K_a(HA) = 10^-10

When equal volumes of the following solutions are mixed, precipitation of AgCl (K_sp = 1.8 × 10^-10) will occur only with: