Ionic Equilibrium Questions

[H⁺] = √(KwKa/C) is suitable for –

Formula for degree of hydrolysis ‘h’; h = [10⁻⁷ (KaKb)⁻½] is applicable to the salt –

The salt of which of the following four weak acids will be most hydrolysed –

The solution of blue vitriol in water is acidic because –

Which of the following compound forms an aqueous solution which is acidic when compared with water –

A basic buffer solution can be prepared by mixing the solution of –

For a salt of weak acid and weak base [pKa − pKb] would be equal to –

The pH of buffer of NH₄OH + NH₄Cl - type is given by -

pOH = 7–0.5 pKa + 0.5 pKb is true for which pair of cation and anion.

If pKb > pKa then the solution of the salt of weak acid and weak base will be -

What is the pH of an aqueous solution of ammonium acetate (Ka = Kb = 1.8 × 10⁻⁵) –

Expression pKh = pKw − pKa − pKb is not applicable to –

Select the correct combination –

Which of the following is an acidic salt –

An aqueous solution of aluminium sulphate would show –

The pH of two solutions are 5 and 3 respectively. What will be the pH of the solution made by mixing equal volumes of the above solutions –

4.0 g of NaOH and 4.9 g of H₂SO₄ are dissolved in water and volume is made upto 250 ml. The pH of this solution is –

The pH of two equimolar weak acids are 3.0 and 5.0 respectively. Their relative strength is –

For an acid solution the [OH⁻] is –

The formula to calculate pKa for acetic acid is –

The aqueous solution whose pH = 0 is-

Pure water ionises as 2H₂O (ℓ) ⇌ H₃O⁺ (aq.) + OH⁻ (aq) At 25°C the pH of pure water is approximately 7.0 At 37°C its pH is –

Kw for water at 25°C is equal to 10⁻¹⁴. What is its value at 90°C –

The value of pKw at 25°C is -

The pKw of water at 50°C is 13.40. An aqueous solution at 50°C has pH = 7. This solution is–

Select the correct statement –

The concentration of a monoprotic acid is C moles L⁻¹ and ionisation constant Ka. The pH of the solution is –

In the aqueous solution of MgCl₂ –

Ostwald’s dilution law for a weak acid HA may be given as –

For two weak acids A and B, the ratio of their percent ionization is 4 : 9. The ratio of their Ka would be–

A monoprotic acid in a 0.1 M solution ionizes to 0.001%. Its ionization constant is –

Ostwald’s dilution law gives satisfactory results for -

K₁ and K₂ are the first and second dissociation constants of oxalic acid. Choose the correct statement –

Ka₁, Ka₂ and Ka₃ are the three dissociation constants of H₃PO₄. Which of the following is a correct order –

The dissociation constant of two weak acids are Ka₁ & Ka₂ respectively. Their relative strength is -

The ionisation constant of a tribasic acid is Ka₁ & Ka₂ . If its first, second and third ionisation constants are Ka₁, Ka₂ and Ka₃ respectively then -

For a binary weak electrolyte, the degree of dissociation is proportional to the-

A solution of 0.1 M weak base (BOH) is to be titrated with 0.1 M strong acid (HA) at the half equivalence point the pH is 10.7 what is the pKₐ of base

What will be the pH of the solution, if 0.01 mole of HCl is dissolved in a buffer solution containing 0.03 mole of propanoic acid (Ka = 1.0 × 10–5) and 0.02 moles of salt, at 25ºC

The solubility product of chalk is 9.3 × 10–8. Calculate its solubility in gram per litre

The dissociation constant of weak acid HA is 4.9×10–8. After making the necessary approximations . Calculate pH in 0.1 M acid

The pKb of dimethylamine and pKa of acetic acid are 3.27 and 4.77 respectively at T(K). The correct option for the pH of dimethylammonium acetate solution is:

Assertion :- Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate AgBr rather than AgCl. Reason :- Ksp of AgCl < Ksp of AgBr.

A solution contains 1 molar each of M²⁺ and X³⁺ ions. NaOH is added gradually to this solution. Which of the following statements is correct about precipitation of M(OH)₂ and X(OH)₃? [Given: Ksp [M(OH)₂] = 4 × 10-10 ; Ksp [X(OH)₃] = 2.7 × 10-14]

Consider the following two statements for the given equilibrium Fe³⁺(aq) + SCN⁻(aq) ⇌ [Fe(SCN)]²⁺(aq) Statement I: Addition of oxalic acid will shift equilibrium to the left side. Statement II: Addition of aqueous HgCl₂ decreases the intensity of red

Nessler's reagent is ?

Which of the following salts will given highest pH in water ?

Arrange in increasing order of solubility of AgBr in the given solutions. (i) 0.1 M NH3 (ii) 0.1 M AgNO3 (iii) 0.2 M NaBr (iv) pure water