Ionic Equilibrium Questions

The degree of hydrolysis of 0.1 RNH₃Cl solution is 1.0 %. If the concentration of RNH₃Cl is made 0.4 M, what is the new degree of hydrolysis (in percentage) ?

The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be -

How much water must be added to 300 mL of 0.2 M solution of CH₃COOH (Ka = 1.8 × 10⁻⁵) for the degree of ionization (α) of the acid to double ?

What concentration of HCOO⁻ is present in a solution of 0.01 M HCOOH (Ka = 1.8 × 10⁻⁴) and 0.01 M HCl ?

Determine the molar solubility of MgF₂ from it's solubility product Ksp = 4 × 10⁻⁹ :

At 25°C, will a precipitate of Mg(OH)₂ form when a 0.0001 M solution of Mg(NO₃)₂ is adjusted to a pH of 9.0 ? At what minimum value of pH will precipitation start ? [Given : Ksp (Mg(OH)₂) = 10⁻¹¹ M³]

Will a precipitate form if 50 cm³ of 0.01 M AgNO₃ and 50 cm³ of 2 × 10⁻⁵ M NaCl are mixed ? [Given : Ksp (AgCl) = 10⁻¹⁰ M²]

Which of the following is a buffer solution ?

H₃PO₄ is a weak triprotic acid; approximate pH of 0.1 M Na₂HPO₄(aq.) is calculated by -

Approximate pH of 0.01 M NaHA is calculated by : (Ka₁ = 10⁻⁶ and Ka₂ = 10⁻⁸ are ionization constants of H₂A)

What will be the pH and % α (degree of hydrolysis) respectively for the salt BA of 0.1 M concentration ? Given : Ka for HA = 10⁻⁶ and Kb for BOH = 10⁻⁶

Consider the following salts. Which one(s) when dissolved in water will produce an acidic solution ? 1. NH₄Cl 2. Al₂(SO₄)₃ 3. NaCN 4. KNO₃

Given the following Ka values, determine which species is the strongest base. HSO₄⁻ = 1.2 × 10⁻², H₂PO₄⁻ = 6.3 × 10⁻⁸, HCO₃⁻ = 4.7 × 10⁻¹¹

Which salt can furnish H⁺ in its aqueous solution ?

What is the minimum concentration of SO₄²⁻ required to precipitate BaSO₄ in a solution containing 1.0 × 10⁻⁴ mole of Ba²⁺ ? Ksp for BaSO₄ = 4 × 10⁻¹⁰ :

At 25°C, the dissociation constants of CH₃COOH and NH₄OH in aqueous solution are almost the same. The pH of a solution of 0.01 N CH₃COOH is 4.0 at 25°C. The pH of 0.01 N NH₄OH solution at the same temperature would be :

'a' moles of a monacidic base are dissolved in one litre of the solution. The pH of the solution will be -

A solution contains 10 ml of 0.1 N NaOH and 10 ml of 0.05 N Na₂SO₄. pH of this solution is-

If the solubility of lithium sodium hexafluoroaluminate, Li₃Na₃(AlF₆)₂ is 'a' mole/litre, the solubility product is equal to -

Solution A has pH = 3 and solution B has pH = 6. Which one of the following is correct -

The units of ionic product of water (Kw) are –

Which of the following acids is stronger than benzoic acid (Ka = 6.3 × 10⁻⁵) -

According to Bronsted-Lowry concept, the relative strengths of the bases CH₃COO⁻, OH⁻ and Cl⁻ are in the order -

Which one of the following is NOT a buffer solution ?

20 cm³ of xM solution of HCl is exactly neutralised by 40 cm³ of 0.05 M NaOH solution, the pH of HCl solution is :

The solubility product of BaCrO₄ is 2.4 × 10⁻¹⁰ M². The maximum concentration of Ba(NO₃)₂ possible without precipitation in a 6 × 10⁻⁴ M K₂CrO₄ solution is :

What is the OH⁻ concentration of an aqueous solution of a substance whose pH = 3.2 ?

Four solutions of NH₄Cl are taken with concentrations 1 M, 0.1 M, 0.01 M and 0.001 M. Their degree of hydrolysis are h₁, h₂, h₃ and h₄. What is the gradation of degree of hydrolysis ?

0.1 M acetic acid solution is titrated against 0.1 M NaOH solution. What would be the difference in pH between 1/4 and 3/4 stages of neutralisation of acid ?

Consider this equilibrium, for which ΔH < 0, HgO(s) + 4I⁻(aq.) + H₂O(ℓ) ⇌ HgI₄²⁻ + 2OH⁻ Which changes will increase the equilibrium concentration of HgI₄²⁻ ? I. Increasing the mass of HgO(s) present II. Increasing [I⁻] III. Adding 1 M HCl

The hydrolysis constant for ZnCl₂ will be -

The ratio of pH of 0.05 M and 0.005 M H₂SO₄ solutions will be –

In a buffer solution X⁻ and HX concentration are same. If Kb value for X⁻ is 10⁻⁸ then pH of the buffer solution is –

When 0.02 moles of NaOH are added to a litre of buffer solution, its pH changes from 5.75 to 5.80. What is its buffer capacity –

0.05 M ammonium hydroxide solution is mixed with 0.001 M ammonium chloride solution. What will be the OH⁻ ion concentration of this solution – Kb(NH₄OH) = 1.8 × 10⁻⁵

The pH of 1 litre solution containing 0.5M NH₄OH and 0.5 M NH₄Cl (pKb = 5) -

Acetic acid (Ka = 2 × 10⁻⁵) and propionic acid (Ka = 2 × 10⁻⁶) have same concentrations. What is the ratio of their degree of ionisation

What is the pH of the solution at half neutralization in the titration of 0.1N CH₃COOH and 0.1N KOH : (Ka = 1.8 × 10⁻⁵)–

The concentration of a HCl solution is 10⁻² N. If this solution is diluted ten times then its pH will-

A solution contains 0.2 M NH₄OH and 0.2 M NH₄Cl. If 1.0 ml of 0.001 M HCl is added to it. What will be the [OH⁻] of the resulting solution (Kb = 2 × 10⁻⁵)

100 ml of 1.0 N CH₃COOH are added to 100 ml of 1.0 N NaOH solution. What will be the pH of resulting solution –

Half of the formic acid solution is neutralised on addition of a KOH solution to it. If Ka(HCOOH) = 2×10⁻⁴ then pH of the solution is – (log 2 = 0.3010)

Phenoxide ion (C₆H₅O⁻) is a weak base, with Kb = 7.7 × 10⁻⁵. Calculate the pH of a 0.20 M solution of C₆H₅O⁻ –

Solubility of AgCl [Ksp = 1 × 10⁻¹⁰] in 0.2 M AgNO₃ and 0.2 M NaCl solution will be respectively –

Equal volumes of 0.005 M and 0.005 N H₂SO₄ solutions are mixed together. The pH of resulting solution is –

Ksp for Pb(IO₃)₂ is 3.2 × 10⁻¹⁴ at a certain temperature. Its solubility will be –

Ksp for A₂B salt is 4 × 10⁻⁹. Evaluate its solubility –

Calculate the solubility of silver phosphate (Ag₃PO₄) in 0.10M AgNO₃ ? Ksp = 1.1 × 10⁻¹⁶ –

What will be the pH of 10⁻³ M monobasic weak acid solution if its dissociation constant is 1.8 × 10⁻⁵ –

The dissociation constants of monobasic acids A,B,C and D are 6 × 10⁻⁴, 5 × 10⁻⁵, 3.6 × 10⁻⁶, and 7 × 10⁻¹⁰ respectively. The pH values of their 0.1 molar aqueous solutions are in the order –