Ionic Equilibrium Questions

Which of the following is the ionisation constant of 0.01 M aniline (0.02% ionised)-

At 298K, the solubility of PbCl₂ is 6.3×10⁻³ moles L⁻¹. Its solubility product at this temperature is –

When HCl gas is passed through a impure saturated solution of common salt, pure NaCl is precipitated because –

In the hydrolysis of sodium acetate –

At 25°C, the solubility product of Ca(OH)₂ is 32 × 10⁻¹². What will be the pOH of its saturated solution at this temperature –

When equal volumes of the following solutions are mixed, precipitation of CaF₂ (Ksp = 1.7 × 10⁻¹⁰) will occur only with –

At 25°C what will be the solubility of silver carbonate in 0.1 M Na₂CO₃ solution. At this temperature Ksp of silver carbonate is 4 × 10⁻¹³ –

At 298 K, how many milligrams of silver bromide can be dissolved in 20 litres of water - [Ksp(AgBr) = 5.0 × 10⁻¹³] (Atomic wt. Ag = 108, Br = 80)

Ksp of AgCl is 1 × 10⁻¹⁰. Its solubility in 0.1 M KNO₃ will be –

Let the solubility of AgCl in water, in 0.01 M CaCl₂, in 0.01 M NaCl and in 0.05 M AgNO₃ be s₁, s₂, s₃ and s₄ respectively. Which of the following relations between these quantities is correct –

The pOH of a basic buffer (e.g. NH₄OH/NH₄Cl) is 5. If the concentration of the salt is tripled whereas that of base remains same. What is the new value of pOH (Given log 3 ≈ 0.48) –

500 ml of 0.2 M acetic acid are added to 500 ml of 0.30 M sodium acetate solution. If the dissociation constant of acetic acid is 1.5 × 10⁻⁵ then pH of the resulting solution is –

In a buffer solution of a weak acid and its salt, if the ratio of concentration of salt to acid is raised 10 times then pH of the solution will-

A certain buffer solution contains equal concentration of X⁻ and HX. The Kb for X⁻ is 1 × 10⁻¹⁰. The pH of the buffer is-

The pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate is (Ka for acetic acid = 1.75 × 10⁻⁵)–

The pH of 0.001M sodium acetate solution is [Ka(CH₃COOH) = 1.8 × 10⁻⁵] –

On hydrolysis of sodium carbonate, the reaction takes place between –

Given the two concentration of HCN are 0.1 M & 0.001 M respectively. What will be the ratio of degree of dissociation -

% hydrolysis of 0.1M CH₃COONH₄, when Ka = Kb = 1.8 × 10⁻⁵ is -

10⁻² mole of KOH is dissolved in 10 litres of water. The pH of the solution is –

0.01 M Acetic acid is 12.5 % dissociated. Its pH will be –

How many moles of HCl must be removed from 1 litre of aqueous HCl solution to change its pH from 2 to 3 -

For a 100 ml solution of 10⁻² M NaOH the ratio pH : pOH would be –

A 0.01 M acetic acid solution is 1.0% ionised. An another acetic acid is 10% ionised. What will be the concentration of another acetic acid -

A sufficient quantity of acid is added to change its pH from 5 to 2. Its hydrogen ion concentration is increased by –

At 298 K, the ratio of number of pure water molecules to number of hydroxyl ions is –

The pH of a solution is 6.0. In this solution –

The [H⁺] of a solution is 0.03 M. The pOH of this solution is –

The dissociation constant of a weak acid is 1.0 × 10⁻⁴. The equilibrium constant of its reaction with strong base is –

What will be the hydrogen ion concentration (moles L⁻¹) of 0.01 M HCN solution if it is 20% ionised

Find the percentage ionisation of 0.2 M acetic acid solution, whose dissociation constant is 1.8 × 10⁻⁵

Phenolphthalein shows colour change in a definite pH range, which is-

According to Modern quinoid theory the indicator used in acid-alkali titrations are-

Phenolphthalein is-

Methyl Orange is-

The colour of phenolphthalein in acid is-

pH range of colour change for methyl orange indicator is-

The correct relation between Ksp and solubility for the salt KAl(SO₄)₂ is

Which of the following expressions shows the saturated solution of PbSO₄ –

At 30°C, the solubility of Ag₂CO₃ (Ksp = 8 × 10⁻²) will be maximum in –

The necessary condition for saturated solution is

Which of the following salts has maximum solubility –

The aqueous solution of which of the following sulphides would contain maximum concentration of S²⁻ ions—

Which of the following would increase the solubility of Pb(OH)₂–

If s is the molar solubility of Ag₂SO₄, then –

H₂CO₃ + NaHCO₃ found in blood helps in maintaining pH of the blood close to 7.4. An excess of acid entering the blood stream is removed by-

H⁺ ion concentration of water does not change by adding –

Addition of sodium acetate solution to acetic acid causes the following change–

In the neutralization process of H₃PO₄ and NaOH, the number of buffers formed will be -

Which one of the following mixture does not act as a buffer solution-