SCERT Maharashtra solutions for Chemistry [English] 12 Standard HSC chapter 3 - Ionic Equilibria [Latest edition]

What is the percentage dissociation of 0.1 M solution of acetic acid? \[\ce{[Ka(CH3COOH) = 10^{-5}]}\]

For a reaction \[\ce{HCl_{(aq)} + H2O_{(l)} ⇌ H3O^+_{ (aq)} + Cl^-_{ (aq)}}\]

Which of the following is a conjugate acid-base pair?

In biochemical system, pH of blood in our body is maintained due to the following buffer:

If ‘IP’ is the ionic product and ‘K_sp’ is the solubility product, precipitation of the compound will occur under the condition when:

NH₄F is a salt of weak acid HF (K_a = 7.2 × 10^–4) and weak base NH₄OH (K_b = 1.8 × 10^–5), the solution of NH₄F will be ______.

The theory which explain amphoteric nature of water is ______.

The pK_b of weak base BOH [K_b(BOH) = 1 × 10^-5] will be ______.

Name the buffer which is used to maintained pH of 8 to 10 for precipitation of cations III A group in qualitative analysis.

Write the solubility product of sparingly soluble salt Bi₂S₃.

What is the pOH if the hydrogen ion concentration in solution is 1 × 10^–3 mol dm^–3?

Write the relationship between molar solubility (S) and solubility product (K_sp) for CaF₂.

Give any one example of salt derived from weak acid and weak base.

Write the formula to calculate pH of buffer solution.

Label the one conjugate acid-base pair in the following reaction.

\[\ce{CO^{2-}_{3(aq)} + H2O_{(l)} ⇌ OH^- + HCO^-_3}\]

Calculate the pOH of 10^-8 M of HCl.

Calculate the pH and pOH of 0.0001 M HCl solution.

The solubility product of BaCl₂ is 4.0 × 10^-8. What will be its molar solubility in mol dm^-3?

Classify the following species into Lewis acids and Lewis bases.

Define pH.

Define pOH.

Define molar solubility. Write it’s unit.

Write solubility product of following sparingly soluble salt.

BaSO₄

Write solubility product of following sparingly soluble salt.

CaF₂

Define buffer solution.

Explain the types of buffer solutions.

Write one application of the following buffer:

Citrate buffer

Write one application of the following buffer:

`"HCO"_3^-  + "H"_2"CO"_3`

Write one application of the following buffer:

NH₄OH + NH₄Cl

Derive the equation which implies that the degree of dissociation of weak acid is inversely proportional to the square root of its concentration.

A buffer solution contains 0.3 mol dm^–3 NH₄OH (K_b = 1.8 × 10^–5) and 0.4 mol dm^–3 NH₄Cl. Calculate pOH of the solution.

The solubility of AgBr in water is 1.20 × 10^–5 mol dm^–3. Calculate the solubility product of AgBr.

Derive the equation p^H + p^OH = 14.

Distinguish between strong electrolyte and weak electrolyte.

If ‘S’ is solubility in mol dm^–3 and Ksp is the solubility product, then write the relation between them for CaF₂ and BaSO₄. Calculate the concentration of H₃O⁺ ion in soft drink whose pH is 3.5.

Explain the amphoteric nature of water.

Define Solubility product.

Define Hydrolysis of salt.