Class 12 Chemistry Ionic Equilibrium Notes and Important Questions
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Notes for Class 12 Ionic Equilibrium (Chemistry) are shown above.
Practice
Important Questions
What amount of Zn(OH)₂ will be precipitated out at 25°C if 100 mL of 0.22 g NaOH is added to 1 litre of a saturated solution of Zn(OH)₂? Precipitate is obtained in this reaction, why? [Solubility product of Zn(OH)₂ at 25°C is 1.8 × 10⁻¹⁴]
Potassium hydroxide having pH 8 is diluted 1000 times. Calculate the pH of the diluted base
The expressions of Ostwald’s dilution law is,
Derive it.
What information can you obtain from this expression?
Will strong electrolytes obey this expression, why?
$0.1\ \text{M}$ ethanoic acid is $1.34%$ ionized. Find its dissociation constant.
Hess's law is applied to calculate different types of enthalpy of reaction.
Illustrate the Hess law of constant heat summation.
Standard enthalpy of combustion of $\text{C (g)}$, $\text{H}_2\text{(g)}$ and $\text{C}_2\text{H}_2\text{(g)}$ are $-394\ \text{kJ mol}^{-1}$, $-286\ \text{kJ mol}^{-1}$ and $-1300\ \text{kJ mol}^{-1}$ respectively. Calculate enthalpy of formation of acetylene.
Draw the energy profile diagram of exothermic and endothermic reaction.
In a solution that is at equilibrium, what happens to the concentration of ions if the concentration of ions is increased?
The concentration of $\text{H}^+$ ions increases
The concentration of $\text{H}^+$ ions decreases
The concentration of $\text{H}^+$ ions stay the same
It depends on the initial concentration of ions
Differentiate between ionic product and solubility product.
Point out the limitation of Ostwald’s dilution law.
Why is aqueous solution of sodium chloride neutral?
Given that Ksp for BaSO₄ is 1 × 10⁻¹⁰, will the precipitate form when:
i) Equal volumes of 2 × 10⁻³ M BaCl₂ solution and 2 × 10⁻⁴ M Na₂SO₄ solution are mixed.
ii) Equal volumes of 2 × 10⁻⁸ M BaCl₂ solution and 2 × 10⁻³ M Na₂SO₄ solution are mixed.
The solubility product of chalk is 9.3 × 10⁻⁸. What is its solubility in gram per liter?
3.04 × 10⁻¹
3.04 × 10⁻²
3.04 × 10⁻³
3.04 × 10⁻⁴
Which of the following is the relation between solubility and product of sparingly soluble salt A₂B?
s = (Ksp)¹ᐟ²
s = [(Ksp)/2]¹ᐟ³
s = [(Ksp)/4]¹ᐟ³
s = [(Ksp)/(12B)]¹ᐟ⁵
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Exam
Ionic Equilibrium focuses on the behavior and equilibrium of ions in aqueous solutions. It covers acid-base theories, ionization of weak electrolytes, Ka, Kb, pH, buffer solutions, solubility product, common ion effect, indicators and hydrolysis of salts.
This page covers Ionic Equilibrium, chapter 2 of 22 in the Class 12 Chemistry syllabus set by the National Examination Board (NEB). 9 important questions for this chapter are available, each with a full solution.
For numerical and derivation-based chapters like this one, working through past NEB questions is usually more useful than re-reading notes alone — try solving each important question above before checking the solution, then compare your working step by step.