.png "mht-cet-ionic-equilibria-mock-test-2026")
MHT CET Ionic Equilibria Mock Test
Instructions:
- Total Questions: 20 MCQs
- Time Limit: 20 Minutes
- No negative marking.
- Do not refresh the page.
Ionic Equilibria
20:00
Test Result
0/20
1. According to Arrhenius theory, an acid is a substance that:
Solution: Arrhenius acids dissociate in water to give H⁺ ions.
2. Which of the following is a Lewis acid?
Solution: BF₃ is electron-deficient (incomplete octet) and accepts an electron pair, acting as a Lewis acid.
3. The conjugate base of HSO₄⁻ is:
Solution: Conjugate base is formed by removing an H⁺. HSO₄⁻ - H⁺ = SO₄²⁻.
4. For pure water at 298 K, the value of Kw is:
Solution: Ionic product of water (Kw) at 25°C is 1 × 10⁻¹⁴.
5. The pH of 0.01 M HCl solution is:
Solution: [H⁺] = 0.01 = 10⁻² M. pH = -log(10⁻²) = 2.
6. Which relation is correct for an aqueous solution at 25°C?
Solution: The sum of pH and pOH is always 14 at 25°C.
7. A buffer solution is a mixture of:
Solution: An acidic buffer contains a weak acid and its salt with a strong base (e.g., CH₃COOH + CH₃COONa).
8. The pH of a solution is 5. Its pOH is:
Solution: pOH = 14 - pH = 14 - 5 = 9.
9. Solubility product (Ksp) of AgCl is expressed as:
Solution: Ksp is the product of ion concentrations: Ksp = [Ag⁺][Cl⁻].
10. Which salt undergoes hydrolysis to form a basic solution?
Solution: CH₃COONa is a salt of Weak Acid + Strong Base. Its hydrolysis produces OH⁻ ions, making it basic.
11. Henderson-Hasselbalch equation for acidic buffer is:
Solution: pH = pKa + log([Salt]/[Acid]).
12. Common ion effect is observed when:
Solution: Adding NH₄Cl (Strong Electrolyte) to NH₄OH (Weak Electrolyte) suppresses dissociation of NH₄OH due to common NH₄⁺ ion.
13. The relation between solubility (S) and solubility product (Ksp) for CaF₂ is:
Solution: CaF₂ → Ca²⁺ + 2F⁻. (S) (2S)². Ksp = S × 4S² = 4S³.
14. Which of the following is a strong electrolyte?
Solution: HCl dissociates completely in water, making it a strong electrolyte.
15. Degree of dissociation (α) for a weak acid is given by Ostwald's dilution law as:
Solution: For weak electrolytes, α = √(Ka/C).
16. The pH of human blood is approximately:
Solution: Human blood acts as a buffer solution with a pH around 7.35 - 7.45.
17. Which species can act as both Bronsted acid and Bronsted base?
Solution: Amphoteric nature: HCO₃⁻ can donate H⁺ (to form CO₃²⁻) or accept H⁺ (to form H₂CO₃).
18. Condition for precipitation is:
Solution: Precipitation occurs when Ionic Product (IP) exceeds the Solubility Product (Ksp).
19. If pH of a solution is 3, the hydrogen ion concentration is:
Solution: [H⁺] = 10^(-pH) = 10⁻³ M.
20. What is the pH of 10⁻⁸ M HCl solution?
Solution: H⁺ from HCl = 10⁻⁸, H⁺ from water = 10⁻⁷. Total H⁺ ≈ 1.1 × 10⁻⁷. pH ≈ 6.96 (slightly less than 7).
Post a Comment