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Ionic Equilibrium Set-1 MCQ Online Practice Test | Class 11 | Quiz Tweek

Ionic Equilibrium Set-1

Practice Important MCQs for Ionic Equilibrium — Chemistry, Class 11.

Ionic Equilibrium is one of the most vital chapters in the Class 11 Chemistry syllabus, serving as a foundation for both Board exams and competitive entrance tests like NEET and JEE. This chapter transitions from chemical kinetics to the behavior of ions in aqueous solutions, covering essential concepts such as acid-base theories, the pH scale, salt hydrolysis, buffer solutions, and the solubility product. Understanding these principles is crucial for mastering analytical chemistry and biological systems where pH balance is fundamental.

For the 2024-25 CBSE session, there is a strong emphasis on conceptual clarity and numerical problem-solving. This practice quiz is meticulously designed to align with the NCERT curriculum, moving from basic definitions to complex calculations involving the common ion effect and $K_{sp}$ values. By working through these 30 questions, students will reinforce their ability to apply Le Chatelier’s principle to ionic systems and calculate the acidity or alkalinity of various salt solutions.

40

Minutes

30

Questions

1 / -0

Marking

Question Bank Preview

Q1. Which of the following acts as both a Bronsted acid and a Bronsted base?

(A)

$CO_3^{2-}$

(B)

$HCO_3^-$

(C)

$NH_4^+$

(D)

$PO_4^{3-}$

Q2. What is the conjugate base of $H_2PO_4^-$ ?

(A)

$H_3PO_4$

(B)

$P_2O_5$

(C)

$HPO_4^{2-}$

(D)

$PO_4^{3-}$

Q3. The pH of a $1.0 \times 10^{-8}$ M solution of $HCl$ is:

(A)

8.0

(B)

6.0

(C)

Between 6 and 7

(D)

Between 7 and 8

Q4. According to the Lewis concept, an acid is a/an:

(A)

Proton donor

(B)

Electron pair donor

(C)

Electron pair acceptor

(D)

Hydroxyl ion donor

Q5. For a neutral solution at $373$ K, where $K_w = 5.13 \times 10^{-13}$ , the pH is:

(A)

7.00

(B)

6.14

(C)

12.28

(D)

6.50

Q6. Which of the following salts will undergo anionic hydrolysis?

(A)

$NaCl$

(B)

$NH_4Cl$

(C)

$CH_3COONa$

(D)

$CuSO_4$

Q7. If the degree of ionization ( $\alpha$ ) of a weak electrolyte is very small, Ostwald’s Dilution Law is expressed as:

(A)

$K_a = C\alpha$

(B)

$K_a = C\alpha^2$

(C)

$K_a = C/\alpha^2$

(D)

$K_a = \alpha^2/C$

Q8. A buffer solution is a mixture of:

(A)

Strong acid and its conjugate base

(B)

Weak acid and its conjugate base

(C)

Strong base and its conjugate acid

(D)

Two strong acids

Q9. The solubility of $AgCl$ will be minimum in:

(A)

Pure water

(B)

$0.1$ M $AgNO_3$

(C)

$0.1$ M $NaCl$

(D)

$0.1$ M $CaCl_2$

Q10. The pH of a $0.01$ M $NaOH$ solution is:

(A)

2

(B)

12

(C)

10

(D)

7

Q11. Which is the strongest conjugate base?

(A)

$Cl^-$

(B)

$NO_3^-$

(C)

$CH_3COO^-$

(D)

$HSO_4^-$

Q12. The relationship between $K_a$ and $K_b$ for a conjugate acid-base pair is:

(A)

$K_a + K_b = K_w$

(B)

$K_a / K_b = K_w$

(C)

$K_a \times K_b = K_w$

(D)

$K_a \times K_w = K_b$

Q13. The pH of a buffer solution containing equal concentrations of $CH_3COOH$ ( $K_a = 1.8 \times 10^{-5}$ ) and $CH_3COONa$ is:

(A)

4.74

(B)

7.00

(C)

9.26

(D)

5.00

Q14. For the salt $A_2B_3$ , the expression for the solubility product ( $K_{sp}$ ) in terms of solubility ( $S$ ) is:

(A)

$6S^5$

(B)

$36S^5$

(C)

$108S^5$

(D)

$25S^4$

Q15. When $HCl$ gas is passed through a saturated solution of $NaCl$ , the $NaCl$ precipitates because:

(A)

$HCl$ is a gas

(B)

Ionic product of $[Na^+][Cl^-]$ exceeds $K_{sp}$

(C)

$K_{sp}$ of $NaCl$ decreases

(D)

$HCl$ reacts with $K_{sp}$

...and 15 more challenging questions available in the interactive simulator.

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