CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs
These CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs are prepared by our Chemistry Expert. By practicing following MCQs, students will be able to quickly revise all the concepts of the CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs. Additionally, CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs will be helpful for JEE And NEET Aspirants.
Refer to our Chemistry 11 7 Ionic Equilibrium MCQs for scoring Excellent Marks in your Exams.
CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs (SET A)
1. pKb for NH4OH at certain temperature is 4.74. The pH of basic buffer containing equimolar concentration of NH4OH and NH4Cl will be:-
(A) 7.74
(B) 4.74
(C) 2.37
(D) 9.26
Answer: 9.26.
2. What is the suitable indicator for titration of NaOH and oxalic acid:-
(A) Methyl orange
(B) Methyl red
(C) Phenolphthalein
(D) Starch solution
Answer: Phenolphthalein.
3. Phenolphthalein does not act as an indicator for the titration between:-
(A) KOH and H2SO4
(B) NaOH and CH3COOH
(C) Oxalic acid and KMnO4
(D) Ba(OH)2 and HCl
Answer: Oxalic acid and KMnO4.
4. Which can act as buffer:-
(A) NH4OH + NaOH
(B) HCOOH + CH3COONa
(C) 40 mL 0.1 M NaCN + 20 mL of 0.1 MHCl
(D) None of them
Answer: 40 mL 0.1 M NaCN + 20 mL of 0.1 MHCl.
5. The Important role played by the buffer solution in:-
(A) Increasing the pH value
(B) Decreasing the pH value
(C) Keeping the pH constant
(D) Solution will be neutral
Answer: Keeping the pH constant.
CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs (SET B)
1. Concentration of Ag+ ions in saturated solution of Ag2CrO4 at 20°C is 1.5 × 10–4 mol L–1. At 20°C, the solubility product of Ag2CrO4 is
(A) 3.3750 × 10^–12
(B) 1.6875 × 10^–10
(C) 1.68 × 10^–12
(D) 1.6875 × 10^–11
Answer: 1.68 × 10^–12.
2. At 90°C, the pH of 0.1M NaCl aqueous solution is:
(A) < 7 (B) > 7
(C) 7
(D) 0.1
Answer: < 7.
3. What will be the pH of 1.0 M ammonium formate solution, if Ka = 1 × 10^–4 and Kb = 1 × 10^–5
(A) 6.5
(B) 7.5
(C) 8.0
(D) 9.0
Answer: 6.5.
4. Which salt will not undergo hydrolysis?
(A) KCl
(B) Na2SO4
(C) NaCl
(D) All
Answer: All.
5. Maximum efficiency of cationic hydrolysis will be shown by:
(A) Al3+
(B) Ga+3
(C) Tl+1
(D) Tl+3
Answer: Al3+.
CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs (SET C)
The pH of aqueous solution of sodium acetate is
(A) 7
(B) Very low
(C) > 7
(D) <7 Answer: > 7
2. If pKb for CN– at 25°C is 4.7. The pH of 0.5M aqueous NaCN solution is
(A) 12
(B) 10
(C) 11.5
(D) 11
Answer: 11.5.
3. The highest pH value is of
(A) 0.1 M NaCl
(B) 0.1 M NH4Cl
(C) 0.1 M CH3COONa
(D) 0.1 M CH3COONH4
Answer: 0.1 M CH3COONa.
4. pH of K2S solution is:(A) 7
(B) Less than 7
(C) More than 7
(D) Zero
Answer: More than 7.
5. In the volumetric estimation of HCl, if we make use of phenolphthalein as an indicator, which base is unsuitable for the titration :-
(A) NaOH
(B) RbOH
(C) KOH
(D) NH4OH
Answer: NH4OH.
CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs (SET D)
1. In a mixture of weak acid and its salt, the ratio of the concentration of acid to salt is increased to ten-fold. The pH of the solution:-
(A) Decreases by one
(B) Increases by one-tenth
(C) Increases by one
(D) Increases ten-fold
Answer: Decreases by one.
2. In a solution of pH = 5, more acid is added in order to reduce the pH = 2. Find increase in concentration of hydrogen ion :-
(A) 100 times
(B) 1000 times
(C) 3 times
(D) 5 times
Answer: 1000 times.
3. The hydrogen ion concentration in a given solution is 6 × 10–4 M. Its pH will be:-
(A) 6
(B) 3.22
(C) 4
(D) 2
Answer: 3.22.
4. For N10H2SO4, pH value is:-
(A) 1
(B) 0.586
(C) 0.856
(D) None
Answer: 1.
5. Calculate pH of a solution whose 100 mL contains 0.2 g NaOH dissolved in it:-
(A) 10.699
(B) 11.699
(C) 12.699
(D) 13.699
Answer:.12.699.
CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs (SET E)
1. What would be [H+] of 0.006 M benzoic acid (Ka = 6 × 10–5)?
(A) 0.6 ×10^–4
(B) 6 × 10^–4
(C) 6 × 10^–3
(D) 3.6 × 10^–4
Answer: 6 × 10^–4.
2. pH of tomato juice is 4.4. Then concentration of H3O+ will be:
(A) 39 × 10^–4
(B) 3.9 × 10^–5
(C) 3.9 × 10^–4
(D) 3.9 × 10
Answer: 3.9 × 10^–5.
3. Find out Ka for 10–2 M HCN acid, having pOH equal to 10.
(A) Ka = 10^–4
(B) Ka = 10^–2
(C) Ka = 10^–5
(D) None of them
Answer: None of these.
4. The pH of 0.15 M solution of HOCl (Ka = 9.6 × 10–6) is
(A) 4.42
(B) 2.92
(C) 3.42
(D) None
Answer: 2.92.
We hope you liked our CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs. If you have any queries regarding CBSE Class 11 Chemistry Chapter 7 Ionic Equilibrium MCQs, drop a comment below and we will reply to you at the earliest.
Related Links:
CBSE Class 11 Chemistry Chapter 11 p-Block MCQs
CBSE Class 11 Chemistry Chapter 7 Chemical Equilibrium MCQs
