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mcqs of
,
1 : Ionic product of water (Kw) increases when temperature increases from 0°C to 100°C:
1
:
25 times
2
:
75 times
3
:
55 times
4
:
65 times
2 : Which of the following can be used to treat acidity in stomach?
1
:
NaHCO3
2
:
Mg(OH)2
3
:
Al(OH)3
4
:
all of these
3 : Milk of magnesium is?
1
:
Mixture of Mg(OH)2 and Al(OH)3
2
:
Mg
3
:
MgCO3
4
:
Mg(OH)2
4 : In case when [OH-] > [H+] the solution is:
1
:
Acidic
2
:
Neutral
3
:
Basic
4
:
None of these
5 : Which of the following is an amphoteric species?
1
:
NH3
2
:
HCl
3
:
H2O
4
:
NaOH
6 : Which of the following is a Lewis acid?
1
:
H2O
2
:
BF3
3
:
KCl
4
:
NH3
7 : The value of pK_w at 25°C for water is:
1
:
10⁻⁷
2
:
7
3
:
10⁻¹⁴
4
:
14
8 : The units for Kw of H2O are:
1
:
moles dm⁻³
2
:
moles·dm⁻⁶
3
:
moles² dm⁻⁶
4
:
moles²·dm⁻³
9 : Acid having Ka > 1 will be:
1
:
weak
2
:
very weak
3
:
moderate
4
:
strong
10 : High value of Ka means that acid is:
1
:
Very weak
2
:
weak
3
:
strong
4
:
very strong
11 : The pH of 10⁻³ mol dm⁻³ of an aqueous solution of HCl is:
1
:
1.5
2
:
2.0
3
:
3.0
4
:
2.7
12 : The term pH was introduced by:
1
:
Henderson
2
:
Sorenson
3
:
Goldsmith
4
:
Thomson
13 : For acidic solution, pH will be:
1
:
7
2
:
less than 7
3
:
greater than 7
4
:
zero
14 : The pH of a solution is 9, the solution is:
1
:
weak acid
2
:
weak base
3
:
strong acid
4
:
strong base
15 : In case when [OH-] < [H+] the solution is:
1
:
Acidic
2
:
Neutral
3
:
Basic
4
:
None
16 : pH of pure water is:
1
:
4.4
2
:
5.4
3
:
7.0
4
:
8.0
17 : The ionic product of water will increase if:
1
:
H+ ions are added
2
:
OH- ions are added
3
:
Temperature is increased
4
:
pressure is increased
18 : Which of the following has highest pH?
1
:
0.1M NaOH
2
:
0.1M H2SO4
3
:
0.1M HCl
4
:
0.2M HNO3
19 : The pOH of solution is 4. The H+ ion concentration of solution is:
1
:
4.0 moles/dm³
2
:
10⁻¹⁰ moles/dm³
3
:
0.4 moles/dm³
4
:
4×10⁻⁴ moles/dm³
20 : The ionic product of water will increase if:
1
:
H+ ions are added
2
:
OH- ions are added
3
:
temperature is increased
4
:
pressure is increased
21 : Ionic product of water (Kw) increases when temperature increases from 0°C to 100°C:
1
:
25 times
2
:
75 times
3
:
55 times
4
:
65 times
22 : The pH of a solution of HCl is 3, the strength of the acid is:
1
:
0.1M
2
:
0.01M
3
:
0.001M
4
:
0.0001M
23 : Which of the following solution has zero pH?
1
:
1M HCl
2
:
0.5M H2SO4
3
:
0.1M HNO3
4
:
2.0M CH3COOH
24 : A solution having H+ ion concentration 1×10⁻⁷. Its pH will indicate it as:
1
:
acid
2
:
Basic
3
:
Neutral
4
:
Amphoteric
25 : Common ion effect finds extensive application in:
1
:
Quantitative analysis
2
:
Qualitative analysis
3
:
spectroscopic analysis
4
:
Thermal analysis
26 : Which of the following can be used to purify NaCl by common ion effect?
1
:
LiCl
2
:
FeCl3
3
:
HCl
4
:
H2S
27 : What is the correct relation between pH and pKa?
1
:
pH = pKa + log (Acid)/(base)
2
:
pH = pKa + log (base)/(Acid)
3
:
pH = pKa - log(Acid)/(base)
4
:
pH = pKb + log(base)/(Acid)
28 : The ionization of NH4OH can be suppressed by adding:
1
:
NH4Cl
2
:
NaCl
3
:
NH3
4
:
H2S
29 : A basic buffer solution can be prepared by mixing:
1
:
Weak acid and its salt with strong base
2
:
Strong acid and its salt with weak base
3
:
Weak base and its salt with strong acid
4
:
weak acid and its salt with strong base
30 : The value of Kw at 25°C is:
1
:
0.11×10⁻¹⁴
2
:
0.03×10
3
:
1×10⁻¹⁴
4
:
3×10⁻¹⁴
31 : Lewis base is:
1
:
a proton donor
2
:
a proton acceptor
3
:
an electron pair donor
4
:
an electron pair acceptor
32 : The pH of mixture of CH3COONa and CH3COOH is:
1
:
7
2
:
>7
3
:
<7
4
:
1
33 : Which salt dissolved in water forms a solution with a pH greater than 7?
1
:
NaCl
2
:
CuSO4
3
:
Na2CO3
4
:
NH4Cl
34 : The pH of an aqueous solution of CH3COONa is:
1
:
less than 7
2
:
greater than 7
3
:
7
4
:
none of these
35 : When a cation reacts with water, then the solution becomes:
1
:
acidic
2
:
basic
3
:
neutral
4
:
highly basic
36 : Dissociation constant, Ka, of acetic acid in water at 25°C:
1
:
4.76
2
:
1.0×10⁻¹⁴
3
:
1.8×10⁻⁵
4
:
1.8×10⁻¹⁰
37 : The sum of pH and pOH at 25°C is always:
1
:
7
2
:
zero
3
:
14
4
:
10⁻¹⁴
38 : The hydrolysis of sodium Carbonate involves the reaction between:
1
:
Na+ and OH-
2
:
Na+ and water
3
:
CO3²⁻ and H+
4
:
CO3²⁻ and water
39 : Which of the relation between ionic product (Q) and solubility product (Ksp) indicates the occurrence of precipitation?
1
:
Q > Ksp
2
:
Q < Ksp
3
:
Q = Ksp
4
:
none
40 : The precipitation occurs if the ionic concentration is:
1
:
less than Ksp
2
:
More than Ksp
3
:
equal to Ksp
4
:
Constant
41 : If Ksp value is larger, the salt in water is:
1
:
less soluble
2
:
more soluble
3
:
Moderately soluble
4
:
Insoluble
42 : In the titration of a strong acid with a strong base, which of the following indicator is used?
1
:
methyl orange
2
:
phenolphthalein
3
:
starch
4
:
KMnO₄
43 : The solubility of CaF₂ is 2 × 10⁻⁴ moles dm⁻³. Its solubility product is:
1
:
2.56 × 10⁻⁴
2
:
3.2 × 10⁻¹¹
3
:
4 × 10⁻⁸
4
:
8 × 10⁻¹²
44 : The phenolphthalein indicators changes its colour in the pH range:
1
:
3.2-4.5
2
:
8.2-10.0
3
:
6.2-8.2
4
:
8.2-10
45 : The pH of 10⁻³ mol dm⁻³ of an aqueous solution of H₂SO₄ is:
1
:
3.0
2
:
2.7
3
:
2.0
4
:
1.5
46 : The solubility product of AgCl is 2.0 × 10⁻¹⁰ mol dm⁻⁶. The maximum concentration of Ag⁺ ions in the solution is:
1
:
2.0 × 10⁻¹⁰ mol dm⁻³
2
:
1.41 × 10⁻⁵ mol dm⁻³
3
:
1.0 × 10⁻¹⁰ mol dm⁻³
4
:
4.0 × 10⁻²⁰ mol dm⁻³
47 : Which indicator is typically used for titration involving strong acids and strong base?
1
:
Methyl orange
2
:
Phenolphthalein
3
:
bromothymol blue
4
:
Litmus solution
48 : Which of the following is the conjugate base of water?
1
:
OH⁻(aq)
2
:
OH⁺(aq)
3
:
H₂O
4
:
H₃O⁺(aq)
49 : Which of the following is a Lewis acid but not a Bronsted-Lowry acid?
1
:
HCl
2
:
NH₃
3
:
AlCl₃
4
:
H₂O
50 : In an acid-base titration, the equivalence point is reached when:
1
:
the pH of the solution is 7
2
:
the indicator changes colour
3
:
equal volumes of acid and base have been added
4
:
the reaction stops
51 : If the concentration of Cl⁻ ion in a solution is increased, the solubility of silver chloride (AgCl) will:
1
:
Decrease
2
:
Increase
3
:
Remain unchanged
4
:
Become zero
52 : Which of the following pairs of substances can act as a conjugate acid-base pair according to the Bronsted-Lowry theory?
1
:
HCl and NaOH
2
:
NH₃ and NH₄⁺
3
:
H₂O and H₂SO₄
4
:
H₂O and CH₄
53 : If the pH of a solution is 11, what is the [OH⁻] concentration in the solution?
1
:
1×10⁻³ M
2
:
1×10⁻¹¹ M
3
:
1×10⁻² M
4
:
1×10⁻¹⁴ M
54 : Which of the following pair forms a buffer solution?
1
:
HCl and NaCl
2
:
CH₃COONa and CH₃COOH
3
:
NaOH and HCl
4
:
NH₃ and Na₂SO₄
55 : In AgCl solution, some salt of NaCl is added. AgCl will be precipitated due to:
1
:
Solubility
2
:
Electrolyte
3
:
Unsaturation effect
4
:
Common ion effect
56 : Which one of the following is the correct presentation for Ksp? AgCl ⇌ Ag⁺ + Cl⁻
1
:
Ksp = [AgCl]/[Ag⁺][Cl⁻]
2
:
Ksp = [Ag⁺][Cl⁻]/[AgCl]
3
:
Ksp = [Ag⁺][Cl⁻]
4
:
Ksp = [AgCl]
57 : What will be the pH of solution of NaOH with a concentration of 10⁻³ M?
1
:
3
2
:
14
3
:
11
4
:
7
58 : Ca(OH)₂ is sparingly soluble having solubility product value 6.5 × 10⁻⁶. What will be its solubility?
1
:
2.75 × 10⁻²
2
:
1.17 × 10⁻²
3
:
2.75 × 10⁻²
4
:
3.63 × 10⁻³
59 : The nature of an aqueous solution of ammonia (NH₃) is:
1
:
Amphoteric
2
:
Neutral
3
:
Acidic
4
:
Basic
60 : Ka for an acid is higher, the stronger is the acid; relate the strength an acid with pKa:
1
:
Higher pKa, weaker the acid
2
:
Lower pKa, stronger the acid
3
:
pKa has no relation with acid strength
4
:
Both A and B
61 : The pH of 10⁻³ moles of HNO₃ is?
1
:
2.7
2
:
3
3
:
2.0
4
:
1.5
62 : A buffer solution is that which resists/minimizes the change in:
1
:
pOH
2
:
pH
3
:
pKa
4
:
pKb
63 : The Ka value of HCl, CH₃COOH, HF and H₂SO₄ are 10⁷, 1.8 × 10⁻⁵, 6.7 × 10⁻⁵ and 10². The order of strength is:
1
:
CH₃COOH > HF > H₂SO₄ > HCl
2
:
HCl > H₂SO₄ > HF > CH₃COOH
3
:
HCl > CH₃COOH > HF > H₂SO₄
4
:
HCl > HF < H₂SO₄ > CH₃COOH
64 : pH = pKa + log [salt] / [Acid] is known as:
1
:
Einstein equation
2
:
Planck equation
3
:
Gibb's equation
4
:
Handerson equation
65 : An acidic buffer solution can be prepared by mixing:
1
:
Strong acid and its salt with strong acid
2
:
Weak base and its salt with strong acid
3
:
Strong base and its salt with weak acid
4
:
Weak acid and its salt with strong base
Chemistry 11th MCQs || Ilam Ghar
Chemistry 11th
Chapter 9 : Acid-Base Chemistry
