Multiple Choice Questions (MCQs) on
Chemical Equilibrium from Textbook
1. Which one of the following statements is false about dynamic equilibrium?
(a) Concentration of reactant and products are not changed(b) It takes place in a close container
(c) Rate of forward reaction is equal to rate of reverse reaction
(d) Equilibrium cannot be disturbed by any external stress.
2. When the magnitude of Kc is small, indicates
(a) Reaction mixture contains most of the reactant
(b) Reaction mixture contains most of the product
(c) Reaction mixture contains almost equal amount of reactant and product
(d) Reaction goes to completion
3. Qc can be defined as
(a) ratio of product and reactant
(b) ratio of molar concentration of product and reactant at specific time
(c) ratio of molar concentration of product and molar volume of reactant
(d) ratio of molar concentration of product and reactant raised to the power of coefficient
4.Consider the following
reaction and indicates which of the following best describe equilibrium
constant expression Kc
4NH3(g) + 5O2(g) ⇌
4NO(g) + 6H2O(g)
5. For which system does the equilibrium constant, Kc has units of concertation?
(a) N2(g) + 3H2(g) ⇌ 2NH3(g)
(b) N2(g) + O2(g) ⇌ 2NO(g)
(c) H2(g) + I2(g) ⇌ 2HI(g)
(d) CO2(g) + H2(g) ⇌ CO(g) + H2O(g)
6. A reaction which is never goes to completion is known as reversible reaction. Reversible reaction is represented by
(a) Double straight line
(b) Single arrow
(c) Double arrow
(d) Doted lines
7. The unit of Kc for reaction; N2(g) + O2(g) ⇌ 2NO(g)
(a) mol dm−3
(b) mol−2 dm6
(c) mol−1 dm3
(d) no unit
8. The system is stable in equilibrium when:
(a) Qc = Kc
(b) Qc > Kc
(c) Qc < Kc
(d) None of these
9. The value of Kc increases when
(a) [Reactant] = [product]
(b) [Product] is more
(c) [Reactant] is more
(d) [Product] is less
10.Which of the following represent backward reaction?
(a) (i) and (ii)
(b) (ii) only
(c) (i) only
(d) (iii) only
Answers of MCQs on Chemical Equilibrium from Text Book
1. D
2. A
3. B
4. A
5. A
6. D
7. B
8. B
9. A
10. B
Multiple Choice Questions (MCQs) on
Chemical Equilibrium from External Source
For Answers and explanation contact me on my WhatsApp no
03009215999
1. A
chemical reaction is at equilibrium when:
(a) Rate of forward reaction >
Rate of reverse reaction
(b) Rate of forward reaction <
Rate of reverse reaction
(c) Rate of forward reaction = Rate
of reverse reaction
(d) All of the above
2. In a
chemical reaction equilibrium is said to have been established when:
(a) Concentration of
reactants and products are equal
(b) Velocities of opposing
reactions become equal
(c) Temperature of opposing
reactions are equal
(d) Opposing reactions
cease.
3. A chemical reaction A ⇌ B is said to be in equilibrium when:
(a) Complete conversion of A to B has taken place
(b) Complete conversion of A to B is only 50% complete
(c) Only 10% conversion of A to B has taken place
(d) The rate of transformation of A to B is just equal to the rate of transformation of B to A in the system.
4. Which
of the following statement is wrong
regarding chemical equilibrium?
(a) At
equilibrium two opposing chemical reactions are proceeding in opposite
direction at the different rate
(b) At
equilibrium there is no change in the concentration of reactant and product
(c) Chemical
equilibrium is always dynamic
(d) Chemical
equilibrium can be distributed by changing conditions like concentration,
pressure, temperature
5. Which
one of the following is not a
reversible reaction?
(a) Oxidation
of SO2 into SO3
(b) Decomposition
of potassium chlorate
(c) Decomposition
of Hydrogen Iodide
(d) Formation
of Ammonia from its constituent elements or Esterification
6. Which
one is incorrect regarding Kc?
(a) It
is a ratio b/w two rate constants and it has no unit when Δn = 0
(b) It
remains constant at all temperature
(c) It
is independent of the pressure or catalyst
(d) It
is independent of the original concentration of reactants
7. The
value of Kc that lies midway between 10−2 to 102
indicates that
(a) Forward
reaction goes to completion
(b) Reverse
reaction goes to completion
(c) Neither
forward nor reverse reaction goes to completion
(d) All
of the above.
8. The
value of Kc more than 102 indicates that
(a) Forward
reaction goes to completion
(b) Reverse
reaction goes to completion
(c) Neither
forward nor reverse reaction goes to completion
(d) All
of the above.
9.The
value of Kc less than 10−2 indicates that
(a) Forward
reaction goes to completion
(b) Reverse
reaction goes to completion
(c) Neither
forward nor reverse reaction goes to completion
(d) All
of the above.
10. Which
one of the following factor will favor the reverse change?
(a) Increase
in concentration of one of the reactant
(b) Removal
of the products regularly
(c) Increase
in concentration of any one of the product
(d) None
of the above.
11. When H2
and I2 are mixed & equilibrium is attained, then
(a) The reaction stops
completely
(b)
HI dissociates completely
(c)
Amount of HI formed is equal to the amount of HI dissociated
(d)
None of these
12. Which
of the following is a characteristic of a reversible reaction?
(a) It
never proceeds to completion
(b) It
can be influenced by a catalyst
(c) It
proceeds only in the forward direction
(d) Number
of moles of reactants and products are equal
13. At
equilibrium, __________.
(a) the rates of the forward and
reverse reactions are equal
(b) the rate constants of the
forward and reverse reactions are equal
(c) all chemical reactions have
ceased
(d) All of them
14. How is the reaction quotient used to
determine whether a system is at equilibrium?
(a) The
reaction is at equilibrium when Q < Keq
(b)
The reaction is at equilibrium when Q > Keq
(c)
At equilibrium, the reaction quotient is undefined
(d)
The reaction is at equilibrium when Q = Keq
15. The equilibrium constant in a reversible chemical reaction at a given temperature
(a) Depends on the initial concentration of the reactants
(b)
Depends on the concentration of one of the products at equilibrium
(c)
Does not depend on the initial concentration of reactants
(d)
Is not characteristic of the reaction
16. When a system
is at equilibrium states:
(a) the
concentration of reactants and products becomes equal
(b) the
opposing reactions (forward and reverse) stop
(c) active
mass is represented by small brackets
(d) active
mass of all reacting species becomes constant.
17. Which one of
the following statement is not
correct about active mass?
(a) rate of reaction is directly proportional to active mass
(b) active mass is taken in molar concentration
(c) active
mass is represented by square brackets
(d) active
mass of all reacting species at equilibrium becomes equal.
18. The characteristics of reversible reactions are the following except;
(a) products never recombine to form reactants
(b) they never complete
(c) they proceed in both ways
(d) they have a double arrow between reactants and
products
19. When the magnitude of Kc is very large it indicates;(a) reaction mixture consists of almost all products
(b) reaction mixture has almost all reactants
(c) reaction has not gone to complete
(d) reaction mixture has negligible products
20. When the
magnitude of Kc is very small it indicates;
(a) equilibrium will never establish
(b) all reactants will be converted into products
(c) reaction will go to completion
(d) the amount of products is negligible
21. At dynamic equilibrium;
(a) the reaction stops to proceed
(b) the amount of reactants and products are equal
(c) the speed of the forward and reverse reaction are
equal
(d) The
reaction can no longer be reversed
22. In an
irreversible reaction, dynamic equilibrium;
(a) never establishes
(b)
establishes before the completion of reaction
(c) establishes after the
completion of reaction
(d) establishes readily
23. A reverse reaction is one that;
(a) which proceeds from left to right
(b) In which the reactants react to form products
(c) which slows down gradually
(d) which speeds up gradually
24. The
reaction which never goes to completion is called:
(a) Exothermic reaction
(b) Endothermic reaction
(c) Reversible reaction
(d)
Irreversible rxn
25.The rate at which substance react is directly proportional to its active mass and the rate of chemical reaction is proportional to the product of active masses of the reacting substances. It is called
(a) Law of mass action
(b) Rate Law
(c) Hess’s law
(d) None of them
26. In Kc
expression, the active masses of ………….. appear in numerator
(a)Products
(b)Reactants
(c) Catalyst
(d)
None of them
27. in Kc expression, the active masses of …….. appear in denominator
(a) Products
(b) Reactants
(c) Catalyst
(d) None of them
28.In which of the following case does the reaction go farthest to completion
(a) Kc = 102
(b) Kc = 10−2
(c) Kc = 10
(d) Kc = 1
29. In which of the following case does the reaction not go farthest to completion
(a) Kc = 102
(b) Kc = 10−2
(c) Kc = 10
(d) Kc = 1
30. A catalyst speeds up the rate of ……….. reaction.
(a) Forward
(b) Backward
(c) Both forward and backward
(d) None of them
31. The reaction between alcohol and acid is called
(a) Hydrolysis
(b) Neutralization
(c) Saponification
(d) Esterification
32. For a reversible reaction, if the concentration of the both the reactants are doubled, then equilibrium constant is:
(a) Also doubled
(b) halved
(c) Quadrupled
(d) Not changed
33. The value of Kc does not depend on _______.
(a) Temperature
(b) Initial concentration
(c) Both of them
(d) None of them
34. If Kc is very large, then reaction is considered to be _______
(a) Reversible
(b) Irreversible
(c) Exothermic
(d) None of them
35. In a reversible chemical reaction having
two reactants in equilibrium, if the concentration of the reactants are doubled
then equilibrium constant will
(a) Also be doubled
(b) Remains the same
(c) Becomes one fourth
(d) Be halved
36. For the reaction, A + B ⇌ C, the equilibrium constant unit is
(a) dm3 mol‒
(b) mol dm‒3
(c) moldm3
(d) mol2dm‒3
Reason
37. The reaction in which the products do not recombine to form reactants are called;
(a) Reversible reactions
(b) Irreversible reactions
(c) Decomposition
(d) Addition
38. The reaction in which the products can recombine to form reactants are called:
(a) Reversible reactions
(b) Irreversible reactions
(c) Decomposition
(d) Addition
39 The colour of iodine is:
(a) purple
(b) Black
(c) red
(d) Pink
40. The colour of hydrogen iodide is:
(a) colourless
(b) black
(c) red
(d) pink
41. When the rate of the forward reaction takes place at the rate of reverse action, the composition of the reaction mixture remains constant it is called:
(a) Static equilibrium
(b) Dynamic equilibrium
(c) Chemical equilibrium
(d) all
42. Guldberg and Waage put forward law of mass action in
(a) 1860
(b) 1864
(c) 1870
(d) 1879
43. The %age of nitrogen and oxygen in our atmosphere is
(a) 80
(b) 90
(c) 95
(d) 99
44. Which gas is used to prepare ammonia?
(a) N2
(b) O2
(c) Cl2
(d) S
45. Which gas is used to manufacture king of chemicals sulphuric acid?
(a) N2
(b) O2
(c) Cl2
(d) SO2
46. Equilibrium constant has no unit when number of moles of reactants and products are;
(a) same
(b) different
(c) both a & b
(d) none
47. For reactions having large Kc value, the
reaction proceeds to;
(a) completion
(b) equilibrium state
(c) backward
(d)
None
48. For the reaction, 2A(g) + B(g) ⇌ 3C(g) the expression for the equilibrium constant is:
(a) [2A][B]/[3C]
(b) [A]2[B]/[C]3
(c) [3C]/[2A][B]
(d) [C]3/[A]2[B]
49. Reactions which have comparable amounts of reactants and products at equilibrium state have;
(a) very small Kc value
(b) very large Kc value
(c) moderate Kc value
(d) none of these
50. Nitrogen and
hydrogen were reacted together to make ammonia
N2 + 3H2 ⇌ 2NH3 K c= 2.86 mol−2dm6
What will be present in the equilibrium mixture?
(a) NH3 only
(b) N2, H2 and NH3
(c) N2 and H2
(d) H2 only
51. For a reaction between PCl3 and Cl2 to form PCl5, the units of Kc are;
(a) mol dm−3
(b) mol−1 dm−3
(c) mol−1 dm3
(d) mol dm3
Explanation; (c)
Unit of Kc = (concentration)∆n
Þ (mol1 dm−3)1‒2
Þ (mol1 dm−3)‒1
Þ mol−1
dm3
52. The two major components of atmosphere are
(a) carbon and nitrogen
(b) Nitrogen and oxygen
(c) Oxygen and chlorine
(d) None of these
53. Which type of reactions do not go to completion?
(a) Irreversible reaction
(b) Reversible reactions
(c) Addition reactions
(d) Decomposition
54. Which type of reaction speed up gradually?
(a) Irreversible reaction
(b) Reversible reactions
(c) Addition reactions
(d) Decomposition
55. Which type of reactions take place in both directions?
(a) Addition reactions
(b) Reversible reactions
(c) Irreversible reactions
(d) Decomposition
56. In a chemical reaction, the substance that combine are called;
(a) reactants
(b) products
(c) mass
(d) material
57.Dynamic means, reaction is;
(a) in forward direction
(b) still continuing
(c) in reverse direction
(d) stop
58. The forward reaction takes place:
(a) right to left
(b) left to right
(c) only to right
(d) only to left
59. The units of molar concentration:
(a) mol.dm−2
(b) mol.dm−1
(c) mol.dm
(d) mol.dm−3
60. Equilibrium constant value “Kc“ is equal to;
(a) Kf/Kr
(b) Kr /Kf
(c) Kc/Qc
(d) Qc/Kr
61. Which chemical is called king of chemicals?
(a) KNO3
(b) H2SO4
(c) HCl
(d) NHO3
62. The rate at which substance react is
directly proportional to its active mass and the rate of chemical reaction is proportional to the product of active
masses of the reacting substances. It is
called
Explanation; (a)
In 1864, two Norwegian chemists
Cato Maximillian (C.M) Guldberg (1836–1902) and Peter (P) Waage (1833–1900)
studied experimentally a number of equilibrium reactions and put forward their
results as a generalization known as law of mass action or equilibrium law.
This law gives a quantitative relationship between the rate of reaction and the
active mass (molar concentration) of reacting substances.
63. For a chemical reaction aA + bB ⇌ cC + dD, Kc expression is written
as:
66. Using molar concentrations, what is the unit of Kc for the following reaction?
(a) M‒2
(b) M2
(c) M‒1
(d) M
Explanation; (b)
Unit of Kc = (concentration)∆n Þ (M)3‒1 Þ M2
65. What is the equlirbium expression for the reaction;
P4(s) + 5O2(g) ⇌ P4O10(s)
Explanation; (d)
Concentration
of pure solid or pure liquid does not appear in the
equlirbium expression. Since P4 and P4O10 are
solids, they are not written in the Kc formula.
Kc
= 1/[O2]5
66. What is the equilibrium constant (Kc)
for the given reaction
2S(s) + 3O2(g) ⇌ 2SO3(g)
Explanation; (d)
Concentration of pure solid or pure liquid does not
appear in the equilibrium expression. Since, S is
a solid reactant, so it does not include in the Kc expression.
67. Which of the following expression of Kc is correct
for following reaction? N2O4 ⇌ 2NO2
Explanation; (c)
[Product] = [NO2]2
= is written in numerator (coefficient becomes power of concentration)
[Reactant] = [N2O4]
= is written in denominator
So the correct option is c.
68. Which of the following is the unit of Kc for
following reaction?
N2(g) +
3H2(g) ⇌ 2NH3(g)
Explanation; (a)
(concentration)∆n Þ (mole dm–3)2‒4 Þ (mole dm–3)‒2 Þ mole–2
dm6
69. What is the equilibrium constant, Kc,
for this reaction?
CO2(g) +
3H2(g) ⇌ CH3OH(g)
+ H2O(g)
Explanation; (a)
Correct option is a.
[Product] = [CH3OH][H2O] = is
written in numerator (coefficient becomes power of concentration)
[Reactant] = [CO2] [H2]3
= is written in denominator (coefficient becomes power of concentration)
Multiple Choice Questions (MCQs) on Acids, Bases and Salts from Text Book
1. Corrosive effect on skin is caused by
(a) Acid
(b) Base
(c) Salt
(d) Both a and b
2. Preservatives are used preserve
(a) Acid
(b) Base
(c) Food
(d) Water
3. Which of the following is NOT an Arrhenius acid?
(a) HCl
(b) CO2
(c) HNO3
(d) H2SO4
4. NH3 can be a base according to
(a) Arrhenius theory
(b) Bronsted-Lowry theory
(c) Lewis theory
(d) Both b and c
5. Which of the following is a Lewis base?
(a) HNO3
(b) CN−
(c) HCl
(d) AlCl3
6. A substance that can donate a pair of electrons to form coordinate covalent bond
(a) Bronsted-Lowry base
(b) Bronsted Lowry acid
(c) Lewis acid
(d) Lewis base
7. If pH value is greater than 7, then solution is
(a) Acidic
(b) Basic
(c) Amphotetic
(d) Neutral
8. Salt among following is
(a) HCl
(b) KCl
(c) HNO3
(d) H2SO4
9. Substance that react with both acids and bases are called
(a) Amphotetic substances
(b) Conjugate acids
(c) Conjugate base
(d) Buffers
10. The reaction of acid and base to form salt and water is called
(a) Hydration
(b) Neutralization
(c) Hydrolysis
(d) both a and c
Answers of MCQs on Acids, Bases and Salts from Text Book
1…….. D
2.…….. C
3.…….. B
4.…….. D
5.…….. B
6.…….. D
7.…….. B
8.…….. B
9.…….. A
10.…… B
Multiple Choice Questions (MCQs) on Acids, Bases and Salts from Past Papers and External Source
For Answers contact me on WhatsApp 03009215999
1. The substance whose aqueous solution change the blue litmus to red:
(a) Acids
(b) Bases
(c) Salts
(d) Neutral
2. The substances having a tendency to lose one or more protons are called:
(a) Acids
(b) Bases
(c) Salts
(d) Neutral
3. The substance which donate the pair of electrons for bond formation are known as:
(a) Acids
(b) Bases
(c) Salts
(d) Neutral
4. When equivalent quantities of acid and base are mixed, salt and water are formed, the reaction is termed as:
(a) Hydration
(b) Hydrolysis
(c) Neutralization
(d) None of these
5. The acids which contain one acidic hydrogen are called
(a) Diprotic
(b) Monoprotic
(c) Triprotic
(d) Polyprotic
6. The number of acidic hydrogen atoms present in a molecule of an acid is called:
(a) Acidity
(b) Basicity
(c) Neutrality
(d) Hydrolysis
7. The number of replaceable OH− ions present in a molecule of base is called:
(a) Acidity
(b) Basicity
(c) Neutrality
(d) Hydrolysis
8. An ionic compound that is formed when an acid neutralizes a base is called:
(a) Acids
(b) Bases
(c) Salts
(d) Indicator
9. The formula of washing soda is:
(a) Na2CO3
(b) Na2CO3.6H2O
(c) Na2CO3.10H2O
(d) NaHCO3
10. The formula of baking soda is ……………..
(a) Na2CO3
(b) Na2CO3.6H2O
(c) Na2CO3.10H2O
(d) NaHCO3
11.The formula of Epsom salt is ………….
(a) Na2CO3
(b) MgSO4.7H2O
(c) Na2CO3.10H2O
(d) NaHCO3
12. A solution whose strength is known is called ………….
(a) Molar solution
(b) Standard solution
(c) Normal solution
(d) None of them
13. If H+ ion concentration of a solution is 1 x 10−14 M, the solution is ………..
(a) Molar solution
(b) Acidic solution
(c) Neutral solution
(d) Basic Solution
14. If the OH− ion concentration of a solution is 1 x 10−10 M, solution is ……….
(a) Basic
(b) Acidic
(c) Neutral
(d) Normal
15. The solution whose pH is 6, then its H+ ion concentration is ……………
(a) 1 x 10−4 M
(b) 1 x 10−6 M
(c) 1 x 10−14 M
(d) 1 x 10−2 M
16. ………….. is the process by which we can determine the concentration of unknown solution with the help of standard solution.
(a) Titration
(b) Sublimation
(c) Crystallization
(d) None of them
17. The volume of a pipette is generally ………… ml or cm3.
(a) 10
(b) 20
(c) 25
(d) 50
18. The solution whose H+ ion concentration is 1 x 10−4 M, then its pH is ………..
(a) 4
(b) 8
(c) 7
(d) 10
19. The pH value of Human blood is
(a) 7.35-7.45
(b) 7.8
(c) 7.2
(d) 7.0
20. The formula of sodium hydrogencarbonate is
(a) Na2CO3
(b) NaHCO3
(c) Na2CO3.10H2O
(d) Na2CO3.6H2O
21. The pH value of distilled water is
(a) 1
(b) 4
(c) 7
(d) 14
22. Chemically strong acid is
(a) Acetic acid
(b) Nitric acid
(c) Hydrochloric acid
(d) Sulphuric acid
23. What is the pH of a neutral solution?
(a) 0
(b) 1
(c) 7
(d) 14
24. The pH value of saliva is
(a) 4.2
(b) 6.5
(c) 7.0
(d) 7.8
25. Which of the following substances is called proton donor?
(a) Acids
(b) Bases
(c) Salts
(d) Alkali
26. It is a proton donor
(a) Acid
(b) Base
(c) Salt
(d) Alkali
27. A specie formed by the loss of proton from an acid is called a…………..
(a) Lewis base
(b) Conjugate base
(c) Conjugate acid
(d) Arrhenius acid
28. A specie formed by the addition of a proton to a base is called ………..
(a) Lewis base
(b) Conjugate base
(c) Conjugate acid
(d) Arrhenius acid
29.In the reaction; NH3 + HCl → NH4+ + Cl–; which one is conjugate base?
(a) NH3
(b) HCl
(c) Cl–
(d) NH4+
30. In the reaction; CH3COOH + H2O ⇌ H3O+ + CH3COO–; which one is conjugate base?
(a) H3O+
(b) H2O
(c) CH3COO–
(d) CH3COOH
31. In the reaction; NH3 + H2O ⇌ NH4+ + OH–, which one is conjugate acid?
(a) NH3
(b) H2O
(c) OH–
(d) NH4+
32. The conjugate base of a strong acid is always a……………
(a) Weak base
(b) Weak acid
(c) Strong acid
(d) Strong acid
33. The conjugate acid of a strong base is always a……………
(a) Weak base
(b) Weak acid
(c) Strong acid
(d) Strong acid
34. HCl is a strong acid since its conjugate base Cl– is a………….
(a) Weak base
(b) Weak acid
(c) Strong acid
(d) Strong acid
35. Which one of the following is a monoprotic acid?
(a) H2C2O4
(b) H2SO4
(c) H4C2O2
(d) C6H4(COOH)2
36. Which one of the following is NOT a dibasic acid?
(a) H2C2O4
(b) H–HSO4
(c) H6C4O4 (succinic acid)
(d) H3BO3
37. Which one is NOT a Lewis base?
(a) NH3
(b) NaNH2
(c) C2H5OH
(d) AlCl3
38. Which one is NOT a Lewis acid?
(a) AlCl3
(b) FeCl3
(c) BF3
(d) NH3
39.The value of ionic product (Kw) of water at 25ºC is equal to:
(a) 1 x 1014
(b) 1 x 10-14
(c) 1 x 10-7
(d) 1 x x 10-10
40. The sum of pH and pOH of any solution at 25ºC is:
(a) 7
(b) 9
(c) 14
(d) 3
41. A solution which contains [H+] concentration equal to 10-7 M is said to be:
(a) Acidic
(b) Neutral
(c) Basic
(d) Alkaline
42. A solution which contains [H+] concentration less than 10-7 M is said to be:
(a) Acidic
(b) Basic
(c) Alkaline
(d) Neutral
43. A solution which contains [H+] concentration greater than 10-7 M is said to be:
(a) Acidic
(b) Basic
(c) Neutral
(d) Amphoteric
44. The hydroxyl ion concentration in a solution having pH value 3 will be:
(a) 10-14 M
(b) 10-7 M
(c) 10-12 M
(d) 10-11 M
45. The hydroxyl ion concentration in a solution having pH value 12 will be:
(a) 10-2 M
(b) 10-7 M
(c) 10-12 M
(d) 10-10 M
46. The pH of a solution with hydrogen ion concentration of 1 x 10-3 is:
(a) 3
(b) 2
(c) 1
(d) 11
47. The pH of a solution that has 0.00001 mole of H+ per liter of solution is:
(a) 2
(b) 5
(c) 4
(d) 9
48. Which one of the following substances has pH value less than 7?
(a) Milk of magnesia
(b) Sea water
(c) Blood
(d) Milk
49. Which one of the following substances has pH value more than 7?
(a) Vinegar
(b) Sodium carbonate
(c) Sulphuric acid
(d) Soda water
50. Which of the following salts has no water of crystallization?
(a) Gypsum
(b) Blue vitriol
(c) Baking soda
(d) Washing soda
51. Metal carbonate on reaction with dilute acid release
(a) CO2
(b) H2O
(c) CO
(d) H2
52. ln general, dissolution of acid or base in water is
(a) Exothermic
(b) Endothermic
(c) Violent
(d) None of these
53. Hydrogen ions produced by acid exist in which of the following form?
(a) Hydroxonium ions
(b) Hydrogen
(c) Water ions
(d) Hydroxide ions
54. The acid found in an ant sting is
(a) Tartaric acid
(b) citric acid
(c) Methanoic acid
(d) Acetic acid
55. Which one of the following acid in not monoprotic?
(a) H3BO3
(b) CH3COOH
(c) HNO3
(d) HO-SO3H
56. Universal indicator turns red in:
(a) Acid solution
(b) Alkaline solution
(c) Neutral solution
(d) Basic solution
57. The pH of milk is:
(a) 7.3
(b) 6.0
(c) 6.3
(d) 5.6
58. 7.3 is the pH of:
(a) Human blood
(b) Tomato juice
(c) Vinegar
(d) Milk
59. The acids which contain two or more acidic hydrogens are called:
(a) Monoprotic
(b) Diprotic
(c) Triprotic
(d) Polyprotic
60. The basicity refers to the number of ionizable ………… ions:
(a) H+
(b) OH−
(c) H2
(d) both a and b
61. If H+ ions concentration of solution is 1 x 100 M, then solution is strongly
(a) Acidic
(b) Basic
(c) Neutral
(d) Amphoteric
62. Universal indicator turns green in:
(a) Neutral solution
(b) Alkaline solution
(c) Acid solution
(d) Basic solution
63. The pH of saliva is:
(a) 7.3
(b) 6.0
(c) 6.3
(d) 5.6
64. Which one of the following is not a strong acid?
(a) HF
(b) HNO3
(c) HCl
(d) H2SO4
65. What will be the value of pH of 10−5 M NaOH solution?
(a) 5
(b) 8
(c) 9
(d) 10
66. What is the pH of a 0.00001 molar HCl solution?
(a) 1
(b) 9
(c) 5
(d) 4
67. The pH of milk of magnesia is
(a) 1.2 %
(b) 1.4 %
(c) 1.9 %
(d) 2.1 %
69. What is the pOH of a solution whose pH is 8?
(a) 6
(b) 10
(c) 4
(d) 2
70. Lime water turns milky when carbon dioxide is passed due to the formation of ______.
(a) CaCO3
(b) CO2
(c) CaO
(d) CaSO4
71. Which ion is not present in dilute sulfuric acid?
(a) H+
(b) OH–
(c) SO32–
(d) SO42–
72. Which oxide will produce the solution with the highest pH when it is mixed with water?
(a) Al2O3
(b) SO2
(c) Na2O
(d) CO2
73. Metal carbonate on reaction with dilute acid release:
(a) H2O
(b) H2
(c) CO2
(d)CO
74. Identify the conjugate acid of SO42−
(a) H2SO4
(b) SO32−
(c) HSO4−
(d) H2SO3
75. Which one of the following is a weak acid?
(a) HF
(b) HClO3
(c) HNO3
(d) HI
76. Which one of the following is a STRONG electrolyte?
(a) HF
(b) KF
(c) HNO2
(d) (CH3)3N
77. Which of the following is classified as a conjugate acid-base pair?
(a) HCl/NaOH
(b) H3O+
(c) O2/H2O
(d) H+/Cl−
78. pOH of pure water at 25ºC is _____________.
(a) 7
(b) 14
(c) 0
(d) -7
79. Acid + Metal oxide → -----------
(a) Base + water
(b) Base + salt
(c) Salt + water
(d) Metal + salt
80. What is formed by the reaction of a non-metal oxide with water?
(a) Acid
(b) Base
(c) Salt
(d) Metal
81. Which of the following solutions is most basic?
(a) pH = 10.6
(b) pH = 11.5
(c) pH = 9.3
(d) pH = 8.2
82. What is used to measure the exact pH of an aqueous solution?
(a) pH paper
(b)Universal indicator
(c) pH meter
(d) Litmus paper
83. Which of the following substances is an antacid?
(a) NaCl
(b) Mg(OH)2
(c) HCl
(d) H2SO4
84. The pH values of solutions A, B, C and D are 1.9, 2.5, 2.1 & 3.0, respectively. Their order of acidity will be
(a) D < C < B < A [C]
(b) D > C > B > A
(c) A < C < B < D [B]
(d) D < B < C < A
85. Which solution will be basic?
(a) [H3O+] = 10−5 M
(b) [H3O+] = 10−12 M
(c) [H3O+] = 10−7 M
(d) [H3O+] = 10−4 M
86. The bond between H+ and H2O in H3O+ is...
(a) Coordinate covalent
(b) Covalent
(c) Metallic
(d) Ionic
87. The hydroxonium ion is
(a) Hydrated proton
(b) Protonated water molecules
(c) Both of them
(d) None of them
88. Whose definition of acids and bases emphasizes the role of protons?
(a) Brønsted and Lowry
(b) Arrhenius
(c) Faraday
(d) Lewis
89. An electron-pair acceptor is a
(a) Lewis base
(b) Brønsted-Lowry base
(c) Lewis acid
(d) traditional acid
90. What is the pH of 1 x 10–4 M HCl solution?
(a) 4
(b) 10
(c) 8
(d) 6
91. What is the pH of a 1 x 10–5 M KOH solution?
(a) 3
(b) 5
(c) 9
(d) 11
92. Which are the correct products for these reactants H2SO4 + NaOH?
(a) Na2SO4 + H2O
(b) Na2SO4 + OH–
(c) NaHSO4 + H2O
(d) Both a and c
93. Which element is always present in Arrhenius acid?
(a) Nitrogen
(b) Hydrogen
(c) Oxygen
(d) None of these
94. Which one of the following is a strong electrolyte?
(a) HF
(b) KF
(c) HNO2
(d) H2O
95. The conjugate base of HSO4– is
(a) H2SO4
(b) H3SO4+
(c) SO42–
(d) HSO4+
96. Which of the given is a strong base?
(a) Potassium hydroxide
(b) Magnesium hydroxide
(c) Ammonium hydroxide
(d) Calcium hydroxide
97. A Bronsted-Lowry base is defined as:
(a) a hydroxide acceptor
(b) an electron pair acceptor
(c) a proton acceptor
(d) a hydroxide donor
98. The conjugate acid of HSO4– is
(a) H2SO4
(b) HSO4 +
(c) SO42–
(d) HSO3+
99.According to Arrhenius acid-base theory, in neutralization reaction, which molecule is formed?
(a) CO2
(b) H2O2
(c) H2O
(d) H2
100. The conjugate acid of HPO32– is
(a) HPO32−
(b) H2PO31−
(c) PO33−
(d) H3PO3
101. The conjugate base of NH3 is
(a) NH4+
(b) NH2–
(c) NH2–
(d) None of them
102. A conjugate acid forms a conjugate base by ……. of a proton
(a) Accepting
(b) Donating
(c) Gaining
(d) None of them
103. A strong base would have a ……… conjugate acid.
(a) Strong
(b) Very strong
(c) Weak
(d) None of them
104. The conjugate acid of O2– is
(a) OH−
(b) H2O
(c) H3O+
(d) None of them
105. …… acid-base theory cannot define that NH3 is a base
(a) Lewis
(b) Bronsted-Lowry
(c) Arrhenius
(d) None of them
106. HSO4– is conjugate acid of ….
(a) H2SO4
(b) SO42–
(c) H2O
(d) None of them
107. Which of these species will act as a Lewis acid?
(a) NH3
(b) H2O
(c) NH4+
(d) BF3
No comments:
Post a Comment