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| Chemistry 10th Chapter 10 Acid, Base and Salts Questions Bank |
Chemistry 10th Chapter 10 Acid, Base and Salts Solved MCQs, Short and Long Questions
Select the right Answer.
1. _______ formula represents group of atoms joined together to each carbon atom.
2. __salts are often prepared in water:
3. “Kw” is k own as:
4. A anion is derived from:
5. A base is a substance which neutralizes an acid. Which of these substances is not a base?
6. A cation is derived from:
7. A reaction between an acid and a base produces:
8. A salt always:
9. A salt is composed of:
10. A solution HCl is 0.001 M. what is pH value?
11. A solution of a compound of pH 7 or pOH 7 is considered a:
12. A solution of pH = 1 has times higher concentration of H* than a solution of pH = 2:
13. A specie which is able to accept a proton is called
14. A substance that donates a pair of electrons to form coordinate covalent bond is called
15. According to Lewis concept the specie is called acid which can:
16. According to the Lewis concept, acid is a substance which can:
17. Acetic acid is used for:
18. Acid used for food preservation:
19. Acidic salts turn __ litmus into red:
20. Acids ionize in water to produce
21. Al(OH)₃ is:
22. All bronsted bases are
23. Ammonia is a base because it:
24. As an electrolyte, water is
25. At which pH methyl orange change color:
26. At which pH phenolphthalein change color:
27. Bases leaves blue litmus
28. Bases react with acid to form:
29. Bronsted lowery acid
30. Calcium sulphide has water of crystallization:
31. Concentration of __ in pure water is the basis for pH scale
32. Copper sulphate has _____ molecules of water of crystallization.
33. Corrosive effect on skin is caused by
34. CuSO₄ can be prepared by the reaction of:
35. Dilute acids react with carbonates to produce the given products except:
36. Double salts are formed by two:
37. Ferric hydroxide (Fe(OH)₃) is precipitated out of solution when sodium hydroxide solution is added to ferric chloride. FeCl₃ + 3NaOH --------->Fe(OH)₃ Colour of the precipitates is:
38. FeSO₄.(NH₄)₂ SO₄.6H₂O is:
39. Formula of phosphoric acid is:
40. Given Kw = [H⁺][OH⁻] = 1.0 x 10⁻¹⁴ at 25C . what is the concentration of H⁺ in pure water at 25c?
41. H₃PO₄ is the formula of:
42. H₃PO₄ + NaOH NaH₂PO₄ + H₂O is an example of :
43. HCI + KOH →→KCI + H₂O is an example of:
44. Heat resistance glass is:
45. High value of pH means:
46. Humphrey Davy proved the presence of as the main constituents of all acids
47. If a liquid has a pH of 7 then it must:
48. If the concentration of H⁺ is greater than 1 x 10⁻⁷ then solution is
49. If the pH value is greater than 7, then solution is
50. In ______, G. N. Lewis proposed his concept of acids and bases.
51. In a reaction between ammonia & borontrifloride , BF₃ is
52. In etching process, the glass or mirror is dipped into:
53. In pure water, the concentrations of
54. In the preparation of insoluble salts, which one of the facts is incorrect?
55. Indicators are:
56. Indicators have_ colour in acidic or basic solution:
57. Ionic product constant depends on :
58. It is a common indicator.
59. It is found in stings of bees and ants:
60. It is much more reliable and accurate method of measuring pH:
61. It is used in etching designs on copper plates:
62. It is used to cure sting of wasps:
63. It is used to treat bee’s sting
64. KOH is used in making of
65. Lewis acid-base concept has the following characteristics except:
66. Litmus is _ in acidic solution:
67. Litmus is _in basic solution:
68. Low pH value means:
69. Maleic acid is found from
70. Metallic oxides are:
71. Methyl orange is _ in alkaline solution :
72. Molecule containing an atom with unshared pair of electron is:
73. Mostly insoluble metallic oxides react with to form salt and water:
74. Neutralization is reaction of
75. Nitric acid was prepared by
76. pH =_
77. pH meter consists of:
78. pH of a neutral solution is always:
79. Phenolphthalein in acidic solution is
80. Preservatives are used to preserve
81. Reaction of acid and a metal is called reaction:
82. Salt have:
83. Salts are found in:
84. Salts are the __________ compounds generally formed by neutralization.
85. Salts are:
86. Salts may be:
87. Sodium carbonate, Sodium sulphate and sodium silicate are used to manufacture:
88. Solution of pH less than are acidic.
89. Solution of pH more than 7 are:
90. Sour milk has ______ acid.
91. Stomach acidity is also called :
92. Substances that react with both acids and bases are called
93. The acid used for the manufacture of fertilizers and explosives is
94. The amount of Hydrochloric Acid (HCl) secreted daily by gastric glands is
95. The Bronsted-Lowery acid in the reaction H₂O + NH₃ NH⁺ 4 + OH⁻ is
96. The colour of phenolphthalein is _____ in a solution having pH more than nine
97. The conjugate acid of HPO₄-2 is:
98. The final product of arrhenius concept is
99. The first acid known to man was:
100. The formula of bleaching powder is:
101. The negative logarithm of molar concentration of hydrogen ions is called:
102. The pH (power of Hydrogen) value of black coffee is
103. The pH at which methyl red changes color is
104. The pH of water is
105. The product of any Lewis acid base reaction is a single specie:
106. The product of Lewis acid-base reaction is called adduct. The bond between the adduct specie is:
107. The range of pH scale is from:
108. The reaction between an acid and a base produce:
109. The salt among the following is
110. The sum of pH and pOH at 25°C is
111. The sum of pH scale and pOH is always :
112. The water of crystallization is responsible for the:
113. The word acid is derived from
114. There are types of salts:
115. These can act as Lewis acids
116. These can act as Lewis bases
117. Uric acid is present in
118. Washing soda has water of crystallization:
119. Water ionizes slightly into ions is a process called:
120. Water is:
121. What is pH value of 0.01 M solution of KOH?
122. What is pH value of 0.01 M sulphuric acid ?
123. What is the pOH of 0.02M Ca(OH)₂?
124. When a metal replaces hydrogen atom then compound form is
125. When acid reacts with metal carbonate, all of the following are formed except:
126. When acid reacts with metal carbonate, the products are
127. When acids react with carbonates and bicarbonates, which evolves out:
128. When Na reacts with HCl the salt produced is:
129. Which ion is a conjugate base of sulphuric acid?
130. Which is amphoteric:
131. Which of the following is not a base?
132. Which of the following is not a mineral acid?
133. Which of the following species is not amphoteric?
134. Which of the following statement is incorrect about acids?
135. Which one of the following is a Lewis base?
136. Which one of the following species is not amphoteric?
137. You want to dry a gas, which one of the following salt you will use:
Short Questions
1. A solution of hydrochloric acid is 0.01M. What is its pH value?
2. Complete and balance the following equation: H₂SO₄+NaHCO₃→
3. Define a base and explain all alkalies are bases, but all bases are not alkalies.
4. Define acid and base according to Lewis theory.
5. Define Adduct.
6. Define and give the characteristics of a Lewis acid.
7. Define Arrhenius acid.
8. Define Arrhenius acid. Give an example.
9. Define Arrhenius base. Give an example.
10. Define Bronsted –Lowry base?
11. Define Bronsted-Lowry acid and base.
12. Define Bronsted-Lowry base and explain with an example that water is a Bronsted-Lowry base.
13. Define conjugate acid and conjugate base.
14. Define double salts. Give two examples.
15. Define neutralization reaction. Give an example.
16. Define pH. What is the pH of pure water?
17. Define salts. Write two examples of salts.
18. Differentiate between ‘p’ and pH.
19. Discuss the important uses of washing soda and write its chemical name and formula.
20. Find out the pH and pOH of 0.001M solution of KOH?
21. Find the pH of 0.01M sulphuric acid?
22. Give a few characteristic properties of salts.
23. Give a reaction of an acid with metal.
24. Give any example of neutralization reaction.
25. Give any two properties of salts.
26. Give the chemical formula and uses of Calcium Chloride.
27. Give the limitation/s of Arrhenius concept.
28. Give the preparation of insoluble salts
29. Give the uses of nitric acid.
30. Give the uses of sulphuric acid.
31. H₃PO₄ is a weak acid but its salt (Na₃PO₄) with strong base NaOH is neutral. Explain it.
32. HCI and H₂SO₄ are strong acids. While their solutions are equimolar, they have different pH value as calculated in problem 10.2 and 10.4. Why they have different pH values?
33. How are salt prepared by the reaction of a metal and acid?
34. How are salt prepared by the reaction of an acid and metallic oxide?
35. How are the insoluble salts prepared?
36. How are the salts named?
37. How are the soluble salts recovered from water?
38. How can we measure pH of a solution?
39. How can you justify that Bronsted –Lowry concept of acid and base is applicable to non-aqueous solutions?
40. How can you justify that NH₃ is Bronsted-Lowry base but not Arrhenius base?
41. How can you justify that Pb(OH)NO₃ is a basic salt?
42. How do the basic salts turn into normal salts? Explain with an example.
43. How many times a solution of pH 1 will be stronger than that of a solution having pH₂?
44. How many water of crystallizations are present in CuSO₄.5H₂O and CaSO₄.2H₂O?
45. Na₂SO₄ is a neutral salt while NaHSO₄ is an acidic salt. Justify.
46. Na₂SO₄ is a neutral salt. What are its uses?
47. Name an acid used in the preservation of food.
48. Name an alkali used in alkaline batteries.
49. Name any two acids prepared by Jabir Bin Hayan.
50. Name any two acids which are used to preserve the food.
51. Name some mineral acids.
52. Name some sources of tartaric acid.
"53. Name the acids present in:
i. Vinegar ii. Ant sting
iii. Citrus fruit iv. Sour milk"
54. Name the gas liberated when alkalies react with ammonium salts.
"55. Name the salts which are formed when Zn metal reacts with following acids.
a. nitric acid b. phosphoric acid c. acetic acid"
56. Name the type of reaction that takes place between an acid and a metal. Which gas would evolve in the reaction? Explain with an example.
57. Name the types of salts.
"58. Name three common household substances having:
1. pH values greater than 7
2. pH values less than 7
3. pH values equal to 7 "
59. Name two acids used in the manufacture of fertilizers.
60. NH₃ is Bronsted-Lowry base but not Arrhenius base. Justify.
61. Prove that water is an amphoteric specie.
62. Quote any two properties of acids.
63. Quote any two properties of bases.
64. Simple cations can act as Lewis acids. Why?
65. State and explain the neutralization reaction according to Lewis concept.
66. Two solutions are having pH 1 and pH₂, Identify the stronger solution. How many times a solution is stronger than the other?
67. Water is an amphoteric specie according to Bronsted- Lowry concept. What is its nature according to Lewis concept?
68. What are acidic salts? Write one chemical equation of their reaction with bases.
69. What are amphoteric substances?
70. What are complex salts?
71. What are indicators? Write names of any two indicators.
72. What are Mixed salt. Give an example.
73. What are universal indicators?
74. What do you mean by neutralization reaction according to Arrhenius acid-base concept?
75. What is acid and a basic radical?
76. What is amphoteric substance? Give an example.
77. What is an adduct?
78. What is meant by water of crystallization? Give an example.
79. What is the difference between Arrhenius base and Bronsted-Lowry base?
80. What is the difference between Lewis acid and base?
81. What is the importance of NaCl?
82. What is the molecular formula of decane?
83. What is the value of pH at which methyl orange changes its colour?
84. When acids react with carbonates and bicarbonates, which gas evolves?
85. When and what was discovered by Sir Humphrey Davy?
86. Which acid is found in apples?
87. Which gas is evolved when zinc metal reacts with an acid?
88. Which kind of bond forms between Lewis acid and base?
89. Which salt is used to prepare plaster of paris?
90. Which types of salts produce SO₂ gas on reacting with acids?
91. Why BF₃ behaves as a Lewis acid?
92. Why does H⁺ ion acts as a Lewis acid?
93. Why ionic-product constant of water is temperature dependent?
94. Why is a salt neutral? Explain with an example.
95. Why is water termed as an amphoteric specie?
96. Why pure water is not a strong electrolyte?
97. Write down characteristic properties of Acids.
98. Write down characteristic properties of Bases.
99. Write down chemical formula and the important uses of sodium tetraborate.
100. Write down limitations of Bronsted-Lowry concept.
101. Write down sources of Malic acid and Stearic acid.
102. Write down the chemical formula and uses of Sodium Chlorate.
103. Write down the chemical formula uses of acetic acid.
104. Write down the colours of the precipitates formed by reaction of aqueous caustic soda with solutions of: copper, zinc and ferric salts.
105. Write down the formula and uses of ammonium hydroxide.
106. Write down the formula and uses of nitric acid.
#NAME?
108. Write down the formulae of silver acetate and calcium phosphate.
109. Write down the name and formula of alkali used in alkaline batteries.
110. Write down the names and formulae of three mineral acids.
111. Write down the names of two natural acids and their sources
112. Write down two chemical properties of bases.
113. Write down uses of ‘pH’.
114. Write down uses of hydrochloric acid.
115. Write down uses of sodium hydroxide and magnesium hydroxide.
116. Write names of any two methods of preparation of salts.
117. Write sources of citric acid and lactic acid.
118. Write the name and chemical formula alkali which is used in the alkaline batteries.
119. Write two differences between acid and base.
120. Write two uses of bases.
121. You are in a need of an acidic salt. How can you prepare it?
Long Questions
1. Write a note on acidic and basic salts.
2. Compare the characteristics properties of acids and bases.
3. Define salts. Also write three characteristics properties of salts.
4. Describe the Lewis concept of acids and bases.
5. Describe the methods of preparation of soluble salts.
6. Describe the reactions of dil. H₂SO₄ in the form of chemical equation with FeS and NaHCO₃.
7. Describe two methods for measuring of pH of solution.
8. Describe uses of any four bases.
9. Explain Arrhenius concept of acids and bases. Also describe its limitations.
10. Explain preparation of insoluble salts.
11. Explain the Bronsted-Lowery concept of acids and bases with the help of examples.
12. Find out the pH and pOH of 0.001 M solution of KOH.
13. Give uses of calcium oxide.
14. State precipitation of hydroxides.
"15. What are salts? Explain with examples the following salts.
i. Double salts. ii. Mixed salts
iii. Complex salts"
16. What is auto-ionization of water? How it is used to establish the pH of water?
17. Write a note on normal and acidic salts.
18. Write a short note on indicators.
19. Write down the characteristics of acids.
20. Write down the characteristics of bases.
"21. Write down the uses of following bases;
i. Sodium Hydroxide
ii. Calcium Hydroxide
iii. Magnesium Hydroxide
iv. Aluminium Hydroxide"
22. Write the four chemical properties of acids.
23. Write the general methods of preparation of soluble and insoluble salts.
24. Write the important characteristics properties of salts.
25. Write the uses of acids.