{"id":12766,"date":"2025-09-22T14:09:10","date_gmt":"2025-09-22T13:09:10","guid":{"rendered":"https:\/\/mcqsadda.com\/?p=12766"},"modified":"2025-11-05T06:33:37","modified_gmt":"2025-11-05T06:33:37","slug":"acids-base-and-salts-top-100-mcqs-with-answer-and-explanation","status":"publish","type":"post","link":"https:\/\/mcqsadda.com\/index.php\/2025\/09\/22\/acids-base-and-salts-top-100-mcqs-with-answer-and-explanation\/","title":{"rendered":"Acids, base, and salts Top 100 MCQs With Answer and Explanation"},"content":{"rendered":"\n

1. According to Arrhenius, an acid is a substance that:<\/mark><\/strong>
A) Accepts a proton
B) Donates a proton
C) Increases H\u207a ions in aqueous solution
D) Increases OH\u207b ions in aqueous solution
Answer:<\/strong> C
Explanation:<\/strong> Arrhenius acid increases concentration of H\u207a (or H\u2083O\u207a) ions in water.<\/p>\n\n\n\n

2. According to Arrhenius, a base is a substance that:<\/mark><\/strong>
A) Accepts a proton
B) Increases OH\u207b ions in aqueous solution
C) Donates H\u207a ions
D) Produces CO\u2083\u00b2\u207b ions
Answer:<\/strong> B
Explanation:<\/strong> Arrhenius base increases OH\u207b ions in aqueous solution.<\/p>\n\n\n\n

3. According to Br\u00f8nsted-Lowry, acids:<\/mark><\/strong>
A) Donate protons
B) Accept protons
C) Donate electrons
D) Accept electrons
Answer:<\/strong> A
Explanation:<\/strong> Br\u00f8nsted-Lowry acid is proton donor.<\/p>\n\n\n\n

4. According to Br\u00f8nsted-Lowry, bases:<\/mark><\/strong>
A) Donate protons
B) Accept protons
C) Donate electrons
D) Accept electrons
Answer:<\/strong> B
Explanation:<\/strong> Br\u00f8nsted-Lowry base is proton acceptor.<\/p>\n\n\n\n

5. Lewis acid is:<\/mark><\/strong>
A) Proton donor
B) Electron pair donor
C) Electron pair acceptor
D) Proton acceptor
Answer:<\/strong> C
Explanation:<\/strong> Lewis acid accepts an electron pair.<\/p>\n\n\n\n

6. Lewis base is:<\/mark><\/strong>
A) Electron pair donor
B) Electron pair acceptor
C) Proton donor
D) Proton acceptor
Answer:<\/strong> A
Explanation:<\/strong> Lewis base donates an electron pair.<\/p>\n\n\n\n

7. Strong acids:<\/mark><\/strong>
A) Partially ionize in water
B) Completely ionize in water
C) Are weak electrolytes
D) Do not conduct electricity
Answer:<\/strong> B
Explanation:<\/strong> Strong acids completely dissociate in water \u2192 strong electrolytes.<\/p>\n\n\n\n

8. Weak acids:<\/mark><\/strong>
A) Partially ionize in water
B) Completely ionize
C) Are strong electrolytes
D) React with water only
Answer:<\/strong> A
Explanation:<\/strong> Weak acids partially dissociate \u2192 weak electrolytes.<\/p>\n\n\n\n

9. Which of the following is a strong acid?<\/mark><\/strong>
A) HCl
B) CH\u2083COOH
C) H\u2082CO\u2083
D) HF
Answer:<\/strong> A
Explanation:<\/strong> HCl completely ionizes in water \u2192 strong acid.<\/p>\n\n\n\n

10. Which of the following is a weak acid?<\/mark><\/strong>
A) HNO\u2083
B) H\u2082SO\u2084
C) CH\u2083COOH
D) HCl
Answer:<\/strong> C
Explanation:<\/strong> Acetic acid is partially ionized \u2192 weak acid.<\/p>\n\n\n\n

11. Strong bases:<\/mark><\/strong>
A) Partially ionize
B) Completely ionize
C) Weak electrolytes
D) Neutral
Answer:<\/strong> B
Explanation:<\/strong> Strong bases like NaOH, KOH completely ionize in water.<\/p>\n\n\n\n

12. Weak bases:<\/mark><\/strong>
A) Partially ionize
B) Completely ionize
C) Strong electrolytes
D) Neutral
Answer:<\/strong> A
Explanation:<\/strong> Weak bases like NH\u2083 partially accept protons in water.<\/p>\n\n\n\n

13. Amphoteric substances:<\/mark><\/strong>
A) Act as acids only
B) Act as bases only
C) Act as both acids and bases
D) Neutral
Answer:<\/strong> C
Explanation:<\/strong> Example: H\u2082O, Al(OH)\u2083, ZnO can act as acid or base.<\/p>\n\n\n\n

14. Example of amphoteric oxide:<\/mark><\/strong>
A) Na\u2082O
B) ZnO
C) CO\u2082
D) SO\u2083
Answer:<\/strong> B
Explanation:<\/strong> ZnO reacts with acids and bases \u2192 amphoteric.<\/p>\n\n\n\n

15. Example of amphoteric hydroxide:<\/mark><\/strong>
A) NaOH
B) Al(OH)\u2083
C) KOH
D) Ca(OH)\u2082
Answer:<\/strong> B
Explanation:<\/strong> Al(OH)\u2083 reacts with HCl (acid) and NaOH (base).<\/p>\n\n\n\n

16. pH of neutral solution at 25\u00b0C is:<\/mark><\/strong>
A) 0
B) 7
C) 14
D) 1
Answer:<\/strong> B
Explanation:<\/strong> Neutral solution [H\u207a] = [OH\u207b] \u2192 pH = 7.<\/p>\n\n\n\n

17. pH of strong acid (0.01 M HCl) is:<\/mark><\/strong>
A) 2
B) 12
C) 7
D) 1
Answer:<\/strong> A
Explanation:<\/strong> pH = -log[H\u207a] = -log(0.01) = 2.<\/p>\n\n\n\n

18. pOH of neutral solution:<\/mark><\/strong>
A) 7
B) 0
C) 14
D) 1
Answer:<\/strong> A
Explanation:<\/strong> pH + pOH = 14 \u2192 for neutral, pOH = 7.<\/p>\n\n\n\n

19. Salt formed from strong acid and strong base is:<\/mark><\/strong>
A) Neutral
B) Acidic
C) Basic
D) Amphoteric
Answer:<\/strong> A
Explanation:<\/strong> Example: NaCl (HCl + NaOH) \u2192 neutral.<\/p>\n\n\n\n

20. Salt formed from strong acid and weak base is:<\/mark><\/strong>
A) Neutral
B) Acidic
C) Basic
D) Amphoteric
Answer:<\/strong> B
Explanation:<\/strong> Example: NH\u2084Cl \u2192 acidic solution.<\/p>\n\n\n\n

21. Salt formed from weak acid and strong base is:<\/mark><\/strong>
A) Neutral
B) Acidic
C) Basic
D) Amphoteric
Answer:<\/strong> C
Explanation:<\/strong> Example: Na\u2082CO\u2083 \u2192 basic solution.<\/p>\n\n\n\n

22. Salt formed from weak acid and weak base is:<\/mark><\/strong>
A) Neutral
B) Acidic or basic depending on K\u2090 and K_b
C) Strongly acidic
D) Strongly basic
Answer:<\/strong> B
Explanation:<\/strong> pH depends on relative strengths of acid and base.<\/p>\n\n\n\n

23. Hydrolysis of Na\u2082CO\u2083 makes solution:<\/mark><\/strong>
A) Neutral
B) Acidic
C) Basic
D) Amphoteric
Answer:<\/strong> C
Explanation:<\/strong> CO\u2083\u00b2\u207b reacts with water \u2192 OH\u207b \u2192 basic solution.<\/p>\n\n\n\n

24. Hydrolysis of NH\u2084Cl makes solution:<\/mark><\/strong>
A) Neutral
B) Acidic
C) Basic
D) Amphoteric
Answer:<\/strong> B
Explanation:<\/strong> NH\u2084\u207a reacts with water \u2192 H\u207a \u2192 acidic solution.<\/p>\n\n\n\n

25. Universal indicator shows strong acid as:<\/mark><\/strong>
A) Red
B) Blue
C) Green
D) Violet
Answer:<\/strong> A
Explanation:<\/strong> Red color indicates strong acid (pH 0\u20133).<\/p>\n\n\n\n

26. Strong acids have:<\/strong><\/mark>
A) Small Ka
B) Large Ka
C) Small Kb
D) No dissociation
Answer:<\/strong> B
Explanation:<\/strong> Strong acids completely ionize \u2192 large acid dissociation constant (Ka).<\/p>\n\n\n\n

27. Weak acids have:<\/mark><\/strong>
A) Small Ka
B) Large Ka
C) Small Kb
D) Large Kb
Answer:<\/strong> A
Explanation:<\/strong> Weak acids partially ionize \u2192 small Ka.<\/p>\n\n\n\n

28. Strong bases have:<\/mark><\/strong>
A) Small Kb
B) Large Kb
C) Small Ka
D) Large Ka
Answer:<\/strong> B
Explanation:<\/strong> Strong bases completely ionize \u2192 large base dissociation constant (Kb).<\/p>\n\n\n\n

29. Weak bases have:<\/mark><\/strong>
A) Small Kb
B) Large Kb
C) Small Ka
D) Large Ka
Answer:<\/strong> A
Explanation:<\/strong> Weak bases partially ionize \u2192 small Kb.<\/p>\n\n\n\n

30. Indicator for strong acid vs strong base titration:<\/mark><\/strong>
A) Methyl orange
B) Phenolphthalein
C) Both A & B
D) Litmus
Answer:<\/strong> C
Explanation:<\/strong> Both can be used; phenolphthalein preferred for sharp endpoint.<\/p>\n\n\n\n

31. Indicator for strong acid vs weak base titration:<\/mark><\/strong>
A) Methyl orange
B) Phenolphthalein
C) Litmus
D) Bromothymol blue
Answer:<\/strong> A
Explanation:<\/strong> Methyl orange changes color at acidic endpoint (pH \u2248 3.1\u20134.4).<\/p>\n\n\n\n

32. Indicator for weak acid vs strong base titration:<\/mark><\/strong>
A) Methyl orange
B) Phenolphthalein
C) Bromothymol blue
D) Litmus
Answer:<\/strong> B
Explanation:<\/strong> Endpoint is basic \u2192 phenolphthalein changes color at pH 8.2\u201310.0.<\/p>\n\n\n\n

33. Buffer solution resists change in:<\/mark><\/strong>
A) pH on adding acid
B) pH on adding base
C) Both A & B
D) Neither
Answer:<\/strong> C
Explanation:<\/strong> Buffers contain weak acid + conjugate base or weak base + conjugate acid \u2192 resist pH changes.<\/p>\n\n\n\n

34. Example of acidic buffer:<\/mark><\/strong>
A) CH\u2083COOH + CH\u2083COONa
B) NH\u2084OH + NH\u2084Cl
C) NaOH + NaCl
D) HCl + NaCl
Answer:<\/strong> A
Explanation:<\/strong> Weak acid + its salt \u2192 acidic buffer solution.<\/p>\n\n\n\n

35. Example of basic buffer:<\/mark><\/strong>
A) NH\u2084OH + NH\u2084Cl
B) CH\u2083COOH + CH\u2083COONa
C) NaOH + NaCl
D) HCl + NaCl
Answer:<\/strong> A
Explanation:<\/strong> Weak base + its salt \u2192 basic buffer solution.<\/p>\n\n\n\n

36. pH of acidic buffer is:<\/mark><\/strong>
A) < 7
B) 7
C) > 7
D) 14
Answer:<\/strong> A
Explanation:<\/strong> Acidic buffer has pH < 7 due to weak acid presence.<\/p>\n\n\n\n

37. pH of basic buffer is:<\/mark><\/strong>
A) < 7
B) 7
C) > 7
D) 0
Answer:<\/strong> C
Explanation:<\/strong> Basic buffer has pH > 7 due to weak base presence.<\/p>\n\n\n\n

38. pH of a buffer depends on:<\/mark><\/strong>
A) Ratio of conjugate base to acid
B) Concentration of salt only
C) Temperature only
D) Indicator used
Answer:<\/strong> A
Explanation:<\/strong> Henderson-Hasselbalch equation: pH = pKa + log([A\u207b]\/[HA]).<\/p>\n\n\n\n

39. Neutralization reaction is:<\/mark><\/strong>
A) Acid + acid \u2192 salt + water
B) Base + base \u2192 salt + water
C) Acid + base \u2192 salt + water
D) Salt + water \u2192 acid + base
Answer:<\/strong> C
Explanation:<\/strong> Neutralization: H\u207a from acid + OH\u207b from base \u2192 H\u2082O + salt.<\/p>\n\n\n\n

40. Product of HCl + NaOH reaction:<\/mark><\/strong>
A) NaCl + H\u2082O
B) NaOH + H\u2082O
C) NaCl only
D) H\u2082O only
Answer:<\/strong> A
Explanation:<\/strong> Strong acid + strong base \u2192 neutral salt (NaCl) + water.<\/p>\n\n\n\n

41. Product of CH\u2083COOH + NaOH reaction:<\/mark><\/strong>
A) CH\u2083COONa + H\u2082O
B) NaOH + H\u2082O
C) CH\u2083COOH + NaOH
D) H\u2082O only
Answer:<\/strong> A
Explanation:<\/strong> Weak acid + strong base \u2192 basic salt (CH\u2083COONa) + water.<\/p>\n\n\n\n

42. Salt from strong acid + weak base is:<\/mark><\/strong>
A) Acidic
B) Neutral
C) Basic
D) Amphoteric
Answer:<\/strong> A
Explanation:<\/strong> Example: NH\u2084Cl \u2192 acidic solution.<\/p>\n\n\n\n

43. Salt from weak acid + strong base is:<\/mark><\/strong>
A) Acidic
B) Neutral
C) Basic
D) Amphoteric
Answer:<\/strong> C
Explanation:<\/strong> Example: Na\u2082CO\u2083 \u2192 basic solution.<\/p>\n\n\n\n

44. Hydrolysis of salts is:<\/mark><\/strong>
A) Reaction with water to form acid\/base
B) Reaction with acid only
C) Reaction with base only
D) None
Answer:<\/strong> A
Explanation:<\/strong> Salt ions react with water \u2192 solution becomes acidic\/basic\/neutral.<\/p>\n\n\n\n

45. Indicator changes color at:<\/mark><\/strong>
A) Specific pH range
B) Any pH
C) Only neutral pH
D) Only strong acids
Answer:<\/strong> A
Explanation:<\/strong> Indicators are weak acids\/bases \u2192 color depends on pH.<\/p>\n\n\n\n

46. Methyl orange changes from red to yellow over pH:<\/mark><\/strong>
A) 3.1\u20134.4
B) 8.2\u201310.0
C) 6.0\u20137.6
D) 0\u20132
Answer:<\/strong> A
Explanation:<\/strong> Red in acid, yellow in base \u2192 transition pH 3.1\u20134.4.<\/p>\n\n\n\n

47. Phenolphthalein changes from colorless to pink over pH:<\/mark><\/strong>
A) 3.1\u20134.4
B) 8.2\u201310.0
C) 6.0\u20137.6
D) 0\u20132
Answer:<\/strong> B
Explanation:<\/strong> Colorless in acid, pink in basic solution \u2192 transition pH 8.2\u201310.0.<\/p>\n\n\n\n

48. Universal indicator shows basic solution as:<\/mark><\/strong>
A) Blue to violet
B) Red to orange
C) Green
D) Yellow
Answer:<\/strong> A
Explanation:<\/strong> pH > 7 – blue\/violet color.<\/p>\n\n\n\n

49. Acid-base titration is used to determine:<\/mark><\/strong>
A) Strength of acid\/base
B) Concentration of acid\/base
C) Both A & B
D) None
Answer:<\/strong> B
Explanation:<\/strong> Titration measures unknown concentration using standard solution.<\/p>\n\n\n\n

50. Salt from weak acid + weak base:<\/mark><\/strong>
A) pH depends on relative strengths
B) Always neutral
C) Always acidic
D) Always basic
Answer:<\/strong> A
Explanation:<\/strong> Example: NH\u2084CH\u2083COO \u2192 pH depends on Kb of NH\u2084\u207a and Ka of CH\u2083COOH.<\/p>\n\n\n\n

51. Hydrolysis of a salt refers to:<\/mark><\/strong>
A) Reaction with acid to form salt
B) Reaction with base to form salt
C) Reaction with water producing acidic, basic, or neutral solution
D) Decomposition on heating
Answer:<\/strong> C
Explanation:<\/strong> Salt ions react with water \u2192 may give acidic, basic, or neutral solution.<\/p>\n\n\n\n

52. Salt of strong acid and strong base:<\/mark><\/strong>
A) Undergoes hydrolysis \u2192 acidic
B) Undergoes hydrolysis \u2192 basic
C) Does not hydrolyze \u2192 neutral solution
D) Amphoteric
Answer:<\/strong> C
Explanation:<\/strong> Example: NaCl \u2192 neutral solution, no hydrolysis.<\/p>\n\n\n\n

53. Salt of strong acid and weak base:<\/mark><\/strong>
A) Acidic solution
B) Basic solution
C) Neutral
D) Amphoteric
Answer:<\/strong> A
Explanation:<\/strong> Example: NH\u2084Cl \u2192 NH\u2084\u207a hydrolyzes \u2192 H\u207a \u2192 acidic.<\/p>\n\n\n\n

54. Salt of weak acid and strong base:<\/mark><\/strong>
A) Acidic solution
B) Basic solution
C) Neutral
D) Amphoteric
Answer:<\/strong> B
Explanation:<\/strong> Example: Na\u2082CO\u2083 \u2192 CO\u2083\u00b2\u207b hydrolyzes \u2192 OH\u207b \u2192 basic.<\/p>\n\n\n\n

55. Salt of weak acid and weak base:<\/mark><\/strong>
A) Neutral
B) Acidic or basic depending on Ka and Kb
C) Always acidic
D) Always basic
Answer:<\/strong> B
Explanation:<\/strong> Example: NH\u2084CH\u2083COO \u2192 pH depends on Kb(NH\u2084\u207a) and Ka(CH\u2083COOH).<\/p>\n\n\n\n

56. Common ion effect:<\/mark><\/strong>
A) Suppression of ionization by presence of common ion
B) Enhancement of ionization
C) No effect
D) Only for acids
Answer:<\/strong> A
Explanation:<\/strong> Presence of common ion shifts equilibrium \u2192 reduces ionization.<\/p>\n\n\n\n

57. Common ion effect decreases:<\/mark><\/strong>
A) Solubility of salts
B) Ionization of acids\/bases
C) Both A & B
D) None
Answer:<\/strong> C
Explanation:<\/strong> Both solubility and ionization suppressed in presence of common ions.<\/p>\n\n\n\n

58. Solubility product (Ksp) represents:<\/mark><\/strong>
A) Concentration of solute in solution
B) Product of ionic concentrations at saturation
C) pH of solution
D) None
Answer:<\/strong> B
Explanation:<\/strong> Ksp = [M\u207f\u207a]^m \u00d7 [X^m\u207b]^n for salt MmXn at saturation.<\/p>\n\n\n\n

59. Precipitation occurs when:<\/mark><\/strong>
A) Ionic product > Ksp
B) Ionic product < Ksp
C) Ionic product = Ksp
D) Solution is neutral
Answer:<\/strong> A
Explanation:<\/strong> When ionic product exceeds solubility product \u2192 excess ions form precipitate.<\/p>\n\n\n\n

60. Example of precipitation reaction:<\/mark><\/strong>
A) AgNO\u2083 + NaCl \u2192 AgCl + NaNO\u2083
B) HCl + NaOH \u2192 NaCl + H\u2082O
C) Na\u2082CO\u2083 + HCl \u2192 NaCl + CO\u2082 + H\u2082O
D) BaCl\u2082 + H\u2082O \u2192 Ba\u00b2\u207a + 2Cl\u207b
Answer:<\/strong> A
Explanation:<\/strong> AgCl precipitates \u2192 insoluble in water.<\/p>\n\n\n\n

61. Salt formed from strong acid and strong base:<\/mark><\/strong>
A) NaCl
B) NH\u2084Cl
C) Na\u2082CO\u2083
D) NH\u2084CH\u2083COO
Answer:<\/strong> A
Explanation:<\/strong> HCl + NaOH \u2192 NaCl (neutral).<\/p>\n\n\n\n

62. Salt formed from strong acid and weak base:<\/mark><\/strong>
A) NH\u2084Cl
B) NaCl
C) Na\u2082CO\u2083
D) K\u2082SO\u2084
Answer:<\/strong> A
Explanation:<\/strong> NH\u2084\u207a hydrolyzes \u2192 acidic solution.<\/p>\n\n\n\n

63. Salt formed from weak acid and strong base:<\/mark><\/strong>
A) Na\u2082CO\u2083
B) NaCl
C) NH\u2084Cl
D) KCl
Answer:<\/strong> A
Explanation:<\/strong> CO\u2083\u00b2\u207b hydrolyzes \u2192 basic solution.<\/p>\n\n\n\n

64. Salt formed from weak acid and weak base:<\/mark><\/strong>
A) NH\u2084CH\u2083COO
B) NaCl
C) KCl
D) Na\u2082SO\u2084
Answer:<\/strong> A
Explanation:<\/strong> pH depends on relative strengths of acid & base.<\/p>\n\n\n\n

65. Solubility of CaSO\u2084 in water is low because:<\/mark><\/strong>
A) Ksp is small
B) Ksp is large
C) Ionic product is high
D) pH is neutral
Answer:<\/strong> A
Explanation:<\/strong> Low Ksp \u2192 low solubility.<\/p>\n\n\n\n

66. Solubility of AgCl decreases in NaCl solution due to:<\/mark><\/strong>
A) Common ion effect
B) Increased temperature
C) Hydrolysis
D) Neutralization
Answer:<\/strong> A
Explanation:<\/strong> Cl\u207b ions from NaCl reduce AgCl solubility.<\/p>\n\n\n\n

67. NaHCO\u2083 reacts with HCl to form:<\/mark><\/strong>
A) NaCl + CO\u2082 + H\u2082O
B) NaOH + CO\u2082
C) NaCl + H\u2082O
D) Na\u2082CO\u2083 + H\u2082O
Answer:<\/strong> A
Explanation:<\/strong> Acid reacts with bicarbonate \u2192 salt + CO\u2082 + water.<\/p>\n\n\n\n

68. Na\u2082CO\u2083 reacts with HCl to form:<\/mark><\/strong>
A) NaCl + CO\u2082 + H\u2082O
B) NaOH + CO\u2082
C) NaCl only
D) NaHCO\u2083
Answer:<\/strong> A
Explanation:<\/strong> Carbonate reacts with acid \u2192 produces CO\u2082, water, and salt.<\/p>\n\n\n\n

69. Na\u2082CO\u2083 reacts with Ca(OH)\u2082 to form:<\/mark><\/strong>
A) CaCO\u2083 + 2NaOH
B) NaOH + H\u2082O
C) Na\u2082CaO\u2082
D) CaCl\u2082
Answer:<\/strong> A
Explanation:<\/strong> Double displacement \u2192 precipitate CaCO\u2083 + NaOH in solution.<\/p>\n\n\n\n

70. Reaction of NaOH with NH\u2084Cl produces:<\/mark><\/strong>
A) NH\u2083 + H\u2082O + NaCl
B) NH\u2084OH only
C) NaNH\u2082
D) NH\u2084NO\u2083
Answer:<\/strong> A
Explanation:<\/strong> Strong base liberates NH\u2083 from ammonium salt.<\/p>\n\n\n\n

71. Reaction of Na\u2082CO\u2083 with H\u2082O produces:<\/mark><\/strong>
A) Basic solution (Na\u207a + CO\u2083\u00b2\u207b + H\u2082O \u2192 OH\u207b)
B) Acidic solution
C) Neutral solution
D) None
Answer:<\/strong> A
Explanation:<\/strong> CO\u2083\u00b2\u207b hydrolyzes \u2192 OH\u207b \u2192 basic solution.<\/p>\n\n\n\n

72. Applications of salts:<\/mark><\/strong>
A) Fertilizers
B) Medicines
C) Food preservatives
D) All of these
Answer:<\/strong> D
Explanation:<\/strong> Salts have diverse applications in industry, medicine, and food.<\/p>\n\n\n\n

73. Baking soda (NaHCO\u2083) is used:<\/mark><\/strong>
A) As antacid
B) In baking
C) Both
D) None
Answer:<\/strong> C
Explanation:<\/strong> Neutralizes acid (antacid) and releases CO\u2082 in baking.<\/p>\n\n\n\n

74. Washing soda (Na\u2082CO\u2083\u00b710H\u2082O) is used:<\/mark><\/strong>
A) In soap and detergent
B) In baking
C) As antacid
D) Fertilizer
Answer:<\/strong> A
Explanation:<\/strong> Reacts with Ca\u00b2\u207a\/Mg\u00b2\u207a ions in water \u2192 softens water.<\/p>\n\n\n\n

75. Common salt (NaCl) is used:
<\/mark><\/strong>A) Food seasoning
B) Chemical industry
C) Both
D) None
Answer:<\/strong> C
Explanation:<\/strong> NaCl is essential for food and industrial chemical processes.<\/p>\n\n\n\n

76. Bromothymol blue changes color in pH range:<\/mark><\/strong>
A) 6.0\u20137.6
B) 3.1\u20134.4
C) 8.2\u201310.0
D) 0\u20132
Answer:<\/strong> A
Explanation:<\/strong> Yellow in acid, green at neutral, blue in basic solution.<\/p>\n\n\n\n

77. Neutralization point in strong acid\u2013strong base titration occurs at:<\/mark><\/strong>
A) pH < 7
B) pH = 7
C) pH > 7
D) pH = 14
Answer:<\/strong> B
Explanation:<\/strong> Strong acid + strong base \u2192 neutral solution at equivalence.<\/p>\n\n\n\n

78. Neutralization point in strong acid\u2013weak base titration occurs at:<\/mark><\/strong>
A) pH < 7
B) pH = 7
C) pH > 7
D) pH = 14
Answer:<\/strong> A
Explanation:<\/strong> Salt formed (e.g., NH\u2084Cl) is acidic \u2192 pH < 7.<\/p>\n\n\n\n

79. Neutralization point in weak acid\u2013strong base titration occurs at:<\/mark><\/strong>
A) pH < 7
B) pH = 7
C) pH > 7
D) pH = 0
Answer:<\/strong> C
Explanation:<\/strong> Salt formed (e.g., Na\u2082CO\u2083) is basic \u2192 pH > 7.<\/p>\n\n\n\n

80. Indicator choice depends on:<\/mark><\/strong>
A) Type of acid & base
B) Equivalence point pH
C) Both A & B
D) Color of solution
Answer:<\/strong> C
Explanation:<\/strong> Indicator must change color at pH near equivalence point.<\/p>\n\n\n\n

81. Phenolphthalein is colorless in:<\/mark><\/strong>
A) Acidic solution
B) Neutral solution
C) Basic solution
D) All
Answer:<\/strong> A
Explanation:<\/strong> Phenolphthalein turns pink in basic solution; colorless in acid.<\/p>\n\n\n\n

82. Methyl orange is red in:<\/mark><\/strong>
A) Acid
B) Base
C) Neutral
D) Both A & B
Answer:<\/strong> A
Explanation:<\/strong> Red in acidic medium, yellow in basic medium.<\/p>\n\n\n\n

83. Universal indicator shows pH 7 as:<\/mark><\/strong>
A) Red
B) Green
C) Blue
D) Violet
Answer:<\/strong> B
Explanation:<\/strong> Green indicates neutral pH.<\/p>\n\n\n\n

84. Acid rain is caused by:<\/mark><\/strong>
A) SO\u2082 and NO\u2082 dissolution in rainwater
B) CO\u2082 dissolution only
C) O\u2082 only
D) N\u2082 only
Answer:<\/strong> A
Explanation:<\/strong> SO\u2082 and NO\u2082 form H\u2082SO\u2084 and HNO\u2083 \u2192 acid rain.<\/p>\n\n\n\n

85. Effect of acid rain on soil:<\/mark><\/strong>
A) Reduces fertility
B) Increases pH
C) No effect
D) Makes soil basic
Answer:<\/strong> A
Explanation:<\/strong> Acid rain leaches nutrients \u2192 soil fertility decreases.<\/p>\n\n\n\n

86. Buffer solution in blood:<\/mark><\/strong>
A) H\u2082CO\u2083 \/ HCO\u2083\u207b
B) NH\u2084\u207a \/ NH\u2083
C) CH\u2083COOH \/ CH\u2083COONa
D) NaCl \/ HCl
Answer:<\/strong> A
Explanation:<\/strong> Carbonic acid-bicarbonate buffer maintains blood pH \u2248 7.4.<\/p>\n\n\n\n

87. Blood pH lower than 7.35 causes:<\/mark><\/strong>
A) Alkalosis
B) Acidosis
C) Neutral
D) None
Answer:<\/strong> B
Explanation:<\/strong> Acidic blood \u2192 acidosis.<\/p>\n\n\n\n

88. Blood pH higher than 7.45 causes:<\/mark><\/strong>
A) Acidosis
B) Alkalosis
C) Neutral
D) None
Answer:<\/strong> B
Explanation:<\/strong> Alkalosis occurs \u2192 blood too basic.<\/p>\n\n\n\n

89. OH\u207b concentration of neutral solution at 25\u00b0C:<\/mark><\/strong>
A) 1 \u00d7 10\u207b\u2077 M
B) 1 \u00d7 10\u207b\u00b9\u2074 M
C) 1 \u00d7 10\u207b\u2074 M
D) 1 \u00d7 10\u207b\u00b9 M
Answer:<\/strong> A
Explanation:<\/strong> For neutral solution, [H\u207a] = [OH\u207b] = 10\u207b\u2077 M.<\/p>\n\n\n\n

90. H\u207a concentration of neutral solution at 25\u00b0C:<\/mark><\/strong>
A) 1 \u00d7 10\u207b\u2077 M
B) 1 \u00d7 10\u207b\u00b9\u2074 M
C) 1 \u00d7 10\u207b\u2074 M
D) 1 \u00d7 10\u207b\u00b9 M
Answer:<\/strong> A
Explanation:<\/strong> Neutral solution: [H\u207a] = 10\u207b\u2077 M.<\/p>\n\n\n\n

91. Indicators are:<\/mark><\/strong>
A) Weak acids or weak bases
B) Strong acids
C) Strong bases
D) Salts
Answer:<\/strong> A
Explanation:<\/strong> They change color depending on pH.<\/p>\n\n\n\n

92. Acid-base theories used in chemistry:<\/mark><\/strong>
A) Arrhenius
B) Br\u00f8nsted-Lowry
C) Lewis
D) All of these
Answer:<\/strong> D
Explanation:<\/strong> All three theories describe acids and bases differently.<\/p>\n\n\n\n

93. Industrial application of acid:<\/mark><\/strong>
A) H\u2082SO\u2084 in fertilizer production
B) HCl in metal cleaning
C) Both A & B
D) None
Answer:<\/strong> C
Explanation:<\/strong> Strong acids are widely used in industry.<\/p>\n\n\n\n

94. Industrial application of base:<\/mark><\/strong>
A) NaOH in soap manufacturing
B) Ca(OH)\u2082 in water treatment
C) Both A & B
D) None
Answer:<\/strong> C
Explanation:<\/strong> Bases are used for cleaning, soap making, water softening.<\/p>\n\n\n\n

95. Lime (CaO) is used in:<\/mark><\/strong>
A) Water treatment
B) Cement production
C) Both
D) None
Answer:<\/strong> C
Explanation:<\/strong> Lime neutralizes acidic water and is used in cement.<\/p>\n\n\n\n

96. Na\u2082CO\u2083 is used in:<\/mark><\/strong>
A) Glass making
B) Water softening
C) Soap production
D) All of these
Answer:<\/strong> D
Explanation:<\/strong> Sodium carbonate has multiple industrial uses.<\/p>\n\n\n\n

97. Alkalinity of water is due to:<\/mark><\/strong>
A) Carbonates and bicarbonates
B) Chlorides
C) Sulfates
D) Nitrates
Answer:<\/strong> A
Explanation:<\/strong> CO\u2083\u00b2\u207b and HCO\u2083\u207b neutralize acids \u2192 alkaline water.<\/p>\n\n\n\n

98. Acidity of water is due to:<\/mark><\/strong>
A) Dissolved CO\u2082 \u2192 H\u2082CO\u2083
B) NaOH
C) CaCO\u2083
D) KCl
Answer:<\/strong> A
Explanation:<\/strong> CO\u2082 forms carbonic acid \u2192 makes water slightly acidic.<\/p>\n\n\n\n

99. Common indicator for titrating strong acid vs weak base:<\/mark><\/strong>
A) Methyl orange
B) Phenolphthalein
C) Litmus
D) Bromothymol blue
Answer:<\/strong> A
Explanation:<\/strong> Endpoint acidic \u2192 methyl orange changes color at low pH.<\/p>\n\n\n\n

100. Common indicator for titrating weak acid vs strong base:<\/mark><\/strong>
A) Methyl orange
B) Phenolphthalein
C) Bromothymol blue
D) Litmus
Answer:<\/strong> B
Explanation:<\/strong> Endpoint basic \u2192 phenolphthalein changes color in basic pH.<\/p>\n","protected":false},"excerpt":{"rendered":"

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