Practice MCQ For Govt Pharmacist Exam, in this article we will solve, Practice MCQ on the topic acid base titrations under the subject Pharmaceutical inorganic chemistry of first semester. Read following article for your reference.
Acid Base Titrations » PHARMACAREERS
Which of the following is true about acid-base indicators?
A) They change color at a specific pH.
B) They are always acidic in nature.
C) They are used as primary standards.
D) They react with water to form salts.
Which of the following is a characteristic of a strong acid?
A) High pH
B) Partial ionization in water
C) Weak electrolyte behavior
D) Low pKa value
What is the primary purpose of an acid-base titration?
A) To determine the concentration of an unknown acid
B) To measure the pH of a solution
C) To study the color changes of indicators
D) To calculate the molar mass of a base
Which type of titration involves the reaction between a strong acid and a strong base?
A) Acid-alkali titration
B) Redox titration
C) Complexometric titration
D) Precipitation titration
The endpoint of an acid-base titration is determined by:
A) The color change of the indicator
B) The initial volume of the titrant
C) The pH of the solution
D) The temperature of the reaction mixture
Which of the following is a secondary standard in acid-base titration?
A) NaOH
B) HCl
C) K2Cr2O7
D) Na2CO3
What is the role of a buffer solution in an acid-base titration?
A) To neutralize excess titrant
B) To enhance the color change of the indicator
C) To maintain a constant pH during the titration
D) To increase the reaction rate
Which of the following is a weak base?
A) NaOH
B) NH3
C) KOH
D) Ca(OH)2
What is the pH of a neutral solution at 25°C?
A) 0
B) 7
C) 14
D) It varies with the concentration of H+ ions
Which acid-base theory defines an acid as a proton donor and a base as a proton acceptor?
A) Arrhenius theory
B) Lewis theory
C) Brønsted-Lowry theory
D) Gilbert-Lewis theory
Which of the following is true about acid-base indicators?
A) They change color at a specific pH.
B) They are always acidic in nature.
C) They are used as primary standards.
D) They react with water to form salts.
Which of the following is a characteristic of a strong acid?
A) High pH
B) Partial ionization in water
C) Weak electrolyte behavior
D) Low pKa value
What is the primary purpose of an acid-base titration?
A) To determine the concentration of an unknown acid
B) To measure the pH of a solution
C) To study the color changes of indicators
D) To calculate the molar mass of a base
Which type of titration involves the reaction between a strong acid and a strong base?
A) Acid-alkali titration
B) Redox titration
C) Complexometric titration
D) Precipitation titration
The endpoint of an acid-base titration is determined by:
A) The color change of the indicator
B) The initial volume of the titrant
C) The pH of the solution
D) The temperature of the reaction mixture
Which of the following is a secondary standard in acid-base titration?
A) NaOH
B) HCl
C) K2Cr2O7
D) Na2CO3
What is the role of a buffer solution in an acid-base titration?
A) To neutralize excess titrant
B) To enhance the color change of the indicator
C) To maintain a constant pH during the titration
D) To increase the reaction rate
Which of the following is a weak base?
A) NaOH
B) NH3
C) KOH
D) Ca(OH)2
What is the pH of a neutral solution at 25°C?
A) 0
B) 7
C) 14
D) It varies with the concentration of H+ ions
Which acid-base theory defines an acid as a proton donor and a base as a proton acceptor?
A) Arrhenius theory
B) Lewis theory
C) Brønsted-Lowry theory
D) Gilbert-Lewis theory
Which of the following combinations cannot produce a buffer solution?
A) HNO2 and NaNO2
B) HCN and NaCN
C) HClO4 and NaClO4
D) NH3 and (NH4)2SO4
E) NH3 and NH4Br
What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NH4Cl?
A) 2.15
B) 4.62
C) 8.26
D) 9.38
E) 8.89
Calculate the ratio [CH3COOH]/[NaCH3COO] that gives a solution with pH = 5.00.
A) 0.28
B) 0.36
C) 0.44
D) 0.56
E) 0.63
Consider a solution which is 0.10 M in CH3COOH and 0.20 M in NaCH3COO. Which of the following statements is true?
A) If a small amount of NaOH is added, the pH decreases very slightly.
B) If NaOH is added, the OH- ions react with the CH3COO- ions.
C) If a small amount of HCl is added, the pH decreases very slightly.
D) If HCl is added, the H+ ions react with CH3COOH ions.
E) If more CH3COOH is added, the pH increases.
A buffer was prepared by mixing 1.00 mole of ammonia and 1.00 mole of ammonium chloride to form an aqueous solution with a total volume of 1.00 liter. To 500 mL of this solution, 30.0 mL of 1.00 M NaOH was added. What is the pH of this solution?
A) 8.96
B) 9.83
C) 9.31
D) 9.11
E) 9.57
How many grams of NaF would have to be added to 2.00 L of 0.100 M HF to yield a solution with a pH = 4.00?
A) 300 g
B) 36 g
C) 0.84 g
D) 6.9 g
E) 60. G
Calculate the pH that results when the following solutions are mixed:
(1) 35 mL of 0.20 M formic acid
(2) 55 mL of 0.10 M sodium formate
(3) 110 mL of water
A) 3.64
B) 3.11
C) 4.58
D) 3.39
E) 4.20
Consider an indicator that ionizes as shown below, with its Ka = 1.0 x 10^-4:
HIn + H2O ⇌ H3O+ + In-
Which of the following statements is true? (Select all that apply.)
(1) The predominant color in its acid range is yellow.
(2) In the middle of the pH range of its color change, a solution containing the indicator will probably be orange.
(3) At pH = 7.00, a solution containing this indicator (and no other colored species) will be red.
(4) At pH = 7.00, most of the indicator is in the un-ionized form.
(5) The pH at which the indicator changes color is pH = 4.
A) 1, 3, 5
B) 2, 4
C) 3, 4, 5
D) 1, 2, 3, 5
E) Another combination
What is the definition of a neutralization reaction?
A) A reaction between an acid and a base that produces a gas
B) A reaction between an acid and a base that forms a precipitate
C) A reaction between an acid and a base that results in the formation of salt and water
D) A reaction between an acid and a base that generates heat
Complete the following reaction: HCl + Mg(OH)2 à
A) MgCl2 + O2
B) MgCl2 + CO2
C) MgCl2 + H2O
D) MgCl2 + CO2 + H2O
What is the pH range of acidic solutions?
A) 0-2
B) 7-14
C) 5-7
D) 0-7
A neutral solution contains:
A) No free ions
B) Salts of metals
C) Electrons and protons
D) Equal numbers of H+ and OH- ions
Neutralization reactions are:
A) Displacement reactions
B) Double displacement reactions
C) Decomposition reactions
D) Combination reactions
Predict the products of the following reaction: HNO3 + KOH à
A) KNO3 + H2O
B) Mg(OH)2 + HClO2
C) NaOH + HF
Calculate the pH of the solution resulting from the addition of 20.0 mL of 0.100 M NaOH to 30.0 mL of 0.100 M HNO3.
A) 1.35
B) 1.70
C) 1.95
D) 2.52
E) 2.80
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