Acid-Base Titrations: Master the Art of Neutralization

Question 1

What is the primary function of an acid-base indicator in a titration?

Accepted Answer

To change color near the equivalence point

Answer

To neutralize the solution

Answer

To speed up the reaction

Answer

To determine the initial concentration of the unknown solution

Question 2

Which of the following is considered a strong acid?

Accepted Answer

Hydrochloric acid

Answer

Acetic acid

Answer

Ammonia

Answer

Sodium hydroxide

Question 3

What is the pH value of a neutral solution at 25°C?

Accepted Answer

7

Answer

0

Answer

14

Answer

It depends on the temperature

Question 4

Which of the following titration curves represents a strong acid-strong base titration?

Accepted Answer

A sharp curve with a near-vertical equivalence point

Answer

A gradual curve with a less steep slope

Answer

A curve with two equivalence points

Answer

A curve that is linear throughout

Question 5

What is the molarity of a solution that contains 0.2 moles of solute dissolved in 500 mL of solution?

Accepted Answer

0.2 M

Answer

0.04 M

Answer

0.4 M

Answer

2 M

Question 6

What is the purpose of performing a blank titration in acid-base titrations?

Accepted Answer

To account for the volume of titrant used to fill the buret and reaction vessel

Answer

To determine the initial concentration of the unknown solution

Answer

To calibrate the buret

Answer

To ensure the purity of the reagents

Question 7

Which titration method is best suited for determining the concentration of a weak acid?

Accepted Answer

Back titration

Answer

Direct titration

Answer

Differential titration

Answer

Conductometric titration

Question 8

Explain the key differences between strong and weak acids, providing specific examples for each type.

Accepted Answer

Strong acids dissociate completely in water, releasing all their H+ ions, while weak acids dissociate only partially, releasing only a fraction of their H+ ions.

Answer

Strong acids are more corrosive than weak acids.

Answer

Strong acids have a lower pH than weak acids.

Answer

Weak acids can be either organic or inorganic, while strong acids are typically inorganic.

Question 9

In a titration curve, the steepest part of the curve occurs at:

Accepted Answer

The equivalence point

Answer

The beginning of the titration

Answer

The end point

Answer

Halfway through the titration

Question 10

What is the role of a base like sodium hydroxide in a titration involving a strong acid?

Accepted Answer

To neutralize the acid

Answer

To act as an indicator

Answer

To speed up the reaction

Answer

To lower the pH of the solution

Question 11

Which of the following can NOT be used as a solvent in a titration?

Accepted Answer

Hydrochloric acid

Answer

Water

Answer

Alcohol

Answer

Acetonitrile

Question 12

What is the primary purpose of a buret in a titration?

Accepted Answer

To measure the volume of the titrant

Answer

To hold the analyte

Answer

To mix the titrant and analyte

Answer

To indicate the endpoint of the titration

Question 13

What is the KHP abbreviation commonly used in titration?

Accepted Answer

Potassium hydrogen phthalate

Answer

Potassium hydroxide solution

Answer

Potassium hexachloroplatinate

Answer

Potassium hydrogen permanganate

Question 14

In acid-base titrations, what is an advantage of using electronic pH meters over traditional acid-base indicators?

Accepted Answer

Electronic pH meters provide more precise and accurate pH measurements.

Answer

Traditional acid-base indicators are more versatile than electronic pH meters.

Answer

Electronic pH meters are generally less expensive than traditional acid-base indicators.

Answer

Traditional acid-base indicators are easier to use than electronic pH meters.

Question 15

How do buffers influence the accuracy and precision of acid-base titrations?

Accepted Answer

Buffers stabilize the pH, minimizing errors from over- or under-titration.

Answer

Buffers accelerate the titration reaction, enabling quicker endpoint identification.

Answer

Buffers hinder the titration endpoint, decreasing accuracy.

Question 16

What is the primary objective of an acid-base titration?

Accepted Answer

To precisely determine the concentration of an unknown acid or base in a solution

Answer

To neutralize a known volume of acid with a known volume of base

Answer

To ascertain the acidity or basicity of a solution

Answer

To measure the volume of gas produced in a chemical reaction

Question 17

In an acid-base titration, what is the equivalence point?

Accepted Answer

The exact point where the moles of acid and base are equal

Answer

The point where the pH of the solution is perfectly neutral (pH 7)

Answer

The point where the buret reading is zero

Answer

The point where the reaction between the acid and base is complete

Question 18

In an acid-base titration, how does the initial concentration of the acid affect the volume of base required to reach the equivalence point?

Accepted Answer

Directly proportional

Answer

Inversely proportional

Answer

Logarithmically related

Answer

No relationship

Question 19

What is the primary function of a standard solution in an acid-base titration?

Accepted Answer

To provide a precisely known concentration of acid or base

Answer

To neutralize the unknown solution

Answer

To serve as an indicator

Answer

To calibrate the buret

Question 20

Which of the following is classified as a weak acid?

Accepted Answer

Acetic acid

Answer

Hydrochloric acid

Answer

Nitric acid

Answer

Sulfuric acid

Question 21

In a titration experiment, 25.0 mL of an unknown acid solution is neutralized by 18.7 mL of a 0.100 M NaOH solution. What is the concentration of the unknown acid solution?

Accepted Answer

0.0748 M

Answer

0.1496 M

Answer

0.2992 M

Answer

0.5984 M

Question 22

Which of the following is a strong acid?

Accepted Answer

Hydrochloric acid

Answer

Acetic acid

Answer

Carbonic acid

Answer

Ammonia

Question 23

What is the purpose of using a buret in a titration?

Accepted Answer

To measure the volume of the acid solution accurately, allowing for precise determination of the equivalence point.

Answer

To mix the acid and base solutions, ensuring proper reaction.

Answer

To indicate the endpoint of the titration, as the color change is easily observed.

Answer

To add the base solution to the acid solution dropwise, providing control over the reaction rate.

Question 24

Which of the following is a common application of acid-base titrations?

Accepted Answer

All of the above, as acid-base titrations have diverse practical applications.

Answer

Determining the unknown concentration of an acid or base through neutralization reactions.

Answer

Measuring the acidity or alkalinity of various substances, such as soil or water.

Answer

Analyzing the purity and composition of food and beverages, ensuring quality control.

Question 25

What is the role of a standard solution in a titration?

Accepted Answer

It is the solution with a precisely known concentration, used for accurate determination of the unknown.

Answer

It is the solution being analyzed, and its concentration is determined through titration.

Answer

It is used to calibrate the buret, ensuring accurate volume measurement.

Answer

It is used to neutralize the solution at the endpoint, indicating the completion of the reaction.

Question 26

What is the difference between a monoprotic acid and a diprotic acid?

Accepted Answer

A monoprotic acid donates one proton per molecule, while a diprotic acid donates two protons per molecule.

Answer

A monoprotic acid has a lower pH than a diprotic acid, indicating greater acidity.

Answer

A monoprotic acid is typically stronger than a diprotic acid, meaning it dissociates more readily.

Answer

There is no difference between a monoprotic acid and a diprotic acid, as they both release protons in water.

Question 27

What is the K_a value of a weak acid?

Accepted Answer

It is an equilibrium constant that represents the extent to which the acid dissociates in water.

Answer

It is a measure of the strength of the acid, with a lower K_a indicating a stronger acid.

Answer

It is the concentration of the acid at which it is 50% dissociated, indicating the midpoint of the dissociation process.

Answer

It is the pH of the solution when the acid is completely dissociated, indicating a highly acidic environment.

Question 28

What is the primary purpose of using an indicator in a titration?

Accepted Answer

To indicate the endpoint of the titration

Answer

To determine the initial pH of the solution

Answer

To neutralize the solution before titration

Answer

To prevent the reaction from occurring

Question 29

Which of the following is considered a strong acid?

Accepted Answer

Hydrochloric acid

Answer

Acetic acid

Answer

Ammonium hydroxide

Answer

Sodium hydroxide

Question 30

Which of the following is the definition of a buffer solution?

Accepted Answer

A solution containing a weak acid and its conjugate base

Answer

A solution containing a strong acid and its conjugate base

Answer

A solution containing only a strong acid

Answer

A solution containing only a weak base

Question 31

What is the purpose of performing a standardization procedure in acid-base titrations?

Accepted Answer

To determine the exact concentration of a solution

Answer

To calibrate the burette used for titration

Answer

To prepare a buffer solution

Answer

To adjust the pH of the solution

Question 32

What is the primary purpose of an acid-base titration?

Accepted Answer

To precisely determine the concentration of an unknown acid or base in a solution.

Answer

To identify the type of acid or base present in a solution.

Answer

To neutralize a solution for further analysis.

Answer

To prepare a buffer solution with a specific pH.

Question 33

What is the primary function of the buret in a titration setup?

Accepted Answer

To accurately measure and dispense a known volume of the titrant solution.

Answer

To hold the solution being analyzed.

Answer

To mix the titrant and analyte solutions together.

Answer

To detect the endpoint of the titration using an indicator.

Question 34

What is the fundamental difference between a strong acid and a weak acid?

Accepted Answer

Strong acids completely dissociate in water, releasing all their hydrogen ions (H+). Weak acids only partially dissociate, releasing fewer H+ ions.

Answer

Weak acids have a higher pH than strong acids, indicating a lower acidity level.

Answer

Strong acids are more corrosive than weak acids due to their higher concentration of H+ ions.

Answer

Weak acids react more slowly than strong acids in chemical reactions.

Question 35

What is the mathematical relationship between pH and pOH in aqueous solutions?

Accepted Answer

pH + pOH = 14

Answer

pH - pOH = 14

Answer

pH = pOH

Answer

pH + pOH = 0

Question 36

Which of the following reactions correctly represents a neutralization reaction?

Accepted Answer

Acid (H+) + Base (OH-) -> Salt (ionic compound) + Water (H2O)

Answer

Acid (H+) + Metal (M) -> Salt (ionic compound) + Hydrogen gas (H2)

Answer

Base (OH-) + Metal Oxide (MO) -> Salt (ionic compound) + Water (H2O)

Answer

Base (OH-) + Nonmetal Oxide (N2O) -> Salt (ionic compound) + Water (H2O)

Question 37

In an acid-base titration, which indicator would be most suitable for a titration between a strong acid and a strong base?

Accepted Answer

Phenolphthalein: A colorless indicator that turns pink at the equivalence point.

Answer

Methyl orange: A yellow indicator that turns red at the equivalence point.

Answer

Litmus: A purple indicator that turns red in acidic solutions and blue in basic solutions.

Answer

Universal indicator: A multicolored indicator that provides a range of colors depending on the pH.

Question 38

How does temperature impact the accuracy of acid-base titrations? Discuss the factors that contribute to temperature-induced errors.

Accepted Answer

Temperature can alter the reaction's equilibrium constant, potentially leading to errors in determining the equivalence point.

Answer

Temperature has no significant effect on the accuracy of acid-base titrations.

Answer

Higher temperatures always enhance titration accuracy due to increased reaction rates.

Answer

Lower temperatures always reduce titration accuracy due to decreased reactant solubility.

Question 39

What is the primary purpose of using a buret in an acid-base titration?

Accepted Answer

To accurately measure the volume of titrant added

Answer

To determine the concentration of the analyte

Answer

To mix the acid and base solutions

Answer

To indicate the endpoint of the titration

Question 40

Which of the following is a strong acid?

Accepted Answer

Hydrochloric acid

Answer

Carbonic acid

Answer

Acetic acid

Answer

Citric acid

Question 41

What is the molarity of a solution that contains 0.1 moles of NaOH in 1 liter of solution?

Accepted Answer

0.1 M

Answer

0.2 M

Answer

1 M

Answer

0.5 M

Question 42

Which of the following is a monoprotic acid?

Accepted Answer

Hydrochloric acid

Answer

Carbonic acid

Answer

Sulfuric acid

Answer

Phosphoric acid

Question 43

What is the endpoint of an acid-base titration?

Accepted Answer

The point at which the indicator changes color

Answer

The point at which the moles of acid are equal to the moles of base

Answer

The point at which the pH of the solution is 7

Question 44

Which of the following is a weak base?

Accepted Answer

Ammonia

Answer

Calcium hydroxide

Answer

Potassium hydroxide

Answer

Sodium hydroxide

Question 45

What is the pH of a solution that has a hydrogen ion concentration of 1 x 10^-4 M?

Accepted Answer

4

Answer

3

Answer

6

Answer

5

Question 46

In an acid-base titration, the endpoint is reached when:

Accepted Answer

The moles of acid equal the moles of base

Answer

The solution becomes colorless

Answer

The pH of the solution is exactly 7

Question 47

Which of the following is a strong acid?

Accepted Answer

HCl

Answer

NH3

Answer

CH3COOH

Answer

H2CO3

Question 48

A solution with a [H+] concentration of 1.0 x 10^-4 M has a pH of:

Accepted Answer

4

Answer

7

Answer

10

Answer

14

Question 49

Which of the following reactions is an acid-base neutralization reaction?

Accepted Answer

HCl + NaOH → NaCl + H2O

Answer

2H2 + O2 → 2H2O

Answer

Fe + 2HCl → FeCl2 + H2

Answer

NH3 + H2O → NH4+ + OH-

Question 50

What is the molarity of a solution containing 0.2 moles of solute in 2 liters of solution?

Accepted Answer

0.1 M

Answer

1 M

Answer

2 M

Answer

0.01 M

Question 51

A graph of pH versus volume of titrant added is referred to as a:

Accepted Answer

Titration curve

Answer

Temperature curve

Answer

Concentration curve

Answer

Mass curve

Question 52

The equivalence point in a titration is characterized by:

Accepted Answer

Equal moles of acid and base

Answer

Colorless solution

Answer

pH of 7

Question 53

Which of the following is a weak base?

Accepted Answer

NH3

Answer

NaOH

Answer

H2SO4

Answer

HCl

Question 54

In a titration, the buret is primarily used for:

Accepted Answer

Measuring the volume of titrant added

Answer

Indicating the endpoint of the titration

Answer

Holding the solution being titrated

Answer

Mixing the solutions together