QUESTION Unit-CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS

CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS

1. UNIT-3 TITRIMETRIC ANALYSES
QUESTION A B C D Answer
1.What does a high standard reduction potential
(E°) indicate about a substance?
It is a strong
oxidizing
agent
It is a strong
reducing agent
It is neither an
oxidizing nor
reducing agent.
It is neutral in
redox
reactions.
2.Which of the following species has the highest
tendency to be reduced? E° = -0.76 VE° = +0.34 VE° = +1.23 VE° = 0 V
3.In the Nernst equation, the reduction potential
of an electrochemical cell is dependent on:TemperaturePressure
Concentration of
reactants and
products
All of the
above
4.Which of the following is true about redox
titrations
They only
involve strong
oxidizing
agents.
They involve the
transfer of
protons between
species.
They involve the
transfer of
electrons
between the
titrant and the
analyte.
They do not
depend on the
standard
reduction
potentials of
the species
involved
5.Which of the following indicators is commonly
used in redox titrations?
Phenolphthale
in Methyl orangeStarch
Potassium
dichromate
6.The number of moles of electrons transferred
in a redox reaction is directly related to:
The number
of protons
transferred
The
stoichiometry of
the half-reactions
The molar mass
of the titrant
The
concentration
of the analyte
7.Which of the following is necessary for a redox
titration to be feasible?
The reducing
agent must
have a higher
E° value than
the oxidizing
agent
The oxidizing
agent must have
a higher E° value
than the reducing
agent.
Both agents must
have the same E°
value.
The titration
must take
place in a
neutral
medium.
8.A redox titration is feasible if:
The reaction
has a large
negative ΔG.
The reaction has
a large positive
ΔG.
The reaction is
slow
The products
are more
reactive than
the reactants.
9.Which of the following is an example of a
redox titration?
Titration of
NaOH with
Titration of
KMnO₄ with
Titration of
acetic acid with
Titration of
Na₂CO₃ with

2. UNIT-3 TITRIMETRIC ANALYSES
HCl
Fe²⁺ in acidic
medium
sodium
hydroxide H₂SO₄
10.For a redox titration to have a well-defined
equivalence point, the reaction must:
Have fast
electron
transfer
kinetics
Involve a weak
reducing agent
and strong
oxidizing agent.
Occur at high
temperature.
Be a multi-
step process
11.In a redox titration involving Iodine (I₂) and
Sodium Thiosulfate (Na₂S₂O₃), what is the
primary role of the I₂?
Oxidizing
agent Reducing agentCatalyst Indicator
12.What is the primary purpose of a
complexometric titration?
To measure
pH changes in
acidic
solutions
To determine the
concentration of
metal ions in a
solution
To analyze the
concentration of
acids and bases
To measure
redox
potential in a
reaction
13.What type of reaction occurs in
complexometric titrations?
Acid-base
neutralizationRedox reaction
Formation of a
stable metal-
ligand complex
Precipitation
reaction
14.What is the stepwise formation constant (K₁,
K₂, etc.) in complexometric titrations?
The constant
that describes
the formation
of the entire
complex in
one step
The constant
describing the
formation of
each successive
metal-ligand
bond
The overall
constant
describing ligand
dissociation
The constant
for the
dissociation
of water
molecules
15.A high overall formation constant (β) for a
metal-ligand complex indicates:
A weak
metal-ligand
complex
A strong metal-
ligand complex
The ligand has
been fully
dissociated
The reaction
is
thermodynami
cally unstable
16.Which factor most significantly affects the
value of stepwise formation constants in
complex formation?
The size of
the ligand
The volume of
the solution
The color of the
solution
The charge
and size of the
metal ion
17.Which of the following is an example of a
monodentate ligand? EDTA Ethylenediamine
Cyanide ion
(CN⁻)
Oxalate ion
(C₂O₄²⁻)
18.Why is EDTA commonly used as a titrant in
complexometric titrations?
It is a
monodentate
It forms multiple
strong bonds
It changes color
during the
It only reacts
with transition

3. UNIT-3 TITRIMETRIC ANALYSES
ligand.
with metal ions,
creating a stable
complex. reaction. metals
19.Which indicator is commonly used in the
titration of calcium and magnesium ions with
EDTA?
Phenolphthale
in Methyl orange
Eriochrome
Black T Starch
20.What characteristic should an ideal
metallochromic indicator have in
complexometric titrations?
It should have
a sharp color
change at the
end point.
It should be a
strong acid.
It should be
insoluble in
water.
It should have
a very slow
reaction rate.
SECTION -B
21.What is the definition of a redox titration?
22.How is the standard reduction potential (E°) related to the feasibility of a redox reaction?
23.What is a redox indicator, and how does it function in redox titrations?
24.Explain the difference between direct and indirect titrations.
25.What are stepwise formation constants, and why are they important in complexometric titrations?
26.Describe the role of EDTA in complexometric titrations.
27.What is the common ion effect, and how does it influence solubility in redox and complexometric titrations?
28.What factors should be considered when choosing a redox indicator for a titration?
29.Explain the concept of masking agents in complexometric titrations.
30.What is the purpose of calculating the potential at different stages of a redox titration?
SECTION -C
31.Discuss the theory behind redox titrations, including the calculation of redox potentials at various stages of the titration. How
does the Nernst equation apply in these calculations, and what information can be derived from the titration curve?
32.Analyze the choice and application of redox indicators in titrations. Discuss at least two examples of redox indicators,
including their chemical basis, color change, and suitable applications.

4. UNIT-3 TITRIMETRIC ANALYSES
33.Explain the principles of complexometric titrations, focusing on the role of monodentate and multidentate ligands. Compare
the complexation reactions involving Cl⁻ and CN⁻ with those involving EDTA, and discuss their applications in analytical
chemistry.
34.Discuss the concept of metallochromic indicators and their significance in complexometric titrations. Provide examples of
metallochromic indicators, their mechanism of action, and how their choice can influence the outcome of the titration.
35.Examine the methods of masking and demasking in complexometric titrations. Describe the rationale for using these methods,
the types of reagents employed, and their impact on the accuracy and precision of the titration results.
36.Compare and contrast direct and indirect titration methods, including substitution titrations. Discuss their theoretical basis,
advantages, and typical applications in analytical chemistry, providing examples for each method.