CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS

analytical chemistry question

1. UNIT-2 CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS
QUESTION A B C D Answer
1.Which of the following statements about chemical
equilibrium is correct?
The
concentrations
of reactants and
products are
equal at
equilibrium.
The rate of the
forward reaction
equals the rate of
the reverse
reaction at
equilibrium.
A catalyst shifts
the position of
equilibrium.
Equilibrium is
reached only
when no
reactants
remain.
2.For the following reaction: 2NO₂(g) N
⇌
₂O₄(g), if
the pressure is increased, what will happen to the
equilibrium position?
Shift to the
right (favoring
products)
Shift to the left
(favoring
reactants) No change
The reaction
will stop
3.Which of the following is true for a system at
dynamic equilibrium?
Both the
forward and
reverse
reactions have
stopped.
The system is in a
closed container.
The temperature
of the system must
decrease for
equilibrium to
occur.
The
concentration
of products
continues to
increase.
4.The pH of a solution is defined as:
The negative
logarithm of
the hydroxide
ion
concentration.
The positive
logarithm of the
hydrogen ion
concentration.
The negative
logarithm of the
hydrogen ion
concentration.
The negative
logarithm of
the water
concentration.
5.What is the pH of a solution with a hydrogen ion
concentration of 1×10
−4
 
M? 2 4 6 10
6.If the pH of a solution decreases from 7 to 4, the
concentration of hydrogen ions:
Increases by 3
times
Increases by 1000
times
Decreases by 3
times
Decreases by
1000 times
7.What is the pH of the solution when a salt formed
by the reaction of a strong acid and a strong base is
dissolved in water? Greater than 7Less than 7 Less than 7
Variable
depending on
the
concentration
8.Which of the following salts will form an acidic
solution upon hydrolysis? NaCl NH₄Cl KNO₃ Na₂CO₃
9.Which of the following salts will form a basic
solution upon hydrolysis? Na₂CO₃ FeCl₃ NaNO₃ KCl
10.The hydrolysis of sodium acetate (CH₃COONa)
results in a solution that is: Neutral Acidic Buffer solution Basic
11.According to the Arrhenius theory, an acid is a
substance that:
Increases the
hydroxide ion
Increases the
hydrogen ion
Donates an
electron pair
Accepts a
proton

2. UNIT-2 CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS
concentration
in water
concentration in
water
12.Which of the following pairs of compounds
represents a conjugate acid-base pair according to
the Brønsted-Lowry theory? HCl and Cl⁻ HCl and OH⁻ NH₃ and H₂O NaOH and H₂O
13.According to Lewis theory, a base is defined as a:Proton donorProton acceptor
Electron pair
donor
Electron pair
acceptor
14.Which of the following substances is an amphoteric
compound, meaning it can act as both an acid and a
base? NaOH HCl H₂SO₄ H₂O
15.Which indicator would be most suitable for a
titration between a strong acid and a strong base?Methyl orange Phenolphthalein Litmus
Bromothymol
blue
16.For a titration between a weak acid and a strong
base, the best indicator is: Methyl orange Phenolphthalein Litmus
Bromothymol
blue
17.Which of the following pH ranges is suitable for
methyl orange as an indicator? 3.1 – 4.4 4.5 – 7.0 6.0 – 8.0 8.3 – 10.0
18.In a titration between a weak base and a strong
acid, which indicator should be used? Methyl orange Phenolphthalein Litmus
Bromothymol
blue
19.Which of the following is a characteristic of a
monoprotic acid?
It donates
multiple
protons per
molecule
It donates only
one proton per
molecule
It accepts one
proton per
molecule
It can donate
two or more
protons
depending on
the pH.
20.For a polyprotic acid, which dissociation constant
(Ka) is the largest? Ka₁ Ka2 Ka3
They are all
equal
SECTION -B
21.Define the concept of chemical equilibrium.
22.What is the equilibrium constant (K) and how is it calculated for a chemical reaction?
23.Explain the difference between strong and weak acids in terms of ionization constants (Ka).
24.What is pH, and how is it related to the concentration of hydrogen ions in a solution?
25.Describe the process of hydrolysis of salts and its effect on pH.
26.What is the purpose of a buffer solution, and how does it maintain pH stability?

3. UNIT-2 CHEMICALEQUILIBRIAANDNEUTRALIZATIONREACTIONS
27.Explain the common ion effect and its significance in solubility equilibria.
28.What are the key differences between monodentate and polydentate ligands in terms of complex formation?
29.Define the degree of hydrolysis and its relation to the hydrolysis constant.
30.What factors influence the choice of indicators in acid-base titrations?
SECTION -C
1.Discuss the activity concept in chemical equilibria. How does it differ from concentration, and why is it important in the
calculation of equilibrium constants? Provide examples to illustrate your points.
2.Explain the dissociation of polyprotic acids, using sulfuric acid as an example. Discuss how each dissociation step affects pH
and the overall acid strength, including the calculation of relevant ionization constants.
3.Analyze the different types of buffers, including their composition and range. Discuss how buffer capacity is determined and
provide examples of common buffer systems used in laboratory settings.
4.Describe the theory behind acid-base titrations, focusing on the concept of equivalence point versus end point. How can
titration curves be used to determine the appropriate indicator for a given titration?
5.Evaluate the hydrolysis of salts in terms of pH changes in solution. Discuss the factors that affect the degree of hydrolysis and
how this impacts the pH of solutions formed from salts of weak acids and bases.
6.Discuss the applications of the common ion effect and salt effect in chemical equilibria. Provide examples of how these effects
can influence solubility and the behavior of buffers in various chemical systems.