Enthalpy of Neutralization of Strong Acid and Strong Base NEET Questions

Organic Chemistry - Principles of Practical Chemistry
Enthalpy of Neutralization of Strong Acid and Strong Base

Enthalpy of Neutralization of Strong Acid and Strong Base MCQ Questions


7.
If specific heat of water = 4.184 J/g·°C and 200 g of solution rises by 5°C, the heat absorbed is:
A.
1000 J
B.
10000 J
C.
4184 J
D.
200 J
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ANSWER :
C. 4184 J
8.
When solid CH₃COOH is mixed with NaOH solution, the heat liberated includes:
A.
Only heat of neutralization
B.
Heat of dissolution + heat of ionization + heat of neutralization
C.
Heat of formation
D.
Only heat of dissolution
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ANSWER :
B. Heat of dissolution + heat of ionization + heat of neutralization
9.
Why must ΔT be measured immediately after mixing?
A.
Heat starts dissipating to surroundings as soon as ΔT > T_room; immediate reading minimizes this loss
B.
Thermometer is slow
C.
Reaction is slow
D.
Mixing takes time
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ANSWER :
A. Heat starts dissipating to surroundings as soon as ΔT > T_room; immediate reading minimizes this loss
10.
Heat liberated in neutralization is the result of formation of:
A.
Crystal lattice
B.
New ionic bond
C.
Strong O-H bond in liquid water (energy released > energy spent in ion solvation)
D.
Weak hydrogen bond
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ANSWER :
C. Strong O-H bond in liquid water (energy released > energy spent in ion solvation)
11.
For weak acid HA: HA(aq) ⇌ H⁺(aq) + A⁻(aq), ΔH₁; H⁺(aq) + OH⁻(aq) → H₂O(l), ΔH₂. The overall ΔH for HA + NaOH → NaA + H₂O is:
A.
ΔH₁ / ΔH₂
B.
ΔH₁ × ΔH₂
C.
ΔH₁ - ΔH₂
D.
ΔH₁ + ΔH₂
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ANSWER :
D. ΔH₁ + ΔH₂
12.
If the experimental enthalpy of neutralization is found to be -55 kJ/mol instead of -57.1 kJ/mol, the most likely reason is:
A.
More acid was used
B.
Calorimeter exploded
C.
Wrong stoichiometry
D.
Heat loss to surroundings during experiment
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ANSWER :
D. Heat loss to surroundings during experiment
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