When 400 mL of 0.2 M H2SO4 solution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is …………… × 10–2 K. [Use : H+(aq) + OH– → H2O; ΔyH = –57.1 kJ mol–1 Specific heat of H2O = 4.18 J K–1 g–1 Density of H2O = 1.0 g cm–3 Assume no. change in volume of solution on mixing.]

Engineering

Chemistry

Enthalpy of Neutralisation and Resonance Energy

Question

When 400 mL of 0.2 M H₂SO₄ solution is mixed with 600 mL of 0.1 M NaOH solution, the increase in temperature of the final solution is …………… × 10^–2 K.

[Use : H⁺(aq) + OH^– → H₂O; Δ_yH = –57.1 kJ mol^–1

Specific heat of H₂O = 4.18 J K^–1 g^–1

Density of H₂O = 1.0 g cm^–3

Assume no. change in volume of solution on mixing.]

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H₂SO₄ + 2NaOH $\to_{}^{}$ Na₂SO₄ + 2H₂O

Milimole 80 60 LR is NaOH

Or H⁺ + OH^– $\to_{}^{}$ H₂O

Milimole 160 60 –

(160–60) 60 –

Heat released = 57.1 × 60 × 10^–3 = 3.426

Total mass of solution = 1000 gram

Q = m.s.ΔT ⇒ 3426 = 1000 × 4.18 × ΔT

ΔT = 0.8196 = 81.96 × 10^–2