A neutralisation reaction occurs when NaOH(aq) is added to H₂SO₄(aq). equation 1 2NaOH(aq) + H₂SO₄(aq) → Na₂SO₄(aq) + 2H₂O(l)

1. (a)Define enthalpy change of neutralisation, ΔH_neut.[2]
2. (b)(i)An experiment is carried out to calculate ΔH_neut for the reaction between NaOH(aq) and H₂SO₄(aq). 100cm³ of 1.00moldm⁻³ NaOH(aq) is added to 75cm³ of 1.00moldm⁻³ H₂SO₄(aq) in a polystyrene cup and stirred. Results from the experiment are shown in Table 2.1. [Table 2.1] Use equation 1 to calculate the amount, in mol, of H₂SO₄(aq) that is neutralised in the experiment.[1]
3. (b)(ii)Calculate ΔH_neut using the results in Table 2.1. Include units in your answer. Assume that: • the specific heat capacity of the final solution is 4.18Jg⁻¹ K⁻¹ • 1.00 cm³ of the final solution has a mass of 1.00g • there is no heat loss to the surroundings • full dissociation of H₂SO₄(aq) occurs • the experiment takes place at constant pressure. Show your working.[3]
4. (c)(i)Complete the equation for the reaction that occurs when a solution of Ba(OH)₂ is added to aqueous sulfuric acid. Include state symbols. ....... H₂SO₄(aq) + .......Ba(OH)₂(aq) →[2]
5. (c)(ii)Suggest why the enthalpy change of neutralisation cannot be determined using the addition of dilute sulfuric acid to aqueous barium hydroxide.[1]