In the presence of heat, copper (II) hydroxide decomposes in to copper (II) oxide. Cu(OH)₂ (s) ----> CuO (s) + H₂O (l) upon decomposition, water is removed from Cu(OH)₂ the amount of Cu(OH)₂ decomposed - 3.67 g number of moles of Cu(OH)₂ - 3.67 g / 97.5 g/mol = 0.038 mol stoichiometry of Cu(OH)₂ to CuO is 1:1 therefore number of CuO moles formed are - 0.038 mol CuO reacts with sulfuric acid to form CuSO₄ CuO + H₂SO₄ ---> CuSO₄ + H₂O stoichiometry of CuO to H₂SO₄ is 1:1 therefore number of H₂SO₄ moles that should react is 0.038 mol the molarity of H₂SO₄ is 3M this means that in 1000 ml - 3 mol of H₂SO₄ present so if 3 mol are present in 1000 ml then volume for 0.038 mol = 1000/3 * 0.038 = 12.67 ml
