*WAEC GCE CHEMISTRY THEORY* (1a) i.Aluminum nitrate ii.Chloric acid (1b) Calculate the concentration in mol/dm³ of a solution containing 355 g of Na₃PO₄ in 3.5 dm³ of solution. Molar mass of Na₃PO₄ Na₃PO₄ = (3 × 23.0) + 31.0 + (4 × 16.0) = 69.0 + 31.0 + 64.0 = 164.0 g/mol Number of moles Moles = Mass / Molar Mass = 355 g / 164.0 g/mol ≈ 2.165 mol Concentration Concentration = Moles / Volume = 2.165 mol / 3.5 dm³ ≈ 0.619 mol/dm³ Final Answer: 0.619 mol/dm³ (1c) Ionization energy is the minimum amount of energy required to remove the most loosely bound electron from a neutral atom in its gaseous state. (1d) Ionization energy increases across a period from left to right in the periodic table due to: -Increase in nuclear charge (more protons attract electrons more strongly). -Decrease in atomic radius, making it harder to remove an electron.