Level 3 Aqueous

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Across
  1. 3. The ion, OH⁻, whose concentration is used to calculate the pH of a strong base solution.
  2. 4. The equilibrium constant for the ionisation of water.
  3. 5. The pH at the halfway point of a weak acid–strong base titration is equal to this.
  4. 8. The ion, H₃O⁺, whose concentration is used to calculate the pH of an acidic solution.
  5. 10. A graph showing how pH changes as titrant is added.
  6. 12. The species formed when a base gains a proton.
  7. 13. The process by which a weak acid or base reacts with water to form ions.
  8. 14. The process of decreasing concentration by adding more solvent.
  9. 15. The equation used to calculate buffer pH from pKa and the ratio of conjugate base to weak acid.
  10. 18. The equilibrium constant for a saturated solution of a sparingly soluble ionic solid.
  11. 21. The reactant that is completely consumed first in a chemical reaction.
Down
  1. 1. A charged species formed when a metal ion bonds with ligands such as ammonia.
  2. 2. The species formed when an acid loses a proton.
  3. 4. The equilibrium constant describing the ionisation of a weak acid in water.
  4. 5. An insoluble solid that forms when ions in solution react.
  5. 6. A substance that changes colour over a particular pH range.
  6. 7. The point in a titration when the moles of acid and base are equal.
  7. 9. The presence of this type of ion decreases the solubility of a sparingly soluble ionic solid.
  8. 11. KS need to be smaller than this for a precipitate to form
  9. 16. The part of a titration curve where pH changes relatively little as titrant is added.
  10. 17. A measure of how well a solution carries electrical current due to mobile charged particles.
  11. 19. The state in which the forward and reverse reactions occur at equal rates.
  12. 20. A solution that resists changes in pH when small amounts of acid or base are added.