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Across 1. The conjugate base of nitric acid 3. This solution is a system that minimises the pH changes when small amounts of acid or alkali are added. 5. Calculated from -log base 10 [hydrogen ion] 8. Describes an acid that fully dissociates 9. High pH means a ______ hydrogen ion concentration 11. A soluble base 12. This is the point where an indicator just changes colour i.e Point where concentrations of [HIn] and [In-] 16. 10 to the power -pH = ________ _____ _____________________ 17. Acid + ______________ makes a salt, carbon dioxide and water 18. The conjugate base of HCl 19. this equals [Hydrogen ions] [hydroxide ions] and is known as the Ionic Product of Water 23. This refers to the type of acid where one H ion in the acid can be replaced per molecule 25. Definition of a Bronsted-Lowry acid 26. The higher the value of Ka the ______________ the acid 27. A buffer solution is formed from excess -_____ _______ + and an alkali 28. Definition of a Bronsted-Lowry base

Down 2. Ka 4. This point is found at the centre of the vertical section of a pH titration curve 5. A tribasic acid 6. Possible indicator for a strong acid - weak base titration 7. The carbonic acid- hydrogen carbonate buffer system is the most important in maintaining the pH of the __________ plasma 10. Describes an acid that partially dissociates 13. pH of pure water at 25oC 14. Best indicator for a strong acid-strong base titration 15. H2CO3 is the formula of ________________ _______ 20. The higher the value of pKa the _______________ the acid 21. The number of decimal places given for pH values 22. The Ka of a weak acid can be determined by making a _______________ solution of the acid and then measuring the pH with a pH probe. The values are then put into the Ka expression 24. This happens to the pH of water as the temperature of the water increases. 25. A conjugate acid-base pair comtains 2 species that can be interconverted by transfer of a _____________