2. An amphiprotic substance can do either!

6. Strong acid Strong base Weak acid Weak base

8. For weak acids we ignore the water as it is constant in aqueous solutions K becomes Ka. The acid dissociation constant

11. In a question, decide whether you write an expression for Ka or Kb. OH - as a product means Kb. H 3 O + means Ka

14. Product of [H 3 O + ] and [OH - ] always equals 10 -14

15. Ions will not react with water so therefore neutral Use the formula to determine the [OH - ] Write the equation for dissolving then the ion reacting with water

16. Pick out the strong acid and base. Remember these go to completion when writing equations Pick out the acidic salt then the weak base

17. Don’t be scared! Use the formula as given for the acid and write equation

18. What equation links H 3 O + with pH?

19. Volume Conc. Moles

20. Look back over the question to see what you have You have [H 3 O + ] You have [HPab] You have the Ka expression Make your assumptions and insert How do we get from Ka to pKa?

21. Amines are weak bases... Hmmmm...no info. We’ll have to use the equations logically Weak bases only partially dissociate so it must be greater than conjugate [OH - ] = [CH 3 NH 3 + ] Weak base so [OH - ] must be greater than [H 3 O + ] Use both equations. Use first formula to predict Cl- [NH 4 + ] would have been the same as [Cl - ] at start, but at equilibrium, some would be changed to NH 3 [NH 4 + ] would be greater than its conjugate as weak acids only partially dissociate [NH 3 ] is the same as [H 3 O + ] In a weak acid, [H 3 O + ] is greater than [OH - ]

22. Ions that move in an electric field With water

23. Salt of a weak acid Must be a weak base Show the equation to show the salt dissolves Show the equation with water only one works!

24. Write equilibrium equation of NH 3 What happens when NH 4 Cl dissolves? Show equation So the NH 4 + increases...what effect will this have on the equilibrium What effect will this have on the H 3 O + conc?