1. By Torben

2. Acids – Prior Knowledge? Record at least the ones you weren’t sure of 1.What is an acid? 2.What determines if an acid is strong or weak? 3.What determines if an acid is concentrated or dilute? 4.Examples of strong acids? 5.Examples of weak acids? 6.Describe the pH scale? 7.What are indicators? 8.How do they work (just the basic idea)? 9.Give examples of indicators with colour changes 10.What is a base? Is it the same as an alkali? 11.What is a salt?

3. Notes – using the specification to guide us

5. Last year many students lost loads of marks on observations during the coursework. This is your chance to prevent that. Record your observations as if you were completing coursework. We can then learn from our mistakes (hopefully) Last year many students lost loads of marks on observations during the coursework. This is your chance to prevent that. Record your observations as if you were completing coursework. We can then learn from our mistakes (hopefully)

6. Step 1 - observations Hydrochloric acid + Copper (II) oxide ethanoic acid + Copper (II) oxide

7. Step 2 - observations Hydrochloric acid + sodium hydroxide ethanoic acid + sodium hydroxide

8. Step 3 - observations Hydrochloric acid + sodium hydroxide then indicator then excess Hydrochloric acid ethanoic acid + sodium hydroxide then indicator then excess ethanoic acid

9. Step 4 - observations Hydrochloric acid + calcium carbonate acid + calcium carbonate

10. Step 5 - observations Hydrochloric acid + magnesium acid + magnesium

12. Key Facts Give the formulae for each of these acids –Sulfuric, Nitric, hydrochloric Give the formulae of each of these –Sodium hydroxide, ammonia, potassium hydroxide, sodium carbonate

13. Handy Memory Aids 1.Acid + metal → 2.Acid + metal oxide → 3.Acid + metal hydroxide → 4.Acid + metal carbonate → 5.Acid + metal hydrogen carbonate → What are likely observations for each of the above?

14. pH A student has a solution of 1 mol dm -3 hydrochloric acid Suggest a likely pH How might the pH change if we add water How might the pH change if we add NaOH

15. Some Common ions CationsAnions

16. Some Common ions CationsAnions Roman numerals

17. Balanced Equations to Complete Work out balanced equations for these reactions Copper (II) oxide + hydrochloric acid Sodium hydroxide + sulfuric acid Calcium carbonate + nitric acid Ammonia + sulfuric acid Copper (II) carbonate + ethanoic acid (CH 3 COOH)

18. If an acid can be considered to be: And your white board is a beaker full of water A-A- H+H+

19. Draw a diagram to show A solution of a weak concentrated acid.

20. Draw a diagram to show A solution of a strong concentrated acid.

21. Draw a diagram to show A solution of a weak dilute acid.

22. Draw a diagram to show A solution of a strong dilute acid.

24. You should: Know the meanings of the terms: –anhydrous, –Hydrated –water of crystallisation. Be able to calculate the formula of a hydrated salt from: –percentage composition –mass composition –experimental data.

26. 1.Calculate the empirical formula of hydrated cobalt (II) chloride 2.Try to write this in the style XCl ?.?H 2 O

27. Answers are behind this

28. 1.Calculate the empirical formula of anhydrous calcium nitrate 2.Calculate the empirical formula of hydrated calcium nitrate 3.Write the hydrated salt in the.H 2 O style 4.Give an equation for the formation of (anhydrous) calcium nitrate from calcium carbonate

31. Work out this empirical formula A 5g sample of the hydrated form of cobalt chloride was found to be made up of the following: CoClHO 1.24g1.49g0.25g2.02g

34. Hydrated Salts calculations Another Type – Experimental

36. From experimental data Work out the number of moles of anhydrous salt. Work out the number of moles of water driven off. Work out the ratio moles salt : moles water

37. Syllabus Ticking

38. Then tackle the questions at the bottom of the sheet

39. Anhydrous and Hydrated Salts P26-27 orange book