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The pH Scale

The pH Scale. Acids. Practical preperation Record into your book. Acids. Try the practical again, but this time instead of using drops of liquid we will use a small piece of paper This time you do not need to record anything but the method is a little different

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The pH Scale

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  1. The pH Scale

  2. Acids • Practical preperation • Record into your book

  3. Acids • Try the practical again, but this time instead of using drops of liquid we will use a small piece of paper • This time you do not need to record anything but the method is a little different • Take a small piece of indicator paper and put 1 or 2 small drops of a single solution on it. Observe the colour. • When you are finished try another solution. Try to keep a sample of all the solutions that you try

  4. Acids and Bases • Acids and bases are one way of classifying solutions • Using “Universal Indicator” we are able to compare different solutions as they will give different colour results • Classifying how acidic or basic a solution is can be done using the pH scale

  5. The pH Scale • The pH scale indicates the number of Hydrogen ions in a solution and goes from 0 to 14 • ACIDS have a pH from 0 to 7 • BASES have a pH from 7 to 14 • If something has a pH of 7 it is NEUTRAL

  6. Do Now • Complete the following formulae: • Na+ + Cl- • K+ + Cl-  • Cl- + H+  • K+ + OH-  • Be careful with these ones! • Mg2+ + Cl-  • NH4+ + OH-  • Ca2+ + OH- 

  7. Do Now • Complete the following formulae: • Na+ + Cl- NaCl • K+ + Cl-  KCl • Cl- + H+  HCl • K+ + OH-  KOH • Mg2+ + Cl-  MgCl2 • NH4+ + OH-  NH4OH • Ca2+ + OH-  CaOH2

  8. Do Now • Complete the following formulae: • Mg2+ + O2-  • Ca2+ + Cl-  • NH4+ + O2- 

  9. Balancing equations • When we have situations like Mg2+ + Cl-  MgCl2 And we look at the number of each type of atom on each side of the arrow they are not the same. When we have a situation like this we must add numbers in front of the ions or elements in order to “balance” the equation Mg2+ + 2Cl-  MgCl2

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