Types Of Reaction 1

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First part of lesson on on types of reaction. Suitable for upper secondary students. Best view with Powerpoint 2003 or later.

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Types Of Reaction 1

  1. 1. TYPES OF REACTION <ul><li>Neutralisation or Acid-Base </li></ul><ul><li>Precipitation </li></ul><ul><li>Redox </li></ul>Suitable for Upper Secondary Students Author: Toh Chui Hoon
  2. 2. NEUTRALISATION <ul><li>A reaction between an acid and a base . </li></ul><ul><li>In this reaction, the acid donates a hydrogen ion (H + or proton) to the base leading to formation of water . </li></ul><ul><li>Examples of base : Oxides, Hydroxides and Carbonates </li></ul><ul><li>Examples of acid : Hydrochloric acid, Sulphuric acid and Nitric acid </li></ul>
  3. 3. Examples of Neutralisation <ul><li>Acid + Oxide </li></ul><ul><li>2HCl + Cu O  CuCl 2 + H 2 O </li></ul><ul><li>Acid + Hydroxide </li></ul><ul><li>H 2 SO 4 + 2Na OH  Na 2 SO 4 + 2H 2 O </li></ul><ul><li>Acid + Carbonate </li></ul><ul><li>2HNO 3 + Ca CO 3  Ca(NO 3 ) 2 + H 2 O + CO 2 </li></ul>Gives a H + to O 2- of CuO to form H 2 O
  4. 4. QUIZ <ul><li>Which of the following basic ions can be identified using products from acid-base reaction? </li></ul><ul><li>A : OH - B : O 2- C : CO 3 2- D : Cl - </li></ul>ANSWER : Yes, it is C . When acid is added to carbonates, bubbling or effervescence can be seen due to production of CO 2 gas which will turn limewater, Ca(OH) 2 , cloudy. This is caused by production of CaCO 3 as a result of acid-base reaction between aqueous CO 2 and Ca(OH) 2 . Ca(OH) 2 + CO 2  CaCO 3 + H 2 O Hint: There must visible change in the reaction.
  5. 5. PRECIPITATION <ul><li>This reaction involves 2 water-soluble compounds leading to formation of a water-insoluble compound . </li></ul><ul><li>Examples of water-soluble compounds : all Nitrates, most Sulphates except BaSO 4 and PbSO 4 , most Chlorides except AgCl and PbCl 2 . </li></ul><ul><li>Examples of water-insoluble compounds : Oxides, Hydroxides and Carbonates except those of Na + , K + and NH 4 + . </li></ul>
  6. 6. Coloured Compounds <ul><li>Compounds containing transition metal ions are coloured. </li></ul><ul><li>Copper sulphate, CuSO 4 is blue . </li></ul><ul><li>Iron(II) hydroxide, Fe(OH) 2 is dirty-green . </li></ul><ul><li>Iron(III) hydroxide, Fe(OH) 3 is reddish-brown . </li></ul><ul><li>Potassium dichromate(VI), K 2 Cr 2 O 7 is orange . </li></ul><ul><li>Potassium manganate(VII), KMnO 4 is violet . </li></ul>
  7. 7. Examples of Precipitation <ul><li>HCl(aq) + AgNO 3 (aq)  AgCl(s) + HNO 3 (aq) </li></ul><ul><li>A white precipitate of silver chloride is seen. </li></ul><ul><li>On further addition of aqueous NH 3 , silver chloride dissolved . </li></ul>After excess aq. NH 3 is added…
  8. 8. Examples of Precipitation <ul><li>KI(aq) + AgNO 3 (aq)  AgI(s) + KNO 3 (aq) </li></ul><ul><li>A yellow precipitate of silver iodide is seen. </li></ul>
  9. 9. Examples of Precipitation <ul><li>Na 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq)  BaSO 4 (s) + 2NaNO 3 (aq) </li></ul><ul><li>A white precipitate of barium sulphate is seen. </li></ul>
  10. 10. Examples of Precipitation <ul><li>H 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq)  BaSO 4 (s) + HNO 3 (aq) </li></ul><ul><li>A white precipitate of barium sulphate is seen. </li></ul>

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