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Reactions of Acid

Reactions of Acid. Today’s Lesson. As I’m not here today, could you please complete the lesson in this order. Complete experiment sheet from last lesson Complete work on reactions of acids Complete work on neutralizations. Experiment Work.

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Reactions of Acid

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  1. Reactions of Acid

  2. Today’s Lesson • As I’m not here today, could you please complete the lesson in this order. • Complete experiment sheet from last lesson • Complete work on reactions of acids • Complete work on neutralizations

  3. Experiment Work • Please complete the questions from your titrations experiment. • If you have lost the sheet – it can be found here: http://yis9chem.wikispaces.com/file/detail/Titrations.docx • I will collect the sheets next lesson to make sure they have been completed

  4. Reactions of Acids • When you react an acid with an alkali (base), you normally have a very simple reaction that occurs: • Acid + alkali  salt + water • This can be seen with a universal indicator. Hydrochloric Acid will turn red as it’s acidic. • When you add Sodium Hydroxide (alkali), it goes green as it turns neutral. • As more Sodium Hydroxide is added, it will turn blue as there is no more Hydrochloric acid left.

  5. Examples • Sulfuric Acid + Magnesium Hydroxide  Magnesium Sulfate + Water • H2SO4 (aq) + Mg(OH)2 (aq)  MgSO4 (aq)+ 2H2O (l) • Nitric Acid + Potassium Hydroxide  Potassium Nitrate + Water • HNO3 (aq) + KOH (aq)  KNO3 (aq) + H2O (l)

  6. With Metals • With metals, a salt is also produced but there may also be another byproduct such as a gas. • A good example is Magnesium Ribbon in Sulfuric Acid • Magnesium + Sulfuric Acid  Magnesium Sulfate + Hydrogen • Mg (s) + H2SO4 MgSO4 (aq) + H2 (g) • The Magnesium Sulfate can be separated through evaporation.

  7. Carbonates • With Carbonates, acids will normally form 3 substances. These substances are a salt, water and Carbon Dioxide. • An example is Calcium Carbonate + Hydrochloric Acid  Calcium Chloride + Water + Carbon Dioxide • CaCO3 (s) + 2HCl (aq)  CaCl2 (aq) + H2O (l) + CO2 (g)

  8. With Bases • Alkalis are soluble bases. • An example is Copper (II) Oxide + Sulfuric Acid  Copper Sulfate + Water • CuO (s) + H2SO4 (aq)  CuSO4 (aq) + H2O (l) • The salt is Copper Sulfate for this reaction.

  9. Basics • Acid + Metal Hydroxide  Metal Salt + Water • Acid + Metal  Metal Salt + Hydrogen • Acid + Metal Carbonate  Metal Salt + Water + Carbon Dioxide • Acid + Metal Oxide  Metal Salt + Water

  10. Your Work • Please read Page 46/47 and answer Q 1-6 in sentences.

  11. Neutralization • What makes something an acid?? • For Hydrochloric Acid: • HCl (aq)  H+ (aq) + Cl- (aq) • What makes a base a base? • For Sodium Hydroxide: • NaOH (aq)  Na+ (aq) + OH- (aq)

  12. Neutralization Reaction • Below is an example of a neutralization reaction: • HCl (aq) + NaOH (aq) NaCl (aq) + H2O (l) • As ions, you would write it like this: • H+ (aq) + OH- (aq)  H2O (l) • Note how the Hydrogen and Hydroxide form water!

  13. Questions • Could you please read Page 48-49 and answer Q 1-4 in sentences. • If you finish early, you can also read Page 50-51 and answer Q 1-5. This will be our next lesson (along with an experiment on identifying acids/bases using litmus paper, universal indicator and pH meter

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