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Precipitation reaction


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Year 10 Precipitation reaction.

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Precipitation reaction

  1. 1. Y E A R 1 0 – C O M P O U N D S A N D R E A C T I O N G . A J E T R A O PRECIPITATION
  2. 2. AIM To investigate precipitation reaction Write a hypothesis for the experiment.
  3. 3. BACKGROUND INFORMATION Precipitation reaction occurs when two solutions are mixed together to form an insoluble compound called precipitate that settles out of solution. AB + CD  AD + BC double displacement reaction
  4. 4. SOLUBILITY RULE Soluble Ionic Compounds • 1. All common compounds of the Group 1A ions (Li+, Na+, K+, etc.) and the ammonium ion (NH4 +) are soluble. • 2. All common nitrates (NO3 -), acetates (C2H3O2 -), and most perchlorates (ClO4 -) are soluble. • 3. All common chlorides (Cl-), bromides (Br-), and iodides (I-) are soluble, except those of Ag+, Pb2+, and Hg2 2+. • 4. All common sulfates (SO4 2-) are soluble, except those of Ca2+, Sr2+, Ba2+, Pb2+, and Ag+.
  5. 5. SOLUBILITY RULE CONTINUED Insoluble Ionic Compounds • 5. All metal hydroxides (OH-) are insoluble, except those of Group 1A, NH4 +, which are soluble, and Ca2+, Sr2+, and Ba2+, which are slightly soluble. • 6. All sulfides (S2-) are insoluble, except those of Group 1A, NH4 +, Ca2+, Sr2+, and Ba2+. • 7. All carbonates (CO3 2-) and phosphates (PO4 3-) are insoluble, except those of Group 1A and NH4 +.
  6. 6. EQUIPMENT Metal ions – barium nitrate, calcium nitrate, lead nitrate, copper nitrate in dropper bottle Non-metal ions- sodium carbonate, sodium chloride, sodium hydroxide, sodium sulfate, sodium iodide in dropper bottle. • Spotting plate
  7. 7. RISK ASSESSMENT Risk Injury Prevention Stain Silver nitrate and lead nitrate are poisonous Avoid contact with skin. Use small amounts of solutions in dropper bottle
  8. 8. METHOD 1. Take a spotting plate. 2. Add one drop of solution to each well of the spotting plate. 3. Add a drop of other solution as shown in the table on the next slide. 4. Record the presence or absence of precipitate. 5. If there is a precipitate observe and record the colour of the precipitate and the colour of the solution.
  9. 9. TABLE CO3 2- Sodium carbonate Cl- Sodium chloride OH- Sodium Hydroxide I- Sodium Iodide SO4 2- Sodium sulfate Ba2+ Barium nitrate Ca2+ Calcium nitrate Pb2+ Lead nitrate Cu2+ Copper nitrate
  10. 10. RESULT TABLE • Construct a result table for data you are going to gather from the investigation.
  11. 11. DISCUSSION 1. Which metals ions are soluble? 2. Which non- metals ions are insoluble?
  12. 12. CONCLUSION • Write a appropriate conclusion (make sure it is related to your results).