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Practical Observation and Deduction in Inorganic Chemistry Exercises

Explore inorganic and organic chemistry pairs of activities with observations and deductions. Examples include identifying halide ions, testing for gases, and conducting precipitation reactions. Learn about metal carbonate reactions and the properties of aqueous ions.

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Practical Observation and Deduction in Inorganic Chemistry Exercises

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  1. Welcome and thanks for visiting. Module 3 Practical: Observation and Deduction 2002-7 NaClFind LEf F Scullion. JustChemy.Com

  2. Inorganic Observation and Deduction

  3. The observations and deductions come in pairs of activities. One involves inorganic chemistry and the other organic chemistry. The inorganic exercise typically involves the analysis of a so-called “Double Salt”. One of the ions in these mixed salts is common to both salts in most cases. Here are some examples: - Sodium Sulphate and Sodium Chloride Calcium Carbonate and Calcium Chloride

  4. Deductions.

  5. Observations A is Ammonium Chloride NH4Cl

  6. Identifying halide ions in solution Na The equations for the reactions are represented thus:NaX(aq)  +  AgNO3(aq)   =   AgX(s)  +  NaNO3(aq) 

  7. Why Can’t You hite ream ellow NaCl(aq)  +  AgNO3(aq)   =   AgCl(s)  +  NaNO3(aq)                                                white pptNaBr(aq)  +  AgNO3(aq)   =   AgBr(s)  +  NaNO3(aq)                                                cream pptNaI(aq)  +  AgNO3(aq)   =   AgI(s)  +  NaNO3(aq)                                              yellow ppt

  8. Both AgCl and AgBr are light sensitive. They have darkened noticeably after 5 minutes AgBr

  9. Solubility of Silver Halides in Ammonia solution.

  10. Ammonium Compounds warm Ammonium + Alkali  Salt + NH3 + H2O Compound warm NH4Cl + NaOH  NaCl + NH3 + H2O warm (NH4)2SO4 + Ca(OH)2  CaSO4 + 2NH3 + 2H2O

  11. (ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. White [1] fumes/smoke [1] glass rod [1] dipped in conc [1] ammonia [1] (max [4]) AMMONIUM + ALKALI  SALT + AMMONIA + WATER COMPD NH4Cl + NaOH  NaCl + NH3 + H2O

  12. Observations

  13. Observations

  14. It is Potassium Carbonate

  15. Potassium flame test & Emission spectrum Lilac

  16. Using HCl & Limewater to test for CO32- Effervescence Limewater Sample of dilute HCl (aq) Sign of CO2 gas

  17. Using Magnesium Nitrate to test for the presence of CO32-(aq) CO32-(aq)+ Mg2+(aq) MgCO3(s)

  18. Reactions of the Carbonate Ion. Metal Carbonate + Acid  Salt + CO2 + H2O Partial Ionic Equation CO32- + H+ H2O + CO2 Balanced Symbol Equation K2CO3 + 2HCl  2KCl + H2O + CO2 -------------------------------------------------------- Precipitation Reaction AB(aq) + CD(aq)  AD(s) + CB(aq) Partial Ionic Equation CO32- + Mg2+ MgCO3 Balanced Symbol Equation K2CO3 + MgCl2 MgCO3 + 2KCl

  19. Observation A is a “double salt”

  20. A is a “double salt”

  21. Colour is a feature of the compounds of TMs Cobalt chloride above Potassium chromate above Nickel chloride opposite Above is from the Chemguide Website

  22. Copper(II) ion, Cu2+(aq) Chromium(III) ion, Cr3+(aq) Iron(II) ion, Fe2+(aq) Chromate ion, CrO42-(aq) Iron(III) ion, Fe3+(aq) Dichromate ion, Cr2O72-(aq) Cobalt(II) ion, Co2+(aq) Manganese(II) ion, Mn2+(aq) Nickel(II) ion, Ni2+(aq) Permanganate ion, MnO4-(aq) Colour of Aqueous Ions

  23. Copper(II) ion, Cu2+(aq) blue Chromium(III) ion, Cr3+(aq) deep green Iron(II) ion, Fe2+(aq) green Chromate ion, CrO42-(aq) yellow Iron(III) ion, Fe3+(aq) Yellow Dichromate ion, Cr2O72-(aq) orange Cobalt(II) ion, Co2+(aq) pink Manganese(II) ion, Mn2+(aq) very pale pink / colourless Nickel(II) ion, Ni2+(aq) deep green Permanganate ion, MnO4-(aq) deep purple Colour of Aqueous Ions

  24. Ammonium Compounds warm Ammonium + Alkali  Salt + NH3 + H2O Compound warm NH4Cl + NaOH  NaCl + NH3 + H2O warm (NH4)2SO4 + Ca(OH)2  CaSO4 + 2NH3 + 2H2O

  25. (ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. White [1] fumes/smoke [1] glass rod [1] dipped in conc [1] ammonia [1] (max [4]) AMMONIUM + ALKALI  SALT + AMMONIA + WATER COMPD NH4Cl + NaOH  NaCl + NH3 + H2O

  26. NH3(aq) A weak alkali JustChemy.Com Dilute ammonia solution with UI: about pH 11

  27. Lithium Calcium Crimson Red Brick Red Strontium Red

  28. Reactions of the Halide Ions with AgNO3(aq). Silver + Sodium  Silver + Sodium Nitrate Halide Halide Nitrate Partial Ionic Equation using X- for Halide Ions Ag+ + X- AgCl Balanced Symbol Equation AgNO3 + NaX AgX + NaNO3 AgNO3 + NaCl AgCl + NaNO3 AgNO3 + NaBr AgBr + NaNO3 AgNO3 + NaI AgI + NaNO3

  29. Mixture of Ammonium Chloride and Li/Sr/Ca Chloride

  30. Acidified Barium Chloride (or Nitrate) is used to test for SO 42-(aq) Ba2+(aq) + SO42-(aq) BaSO4(s)

  31. Has Ammonium Sulphate and Sodium Sulphate

  32. Ammonium Compounds warm Ammonium + Alkali  Salt + NH3 + H2O Compound warm NH4Cl + NaOH  NaCl + NH3 + H2O warm (NH4)2SO4 + Ca(OH)2  CaSO4 + 2NH3 + 2H2O

  33. (ii) Describe how you would carry out the test for hydrogen chloride gas and state what you would observe. White [1] fumes/smoke [1] glass rod [1] dipped in conc [1] ammonia [1] (max [4]) AMMONIUM + ALKALI  SALT + AMMONIA + WATER COMPD NH4Cl + NaOH  NaCl + NH3 + H2O

  34. NH3(aq) A weak alkali JustChemy.Com Dilute ammonia solution with UI: about pH 11

  35. Flame test for Sodium Orange-yellow

  36. Complete Formula Equation: BaCl2(aq) + CuSO4(aq) BaSO4(s)  + CuCl2(aq) Complete Ionic Equation: Ba2+(aq) + 2 Cl-(aq) + Cu2+(aq) + SO42-(aq)  BaSO4(s) + Cu2+(aq) + 2 Cl-(aq) Net Ionic Equation: Ba2+ + 2 Cl- + Cu2+ + SO42- BaSO4(s) + Cu2+ + 2 Cl-       Ba2+(aq) + SO42-(aq) BaSO4(s)

  37. Observations A is a mixture of 2 salts

  38. Observations A is a White solid A is a mixture of 2 salts

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