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Reactions of Halide Ions with Different Reagents

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Purpose

The purpose of this lab is to observe the reactions of halide ions with different reagents by mixing them together. Analyze data to determine the characteristic reactions of each halide ion. Infer the identity of unknown solutions.

Materials

  •  0.1 M AgNo3
  • 0.1 M NaCl
  • 0.1 M NaF
  • 0.2 M KBr
  • 0.2M Kl
  • 0.2 M Na2S2)3
  • 0.5 M Ca(NO3)2
  • 3% Starch solution
  • 5% NaOCl ( commercial bleach)
  • 12 test tubes, 18 mm X 150 mm test tube rack
  • Pipette

Procedure

  1. Place the 4 solutions in separate test tubes with about 2.5 mL in each.
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    (NaF, NaCl, KBr, KI) Use a dropper or you can use a pipette. Add 1 Ml ( 20 drops) of 0.5 M Ca ( NO3h) to each test tubes. Observe and record. Make sure to note which one DID NOT precipitate.

  2. Drain the 4 test tubes and refill them with clean solutions. (NaF, NaCl, KBr, KI) This time add 2.5 mL (20 drops) of 0.1 M AgNo3 to each of the test tubes. Observe and record in the data table.
  3. This time do not drain the already mixed solutions.

    Add 2.5 mL of 0.2 Na2S2O3 and record your observations.

  4. Drain the test tubes and refill with (NaF, NaCl, KBr, KI) Add 2.5 mL of 3% starch to each test tube, Afterword add a drop or 2 of 5% NaOCI (commercial bleach). Record observations
  5. Get the 2 unknown solutions and repeat steps 1-4.

Data/Observations

  • Refer to Data Table
  • NaF = sodium fluoride
  • NaCI= table salt
  • KBr= Potassium bromide (KBr) is a salt
  • KI= Potassium Iodide
  • Ca(NO3)2= Calcium nitrate
  • AgNO3= Silver nitrate

Both sodium fluoride and calcium nitrate are salts formed from a strong acid and strong base. When any such salt dissolves in water, it completely dissociates into ions. For the ions to react, however, either precipitation would occur. The reason why sodium fluoride and calcium nitrate would react is that calcium fluoride is insoluble in water but other calcium halides are highly soluble. This is also why the other halides did not form any reaction with the Calcium Nitrate. The precipitate forms because the solid (AgCl) is insoluble in water. Salts containing Group I elements are soluble (Li+, Na+, K+, Cs+, Rb+). Exceptions to this rule are rare. Salts containing the ammonium ion (NH4+) are also soluble. Salts containing Cl -, Br -, I – are generally soluble. Fluorides are frequently insoluble. The two unknowns are NaCl and KBr.

Calculations

There was no calculation for this lab

Conclusion

A halide is a binary compound, of which one part is a halogen atom and the other part is an element or radical that is less electronegative than the halogen, to make a fluoride, chloride, bromide, iodide, or astatide compound. Many salts are halides. All Group 1 metals form halides which are white solids at room temperature. A halide ion is a halogen atom bearing a negative charge. The halide anions are fluoride (F−), chloride (Cl−), bromide (Br−), iodide (I−), and astatide (At−). Such ions are present in all ionic halide salts. An easy way to remember the results is that as we move down Group VII of the periodic table, the colors get “darker”. So AgF is colorless because it is completely soluble, AgCl forms white precipitation, AgBr forms cream precipitation, and AgI forms a yellow ppt. Halide compounds such as KCl, KBr, and KI can be tested with silver nitrate solution, AgNO3. The halogen will react with Ag+ and form a precipitate, with varying color depending on the halogen:

Cite this Reactions of Halide Ions with Different Reagents

Reactions of Halide Ions with Different Reagents. (2016, Oct 27). Retrieved from https://graduateway.com/reactions-of-halide-ions-with-different-reagents/

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