Halide Ions Lab
Reactivity of Halide Ions
Michelle Faktor and Kelly Freas
Date of Experiment: October 28, 2012
Period 2
Honors Chem
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 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. (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 …show more content…
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 …show more content…
When any such salt dissolves in water, it completely dissociate into ions. For the ions to react, however, either precipitation would occur. The reason why sodium fluoride and calcium nitrate would react is because 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
Michelle Faktor and Kelly Freas
Date of Experiment: October 28, 2012
Period 2
Honors Chem
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 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. (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 …show more content…
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 …show more content…
When any such salt dissolves in water, it completely dissociate into ions. For the ions to react, however, either precipitation would occur. The reason why sodium fluoride and calcium nitrate would react is because 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