how do you know which halide salts confirms a presence of F- ions, Cl- ions, Br- ions, and I- ions?
Imagine receiving the same question from your chem teacher that Amanda had eleven years ago. Why are we still asking the same question? Did we ever get an answer?
Amanda--I must admit that I don't have the slightest idea what you are asking. Is there some added information you have that might help?
im sorry.. i don't even know how to ask. maybe if i knew what i was doing i could ask. but we did a lab about halide ions. we used NaF, CaCl, NaBr, and NaI. we used reagents Ca(NO3)2, AgNO3, NH3(aq), Na2S2O3, and starch + NaOCl. we had to tell if a precipitate formed and the color it changed to. and then the first question asks.. which procedures confirms the presence of a. F- ions b. Cl- ions c. Br- ions d. I- ions.
maybe that will help? i have no clue what to do.
That helps.
I don't know the order in which these test were done; however, here is some back ground that may help you get started.
CaF2 is insoluble in water; therefore, CaCl2 + F^- gives a white ppt.
AgNO3 reacts with Cl^-, Br^- and I^- producing AgCl (white ppt), AgBr(pale yellow ppt), and AgI(a darker yellow ppt). AgCl is soluble in NH3, AgBr is slightly soluble in NH3, and AgI is not soluble in water.
NaOCl reacts with I^- to produce I2 (iodine) which turns a VERY DARK blue (if there is very much I2 there it will be so dark it will look black) when stach is added. The color is removed with Na2S2O3.
There should be enough information here to allow you to pick and choose, either individually or in combination, what you need. For example, the confirmation test for Cl^- is treatment with AgNO3, add NH3, the WHITE ppt dissolves completely. (I don't call the treatment with AgNO3 as part of the confirmation but the AgNO3 must be added to obtain the AgCl which then can be used in what I call the confirmation test. Your teacher probably gave you some instructions that should be helpful here. Another confirming test, for I^-, treat some of the sample with NaOCl, add starch, a dark blue to black color which disappears upon addition of Na2S2O3 confirms the presence of iodide ion.
agh3+no3
sorry its taken me so long but I sadly have not figured out the answer to your question but the fact that it has been 7 years i'm hoping you found it
lol val
Swag’s reply is also a year after val’s
2022 and were still being asked the same question with no answer
To determine which halide salts confirm the presence of fluoride ions (F-), chloride ions (Cl-), bromide ions (Br-), and iodide ions (I-), we can use a simple testing method known as precipitation reactions.
1. To test for fluoride ions (F-), add a few drops of a solution containing the suspected fluoride ions to a small amount of silver nitrate solution (AgNO3) or silver acetate solution (AgC2H3O2). If a white precipitate forms, it indicates the presence of fluoride ions.
2. To test for chloride ions (Cl-), add a few drops of a solution containing the suspected chloride ions to a small amount of silver nitrate solution (AgNO3). If a white precipitate forms, it confirms the presence of chloride ions.
3. To test for bromide ions (Br-), add a few drops of a solution containing the suspected bromide ions to a small amount of silver nitrate solution (AgNO3). If a cream or pale yellow precipitate forms, it indicates the presence of bromide ions.
4. To test for iodide ions (I-), add a few drops of a solution containing the suspected iodide ions to a small amount of lead(II) nitrate solution (Pb(NO3)2). If a yellow precipitate forms, it confirms the presence of iodide ions.
These precipitation reactions are based on the solubility rules for halide salts with silver and lead(II) ions. Each halide salt has a specific solubility product constant and tends to form precipitates with specific metal ions.
Please note that it's important to handle chemicals with care and follow proper safety precautions when conducting these tests.