Posted by annonomus on Wednesday, August 11, 2010 at 4:17am.
1. Take a clean test tube from the Glassware shelf and place it on the workbench. Add 1 mL your mystery solution to the test tube.
2. PRECIPITATION BY NaC2H3O2(aq)
(a) Add 2 mL of sodium acetate solution to the test tube.
(b) If a white precipitate forms at the bottom of the test tube, decant the remaining liquid into another clean test tube and retain the precipitate. (Decanting is the same as pouring, but clicking the "decant" option instead of entering an amount). Proceed to step 3 using the test tube containing decanted liquid.
(c) If no white precipitate forms, proceed to step 3.
3. PRECIPITATION BY NaCl(aq)
(a) To a test tube that contains only liquid and no precipitate, add 2 mL of sodium chloride solution.
(b) If a white precipitate forms at the bottom of the test tube, decant the remaining liquid into another clean test tube and retain the precipitate. (Decanting is the same as pouring, but clicking the "decant" option instead of entering an amount). Proceed to step 4 using the test tube containing decanted liquid.
(c) If no white precipitate forms, proceed to step 4.
4. PRECIPITATION BY Na2SO4(aq)
(a) To a test tube that contains only liquid and no precipitate, add 2 mL of sodium sulfate solution.
(b) If a white precipitate forms at the bottom of the test tube, decant the remaining liquid into another clean test tube and retain the precipitate. (Decanting is the same as pouring, but clicking the "decant" option instead of entering an amount). Proceed to step 5.
(c) If no white precipitate forms, proceed to step 5.
5. You have completed the lab. Use your results to complete the assignment.
Question #1 :
1. Which ions did you determine to be present in the mystery solution?
2. Write the net ionic equations for the formation of the three possible precipitates formed in steps 2, 3 and 4.
3. Explain how you could use flame tests to verify identity of the precipitates formed in each step.
- Chemistry - DrBob222, Wednesday, August 11, 2010 at 1:54pm
See above response about what you don't understand.
- Chemistry - annonomus, Wednesday, August 11, 2010 at 2:04pm
I dont understand how to write the net ionic equations for the foration of the three possible precipitates formed in steps 2 3 and 4
im guessing for number 1 we are dealing with barium and siver for sure
and i dont understand 3 at all
Answer this Question
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