PRECIPITATION BY NaC2H3O2(aq)

Question

(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.

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.

Answer 1

This is not a question. It is a set of lab experiment instructions you should have followed. You need to perform the experiment and document your own results.