You have been given an unknown that contains a Group I ion (Ag+ or Hg22+), a Group II ion (Fe2+ or Mn2+) and a Group III ion (Cu2+ or Ni2+). First you place 5 drops in a test tube and add 3 drops of 3 M HCl. You see a white precipitate. Next you add 1mL of 6 M NH3. The precipitate turns a little gray, but you are unsure if it is gray or white. You run some tests to confirm and believe it is gray. 1. What test did you run to confirm the precipitate is gray and what is the identity of the Group I ion (use complete sentences and type your answer in the space below)? Next, you place 5 mL of fresh unknown in a test tube and add 5 mL of HCl (and again see a white precipitate. 2. How do you separate the white precipitate, so that you can test the ions in the solution that aren’t precipitated (use complete sentences and type your answer in the space below)? Now you have separated the solution from the precipitate. You discard the precipitate and need to test the solution for Groups II and III ions. 3. What is the next step to separate the Group II and Group III ions (use complete sentences and type your answer in the space below)? You have separated the Group II and Group III ions (using your explanation in #3 above)into two test tubes. In the test tube containing the Group II ions, you add 1 M NaOH and see a dark precipitate. 4. How do you test this precipitate for Group II ion (use complete sentences and type your answer in the space below)? When you are done with your Group II tests, you have a purple solution. 5. Explain the identity of the Group II ion and how you came to this conclusion (use complete sentences and type your answer in the space below). Now you return to the test tube containing Group III ions. After testing, you have a pink precipitate. 6. Explain the identity of the Group III ion and how you came to this conclusion (use complete sentences and type your answer in the space below).

You have been given an unknown that contains a Group I ion (Ag+ or Hg22+), a Group II ion (Fe2+ or Mn2+) and a Group III ion (Cu2+ or Ni2+). First you place 5 drops in a test tube and add 3 drops of 3 M HCl. You see a white precipitate. Next you add 1mL of 6 M NH3. The precipitate turns a little gray, but you are unsure if it is gray or white. You run some tests to confirm and believe it is gray. 1. What test did you run to confirm the precipitate is gray and what is the identity of the Group I ion (use complete sentences and type your answer in the space below)? Next, you place 5 mL of fresh unknown in a test tube and add 5 mL of HCl (and again see a white precipitate. 2. How do you separate the white precipitate, so that you can test the ions in the solution that aren’t precipitated (use complete sentences and type your answer in the space below)? Now you have separated the solution from the precipitate. You discard the precipitate and need to test the solution for Groups II and III ions. 3. What is the next step to separate the Group II and Group III ions (use complete sentences and type your answer in the space below)? You have separated the Group II and Group III ions (using your explanation in #3 above)into two test tubes. In the test tube containing the Group II ions, you add 1 M NaOH and see a dark precipitate. 4. How do you test this precipitate for Group II ion (use complete sentences and type your answer in the space below)? When you are done with your Group II tests, you have a purple solution. 5. Explain the identity of the Group II ion and how you came to this conclusion (use complete sentences and type your answer in the space below). Now you return to the test tube containing Group III ions. After testing, you have a pink precipitate. 6. Explain the identity of the Group III ion and how you came to this conclusion (use complete sentences and type your answer in the space below).

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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You have been given an unknown that contains a Group I ion (Ag+ or Hg22+), a Group II ion (Fe2+ or Mn2+) and a Group III ion (Cu2+ or Ni2+).

First you place 5 drops in a test tube and add 3 drops of 3 M HCl. You see a white precipitate.

Next you add 1mL of 6 M NH3. The precipitate turns a little gray, but you are unsure if it is gray or white. You run some tests to confirm and believe it is gray.

1. What test did you run to confirm the precipitate is gray and what is the identity of the Group I ion (use complete sentences and type your answer in the space below)?

Next, you place 5 mL of fresh unknown in a test tube and add 5 mL of HCl (and again see a white precipitate.

2. How do you separate the white precipitate, so that you can test the ions in the solution that aren’t precipitated (use complete sentences and type your answer in the space below)?

Now you have separated the solution from the precipitate. You discard the precipitate and need to test the solution for Groups II and III ions.

3. What is the next step to separate the Group II and Group III ions (use complete sentences and type your answer in the space below)?

You have separated the Group II and Group III ions (using your explanation in #3 above)into two test tubes. In the test tube containing the Group II ions, you add 1 M NaOH and see a dark precipitate.

4. How do you test this precipitate for Group II ion (use complete sentences and type your answer in the space below)?

When you are done with your Group II tests, you have a purple solution.

5. Explain the identity of the Group II ion and how you came to this conclusion (use complete sentences and type your answer in the space below).

Now you return to the test tube containing Group III ions. After testing, you have a pink precipitate.

6. Explain the identity of the Group III ion and how you came to this conclusion (use complete sentences and type your answer in the space below).

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