{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Experiment_13_-_Sample_Analysis

Experiment_13_-_Sample_Analysis - Chem istry 1B Experimen t...

Info icon This preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
Chemistry 1B Experiment 13 61
Image of page 1

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
62 Chemistry 1B Experiment 13 Sample Analysis. Precipitates and Complexes of Silver Ion Data for Determining Formulas Solutions containing NH 3 , CO 3 2– , Cl , I , PO 4 3– , and S 2 O 3 2– ions were added to equal proportions of a silver nitrate solution, which contained the complex ion Ag(H 2 O) 2 + . All of the added solutions were also clear and colorless. AgNO 3 ( aq ) by itself Colorless solution AgNO 3 ( aq ) with NH 3 ( aq ) Colorless solution AgNO 3 ( aq ) with Na 2 CO 3 ( aq ) Pale yellow precipitate AgNO 3 ( aq ) with NaCl ( aq ) White precipitate AgNO 3 ( aq ) with NaI ( aq ) Yellow precipitate AgNO 3 ( aq ) with Na 3 PO 4 ( aq ) Yellow precipitate AgNO 3 ( aq ) with Na 2 S 2 O 3 ( aq ) Colorless solution Formulas of Silver Complexes and Precipitates Ag + ions formed precipitates with CO 3 2– , Cl , I , and PO 4 3– ions. Solids are electrically neutral; the charges of all their ions add up to zero. Therefore, the formulas of these precipitates are: Ag 2 CO 3 , AgCl, AgI, and Ag 3 PO 4 . It is not obvious from these observations that Ag + ions formed soluble complex ions with NH 3 and S 2 O 3 2– ions. However, data on the next page shows that solutions containing NH 3 and S 2 O 3 2– ions were able to convert the pale yellow precipitate Ag 2 CO 3 into colorless solutions. Thus, complex ions more stable than Ag 2 CO 3 must have formed. Ag + has a coordination number of 2, so it binds to two ligands when it forms complex ions. The formulas of the complex ions formed with NH 3 and S 2 O 3 2– are therefore: Ag(NH 3 ) 2 + and Ag(S 2 O 3 ) 2 3– . The product-favored reactions that occurred when NH 3 ( aq ) and Na 2 S 2 O 3 ( aq ) solutions were added to Ag 2 CO 3 ( s ) were: Ag 2 CO 3 ( s ) + 2 NH 3 ( aq ) → 2 Ag(NH 3 ) 2 + ( aq ) + CO 3 2– ( aq ) Ag 2 CO 3 ( s ) + 2 S 2 O 3 2– ( aq ) → 2 Ag(S 2 O 3 ) 2 3– ( aq ) + CO 3 2– ( aq ) Ag(H 2 O) 2 + ( aq ) Colorless solution Ag(NH 3 ) 2 + ( aq ) Colorless solution Ag 2 CO 3 ( s ) Pale yellow precipitate AgCl ( s ) White precipitate AgI ( s ) Yellow precipitate Ag 3 PO 4 ( s ) Yellow precipitate Ag(S 2 O 3 ) 2 3– ( aq ) Colorless solution
Image of page 2
Chemistry 1B Experiment 13 63 Data for Determining Relative Stabilities
Image of page 3

Info icon This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 4
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern