How would you analyze a solution known to contain Hg22+ and Cu2+?
depends on what you mean "analyze".
Mercury I chloride is not soluble in water, whereas cupric chloride is.
calculate the specific rate constant
A] (mol/L) [B] (mol/L) Rate of appearance of C (mol/L-hr)
1.0 ×10^-2 1.0 0.30×10^−6
1.0 ×10^−2 3.0 8.10×10^−6
2.0 ×10^−2 3.0 3.24×10^−5
2.0 ×10^−2 1.0 1.20×10^−6
3.0 ×10^−2 3.0 7.30×10^−5
It looks like the rate equation is
rate = k[A]2[B]3 but the numbers are so scrunched it's difficult to make them out. You would do well to space them and the easy way to do that is with periods; i.e.,
1.0E-2...1.0...0.3E-6 etc.
To find k, use any trial, plug the concns of A and B into the rate equation I wrote and calculate k.
To analyze a solution known to contain Hg2^2+ and Cu^2+ ions, you would typically perform a series of qualitative tests and confirmatory tests. These tests can help you identify the presence of these ions and differentiate between them. Here is a step-by-step process to analyze the solution:
1. Preliminary Observation: Begin by examining the solution's physical characteristics, such as color, transparency, and any precipitates or sediments present. This initial observation can provide some clues about the nature of the ions present.
2. pH test: Determine the pH of the solution using a pH indicator or pH meter. The pH can give insight into the potential presence of certain ions or compounds.
3. Qualitative tests for Copper (Cu^2+):
a. Add a few drops of 6 M sodium hydroxide (NaOH) to a small portion of the solution. If a blue precipitate is formed, it confirms the presence of Cu^2+ ions. Copper hydroxide (Cu(OH)2) is insoluble in water and appears as a blue solid.
4. Qualitative tests for Mercury (Hg2^2+):
a. Add a few drops of aqueous solution of potassium iodide (KI) to a small portion of the solution. If a yellow precipitate forms, it suggests the presence of Hg2^2+ ions. The yellow precipitate indicates the formation of mercury(II) iodide (HgI2), which is insoluble in water.
b. Additionally, mercury(II) ions can also be identified using the Luminous flame test. Take a platinum or nichrome wire and dip it into the solution. Then, hold the wire in a Bunsen burner or gas flame. If the flame exhibits a bluish-green color, it suggests the presence of Hg2^2+ ions.
5. Confirmatory tests:
a. To confirm the presence of Cu^2+ ions, perform the Sodium Potassium Tartrate (SPT) test. To a small portion of the solution, add sodium potassium tartrate and sodium hydroxide. The formation of a deep blue color complex known as the "Schiff's Reagent" indicates the presence of copper(II) ions.
b. To confirm the presence of Hg2^2+ ions, perform the Stannous Chloride (SnCl2) test. Add a few drops of stannous chloride solution to a small portion of the solution. A white precipitate of mercury(I) chloride (Hg2Cl2) confirms the presence of Hg2^2+ ions.
It is important to note that these tests are indicative but not conclusive. Interpret the results carefully, and it is always advisable to consult relevant literature or consult with an analytical chemist if required.