Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C is red. In the reactions in which they participate, they are reduced to A−, B−, and C− ions, all of which are colorless. You are given an unknown, colorless, solution that contains one of the following salts: NaA, NaB, NaC. In solution, each salt dissociates completely into the Na+ ion and the anion A−, B−, or C−. The Na+ ion is effectively inert. You are given the availability of solutions of A, B, and C, develop a simple procedure for identifying the salt that is present in your unknown.   Question 6 options:   React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a better oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown.   React your unknown with NaA, NaB and NaC respectively. If a reaction occurs, your unknown is a worse oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown.   React your unknown with A, B and C respectively. If a reaction occurs, your unknown is a worse oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown.   React your unknown with A, B and C respectively. If a reaction occurs, your unknown is a better oxidizing agent than what you reacted it with. Use the oxidation strength order calculated in the previous question to determine your unknown.

Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --

During the demonstration, before each metal was added to the water, a drop of an acid-base indicator, phenolphthalein, was added to the water to monitor the reaction. What color was the water prior to the addition of the metal?

Write a balanced redox reaction for the reaction shown below.   Cr(s) │ Cr+3 (aq) ║ Fe+2(aq) │ Fe(s)

Identify the oxidizing agent, element oxidized, reducing agent and element reduced from the following line notation. Fe(s)||FeBr2(aq)||||NaBr(aq)||Br2(l)||Pt(s)

Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C is red. In the reactions in which they participate, they are reduced to A minus, B minus, and C minus ions, all of which are colorless. You are given an unknown, colorless, solution that contains one of the following salts: N a A, N a B, N a C. In solution, each salt dissociates completely into the Na+ ion and the anion A minus, B minus, or C minus. The N a + ion is effectively inert. You are given the availability of solutions of A, B, and C, develop a simple procedure for identifying the salt that is present in your unknown. Hint: For X2 + 2 Y 1 minus --->  Y2 + 2 X 1 minus   If a reaction occurs, X is more active than Y. If a reaction does not occur, Y is more active than X.   Question options:   React your unknown with A, B and C respectively. If a reaction occurs, your unknown is less active than what you reacted it with.    React your unknown with N a…

how many electrons are transferred in the following reaction (reaction is unbalanaced) Mg(s) + Al^3+(aq) --> Al(s) + Mg^2+(aq)

In a particular redox reaction, NO−2 is oxidized to NO3− and Cu2+ is reduced to Cu+. Complete and balance the equation for this reaction in acidic solution. Phases are optional.

For a particular redox reaction, BrO−  is oxidized to  BrO−3 and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in a BASIC SOLUTION. Phases are optional.   BrO−+ Ag+ + OH- -⟶BrO−3 + Ag + H2O