Silver tarnish is mainly \(\mathrm{Ag}_{2} \mathrm{S}\) : $$\begin{array}{r}\mathrm{Ag}_{2} \mathrm{S}(\mathrm{s})+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{Ag}(\mathrm{s})+\mathrm{S}^{2-}(\mathrm{aq}) \\\E^{\circ}=-0.691 \mathrm{V}\end{array}$$ A tarnished silver spoon is placed in contact with a commercially available metallic product in a glass baking dish. Boiling water, to which some \(\mathrm{NaHCO}_{3}\) has been added, is poured into the dish, and the product and spoon are completely covered. Within a short time, the removal of tarnish from the spoon begins. (a) What metal or metals are in the product? (b) What is the probable reaction that occurs? (c) What do you suppose is the function of the \(\mathrm{NaHCO}_{3} ?\) (d) An advertisement for the product appears to make two claims: (1) No chemicals are involved, and (2) the product will never need to be replaced. How valid are these claims? Explain.

In the context of silver tarnish removal, a redox reaction—short for reduction-oxidation reaction—is the chemical process at play. Redox reactions are a type of chemical reaction where electrons are transferred between two substances. During this transfer, one substance is oxidized (loss of electrons) and another is reduced (gain of electrons).For a tarnished silver spoon, the tarnish is a layer of silver sulfide \( \mathrm{Ag}_2 \mathrm{S} \). The redox reaction involves the reduction of silver sulfide back to silver metal. A metal, likely aluminum in this case, gets oxidized, thereby donating electrons that transform the silver sulfide (reductant) into elemental silver (reducing agent).Understanding these reactions helps explain why certain home remedies, like lining a container with aluminum foil and adding boiling water and baking soda, can remove tarnish. The aluminum foil undergoes oxidation, and in exchange, the silver sulfide reduces to silver, restoring the shine to the silver object. Considering this, the claim of 'no chemicals involved' in such a process is incorrect as the aluminum, water, and baking soda are all chemicals participating in the redox reaction.

Chemical reactions are not just confined to laboratory settings; they are a part of our day-to-day lives. For example, when a silver spoon becomes tarnished over time, it's due to a chemical reaction between silver and sulfur-containing substances in the air, leading to the formation of silver sulfide.In a redox reaction for tarnish removal, everyday materials can facilitate the reaction. Baking soda \(\mathrm{NaHCO}_{3}\), a common household chemical, is often used as an electrolyte to create a conductive solution, which can assist in the transfer of electrons necessary for the redox reaction between the aluminum and the silver sulfide tarnish.Even the digestion of food in our bodies involves chemical reactions. When products are marketed as not using chemicals, it's a misconception—even the air we breathe and the water we drink are composed of chemicals. Thus, educating oneself on the basics of chemistry can help navigate through marketing claims and understand the science behind common household processes.

The electrochemical series, also known as the activity series, is a list of metals arranged according to their standard electrode potentials. A metal’s position in the series predicts its ability to be oxidized or reduced. Metals higher in the series, like aluminum, are more likely to be oxidized and hence are more reactive than those lower in the series, such as silver.In the exercise, when a tarnished silver spoon is placed in contact with a reactive metal and immersed in a boiling baking soda solution, it's the relative positions of these metals in the electrochemical series that determine the direction of the redox reaction. Aluminum, being higher than silver in the series, donates electrons to the silver ions in the tarnish, causing the silver ions to become reduced to elemental silver.The electrochemical series also explains the claim that the product, likely composed of aluminum, will never need to be replaced. While aluminum can theoretically be used multiple times, it will eventually be consumed through continuous reactions. However, due to its low cost and abundant nature, aluminum is often considered a disposable reagent in this process.