When an aqueous solution of H2 S(a q) is mixed with an aqueous solution of copper(II) sulfate,

step 1 We're asked to consider an aqueous solution of H2S with an aqueous solution of CO, copper 2 sulf

When an aqueous solution of H2 S(a q) is mixed with an...

When an aqueous solution of $\mathrm{H}_{2} \mathrm{~S}(a q)$ is mixed with an aqueous solution of copper(II) sulfate, a black precipitate of CuS forms. (a) Write and balance the full reaction equation for the reaction of $\mathrm{H}_{2} \mathrm{~S}(a q)$ with $\operatorname{CuSO}_{4}(a q)$. (b) Explain how your answer to (a) demonstrates that $\mathrm{H}_{2} \mathrm{~S}(a q)$ is an acid. (c) Write the net ionic equation for the formation of $\operatorname{CuS}(s)$

When an aqueous solution of $\mathrm{H}_{2} \mathrm{~S}(a q)$ is mixed with an aqueous solution of copper(II) sulfate, a black precipitate of CuS forms.
(a) Write and balance the full reaction equation for the reaction of $\mathrm{H}_{2} \mathrm{~S}(a q)$ with $\operatorname{CuSO}_{4}(a q)$.
(b) Explain how your answer to (a) demonstrates that $\mathrm{H}_{2} \mathrm{~S}(a q)$ is an acid.
(c) Write the net ionic equation for the formation of $\operatorname{CuS}(s)$

Key Concepts

Precipitation Reactions

A precipitation reaction occurs when two aqueous solutions combine and form an insoluble solid, known as the precipitate. In such reactions, specific ion pairs react to form a compound with low solubility, removing those ions from the solution. Understanding precipitation involves knowing solubility rules and the ability to differentiate between the ions that remain in solution and those that form the solid product.

Net Ionic Equations

Net ionic equations focus on the chemical species that undergo a change during a reaction, omitting the spectator ions that do not participate directly in the formation of the precipitate or any other reaction product. This simplification helps in understanding the actual chemical change that is taking place. Formulating a net ionic equation involves identifying which ions form the insoluble compound from the reaction.

Acid-Base Behavior

Acid-base behavior, particularly in the context of Bronsted-Lowry theory, describes an acid as a substance capable of donating a proton (H?) and a base as a substance that can accept a proton. In reactions where acid behavior is demonstrated, the acid donates its proton to a base, leading to the formation of a conjugate base and a conjugate acid. Recognizing H?S as an acid involves showing how it donates protons in a chemical reaction.

Balancing Chemical Equations

This concept involves ensuring that the number of atoms of each element and the charge is conserved in a chemical reaction. It is a fundamental principle in chemistry that reflects the conservation of mass and charge, requiring that the same number of atoms for each element appear on both sides of the chemical equation. Balancing equations is a key step when writing both full and net ionic equations in reactions.

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