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Chapter 34: Problem 71

The ion that cannot be precipitated by both \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{~S}\) is (a) \(\mathrm{Ag}^{+}\) (b) \(\mathrm{Cu}^{+}\) (c) \(\mathrm{Sn}^{2+}\) (d) \(\mathrm{Pb}^{2+}\)

Short Answer

Expert verified
The ion that cannot be precipitated by both HCl and H鈧係 is Sn虏鈦�.

Step by step solution

01

Understanding precipitation with HCl

Analyze which ions can form insoluble chlorides with the addition of hydrochloric acid (HCl). - When HCl is added, ions that form insoluble chlorides and get precipitated include silver ion (Ag鈦�) and lead ion (Pb虏鈦�) as they form silver chloride (AgCl) and lead chloride (PbCl鈧�), respectively. Cu鈦� can also form a precipitate as cuprous chloride (CuCl). Tin ion (Sn虏鈦�) does not form a precipitate with HCl.
02

Analyzing precipitation with H2S

Determine which ions form sulfides that are insoluble in dilute HCl when hydrogen sulfide (H鈧係) is bubbled through a solution. - In acidic conditions, H鈧係 will precipitate metal ions as metal sulfides. Ag鈦� and Cu鈦� can be precipitated as Ag鈧係 and Cu鈧係, respectively. Pb虏鈦� can also form lead sulfide (PbS) which is insoluble. Sn虏鈦� gets precipitated as stannous sulfide (SnS) in acidic solutions.
03

Final analysis and conclusion

Combine the analysis from the first two steps to find the ion that cannot be precipitated by both methods. - From the analysis, Ag鈦� and Pb虏鈦� are precipitated by both HCl and H鈧係. Cu鈦� is also precipitated by both reagents. Sn虏鈦�, however, does not precipitate with HCl, even though it does with H鈧係.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Precipitation Reactions
Precipitation reactions are a type of chemical reaction where soluble ions in different solutions are mixed to form an insoluble compound known as a precipitate. When studying precipitation reactions, it is critical to understand which ions can combine to form these insoluble compounds.
In our specific problem, the ions tested against different reagents include silver ion (Ag鈦�), cuprous ion (Cu鈦�), tin ion (Sn虏鈦�), and lead ion (Pb虏鈦�). When hydrochloric acid (HCl) is added in these cases:
  • Ag鈦� forms a precipitate as silver chloride (AgCl).
  • Cu鈦� forms a precipitate as cuprous chloride (CuCl).
  • Pb虏鈦� forms a precipitate as lead chloride (PbCl鈧�).
  • Sn虏鈦� does not form a precipitate.
When hydrogen sulfide (H鈧係) is used in acidic conditions, each of these ions undergo different reactions to form sulfides:
  • Ag鈦� forms silver sulfide (Ag鈧係).
  • Cu鈦� forms cuprous sulfide (Cu鈧係).
  • Pb虏鈦� forms lead sulfide (PbS).
  • Sn虏鈦� forms stannous sulfide (SnS).
Understanding these reactions helps determine the solubility and stability of ions in different chemical settings.
Metal Ions
Metal ions are positively charged atoms that may participate in chemical reactions by forming various compounds. The charge on these ions, denoted by the symbols like Ag鈦�, Cu鈦�, Sn虏鈦�, and Pb虏鈦�, determines their reactivity and the types of compounds they will form in both acidic and neutral environments.
The behavior of metal ions in precipitation reactions can be predicted by considering their interactions with other ions:
  • Ag鈦� is known for forming insoluble salts such as AgCl and Ag鈧係.
  • Cu鈦� is somewhat less common but also forms less soluble compounds like CuCl and Cu鈧係.
  • Sn虏鈦�, though reactive, is unique because it does not precipitate with HCl, but does with sulfide ions.
  • Pb虏鈦� creates insoluble precipitates such as PbCl鈧� and PbS, even in dilute solutions.
Knowledge about metal ions and their specific reactions is crucial in predicting outcomes of precipitation reactions and understanding their occurrence in chemical analysis.
Chemical Analysis
Chemical analysis involves a variety of techniques and methods to determine the composition of substances. Precipitation reactions play a significant role in qualitative chemical analysis by helping to identify the presence of specific ions in solution.
Through controlled chemical reactions, such as those observed with HCl and H鈧係 in our problem, chemists can isolate and identify unknown ionic species. In a laboratory setting, precipitation is often used to:
  • Test for specific ions by observing the formation of a precipitate.
  • Separate ions based on their reactivity and formation of insoluble products.
  • Confirm the identity of ions by comparing the observed precipitate with known reactions.
By understanding the solubility rules and reactivity characteristics of different metal ions, chemists can effectively use precipitation as a diagnostic tool. This enhances the precision and accuracy of chemical analysis in both research and applied chemistry contexts.

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Most popular questions from this chapter

Which of the following compounds on reaction with \(\mathrm{NaOH}\) and \(\mathrm{Na}_{2} \mathrm{O}_{2}\) gives yellow colour? (a) \(\mathrm{Zn}(\mathrm{OH})_{2}\) (b) \(\mathrm{Cr}(\mathrm{OH})_{3}\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}\) (d) none of these

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