Metal sulfides are prepared by bubbling hydrogen sulfide gas, H, S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H, S, which occurs when [H, S] = 0.100 M, the equilibrium shown is established. H,S(aq) + 2 H,O1) = s²-(aq) + 2H,O*(aq) Keg = 1.1 x 10-20 An aqueous solution containing 0.0117 M Pb2+ and 0.0117 M Ag+ is saturated with H, S. Above what concentration of S2- will PbS precipitate? The Ksp of PbS is 8.9 x 10-29. [s²-] = M Above what concentration of S2- will Ag, S precipitate? The Kp of Ag, S is 3.3 x 10-50. [s²-] = M If the pH of the solution is adjusted to 2.73, which species will precipitate from the saturated H, S solution? neither species PbS both PbS and Ag,S Ag, S
Metal sulfides are prepared by bubbling hydrogen sulfide gas, H, S, through an aqueous solution containing the metal ion, and then adjusting the pH. When the solution is saturated with H, S, which occurs when [H, S] = 0.100 M, the equilibrium shown is established. H,S(aq) + 2 H,O1) = s²-(aq) + 2H,O*(aq) Keg = 1.1 x 10-20 An aqueous solution containing 0.0117 M Pb2+ and 0.0117 M Ag+ is saturated with H, S. Above what concentration of S2- will PbS precipitate? The Ksp of PbS is 8.9 x 10-29. [s²-] = M Above what concentration of S2- will Ag, S precipitate? The Kp of Ag, S is 3.3 x 10-50. [s²-] = M If the pH of the solution is adjusted to 2.73, which species will precipitate from the saturated H, S solution? neither species PbS both PbS and Ag,S Ag, S
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
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![### Metal Sulfide Precipitation and Equilibrium
Metal sulfides are created by introducing hydrogen sulfide gas, \( \text{H}_2\text{S} \), into an aqueous solution containing the metal ion and then adjusting the pH. When the solution reaches saturation with \( \text{H}_2\text{S} \) at a concentration of 0.100 M, the following equilibrium is established:
\[ \text{H}_2\text{S}(\text{aq}) + 2 \text{H}_2\text{O}(l) \rightleftharpoons \text{S}^{2-}(\text{aq}) + 2 \text{H}_3\text{O}^+(\text{aq}) \]
The equilibrium constant (\( K_{\text{eq}} \)) for this reaction is \( 1.1 \times 10^{-20} \).
#### Precipitation of Lead Sulfide (\( \text{PbS} \))
An aqueous solution containing 0.0117 M of \( \text{Pb}^{2+} \) and 0.0117 M of \( \text{Ag}^+ \) is saturated with \( \text{H}_2\text{S} \). The solubility product constant (\( K_{\text{sp}} \)) for \( \text{PbS} \) is \( 8.9 \times 10^{-29} \).
- **Determine the concentration of \( \text{S}^{2-} \) above which \( \text{PbS} \) will precipitate:**
\[ [\text{S}^{2-}] = \_\_\_\_\_\_\_ \text{ M} \]
#### Precipitation of Silver Sulfide (\( \text{Ag}_2\text{S} \))
The solubility product constant (\( K_{\text{sp}} \)) for \( \text{Ag}_2\text{S} \) is \( 3.3 \times 10^{-50} \).
- **Determine the concentration of \( \text{S}^{2-} \) above which \( \text{Ag}_2\text{S} \) will precipitate:**
\[ [\text{S}^{2-}] = \_\_\_\_\_\_\_ \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1d39eb1c-3154-4bee-b19a-a1be6277f6e8%2Fa3690418-7ce3-47ef-834a-f06d3bd45910%2Fsahuhy_processed.png&w=3840&q=75)
Transcribed Image Text:### Metal Sulfide Precipitation and Equilibrium
Metal sulfides are created by introducing hydrogen sulfide gas, \( \text{H}_2\text{S} \), into an aqueous solution containing the metal ion and then adjusting the pH. When the solution reaches saturation with \( \text{H}_2\text{S} \) at a concentration of 0.100 M, the following equilibrium is established:
\[ \text{H}_2\text{S}(\text{aq}) + 2 \text{H}_2\text{O}(l) \rightleftharpoons \text{S}^{2-}(\text{aq}) + 2 \text{H}_3\text{O}^+(\text{aq}) \]
The equilibrium constant (\( K_{\text{eq}} \)) for this reaction is \( 1.1 \times 10^{-20} \).
#### Precipitation of Lead Sulfide (\( \text{PbS} \))
An aqueous solution containing 0.0117 M of \( \text{Pb}^{2+} \) and 0.0117 M of \( \text{Ag}^+ \) is saturated with \( \text{H}_2\text{S} \). The solubility product constant (\( K_{\text{sp}} \)) for \( \text{PbS} \) is \( 8.9 \times 10^{-29} \).
- **Determine the concentration of \( \text{S}^{2-} \) above which \( \text{PbS} \) will precipitate:**
\[ [\text{S}^{2-}] = \_\_\_\_\_\_\_ \text{ M} \]
#### Precipitation of Silver Sulfide (\( \text{Ag}_2\text{S} \))
The solubility product constant (\( K_{\text{sp}} \)) for \( \text{Ag}_2\text{S} \) is \( 3.3 \times 10^{-50} \).
- **Determine the concentration of \( \text{S}^{2-} \) above which \( \text{Ag}_2\text{S} \) will precipitate:**
\[ [\text{S}^{2-}] = \_\_\_\_\_\_\_ \text
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