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To complete the table, we need to identify each acid as either strong or weak and list the species present at concentrations greater than [tex]\(10^{-6}\)[/tex] mol/L when approximately a tenth of a mole of the acid is dissolved in a liter of water.
Here’s the detailed solution:
1. HIO[tex]\(_3\)[/tex] (Iodic acid)
- Strong or Weak?: Strong Acid
- Explanation: Strong acids dissociate completely in water.
- Dissociation: [tex]\( \text{HIO}_3 \rightarrow \text{H}^+ + \text{IO}_3^- \)[/tex]
- Species present:
- HIO[tex]\(_3\)[/tex] (remaining undissociated)
- H[tex]\(^+\)[/tex]
- IO[tex]\(_3^-\)[/tex]
2. H[tex]\(_2\)[/tex]S (Hydrosulfuric acid or Hydrogen sulfide)
- Strong or Weak?: Weak Acid
- Explanation: Weak acids only partially dissociate in water.
- Dissociation: [tex]\( \text{H}_2\text{S} \rightleftharpoons \text{H}^+ + \text{HS}^- \rightleftharpoons \text{H}^+ + \text{S}^{2-} \)[/tex]
- Species present:
- H[tex]\(_2\)[/tex]S
- H[tex]\(^+\)[/tex]
- HS[tex]\(^{-}\)[/tex]
- S[tex]\(^2{}^{-}\)[/tex]
3. H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex] (Sulfurous acid)
- Strong or Weak?: Weak Acid
- Explanation: Weak acids only partially dissociate in water.
- Dissociation: [tex]\( \text{H}_2\text{SO}_3 \rightleftharpoons \text{H}^+ + \text{HSO}_3^- \rightleftharpoons \text{H}^+ + \text{SO}_3^{2-} \)[/tex]
- Species present:
- H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex]
- H[tex]\(^+\)[/tex]
- HSO[tex]\(_3^-\)[/tex]
- SO[tex]\(_3^{2-}\)[/tex]
4. HI (Hydroiodic acid)
- Strong or Weak?: Strong Acid
- Explanation: Strong acids dissociate completely in water.
- Dissociation: [tex]\( \text{HI} \rightarrow \text{H}^+ + \text{I}^- \)[/tex]
- Species present:
- HI (remaining undissociated)
- H[tex]\(^+\)[/tex]
- I[tex]\(^{-}\)[/tex]
Now, we can fill in the table:
\begin{tabular}{|c|c|c|}
\hline
acid & \begin{tabular}{c}
strong or \\
weak?
\end{tabular} & \begin{tabular}{c}
species present at [tex]$10^{-6}$[/tex] mol/L or greater \\
when dissolved in water
\end{tabular} \\
\hline
HIO[tex]\(_3\)[/tex] & strong & HIO[tex]\(_3\)[/tex], H[tex]\(^+\)[/tex], IO[tex]\(_3^{-}\)[/tex] \\
\hline
H[tex]\(_2\)[/tex]S & weak & H[tex]\(_2\)[/tex]S, H[tex]\(^+\)[/tex], HS[tex]\(^-\)[/tex], S[tex]\(^2{}^{-}\)[/tex] \\
\hline
H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex] & weak & H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex], H[tex]\(^+\)[/tex], HSO[tex]\(_3^{-}\)[/tex], SO[tex]\(_3^{2-}\)[/tex] \\
\hline
HI & strong & HI, H[tex]\(^+\)[/tex], I[tex]\(^{-}\)[/tex] \\
\hline
\end{tabular}
This table now correctly lists each acid as strong or weak and enumerates the species present at significant concentrations when dissolved in water.
Here’s the detailed solution:
1. HIO[tex]\(_3\)[/tex] (Iodic acid)
- Strong or Weak?: Strong Acid
- Explanation: Strong acids dissociate completely in water.
- Dissociation: [tex]\( \text{HIO}_3 \rightarrow \text{H}^+ + \text{IO}_3^- \)[/tex]
- Species present:
- HIO[tex]\(_3\)[/tex] (remaining undissociated)
- H[tex]\(^+\)[/tex]
- IO[tex]\(_3^-\)[/tex]
2. H[tex]\(_2\)[/tex]S (Hydrosulfuric acid or Hydrogen sulfide)
- Strong or Weak?: Weak Acid
- Explanation: Weak acids only partially dissociate in water.
- Dissociation: [tex]\( \text{H}_2\text{S} \rightleftharpoons \text{H}^+ + \text{HS}^- \rightleftharpoons \text{H}^+ + \text{S}^{2-} \)[/tex]
- Species present:
- H[tex]\(_2\)[/tex]S
- H[tex]\(^+\)[/tex]
- HS[tex]\(^{-}\)[/tex]
- S[tex]\(^2{}^{-}\)[/tex]
3. H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex] (Sulfurous acid)
- Strong or Weak?: Weak Acid
- Explanation: Weak acids only partially dissociate in water.
- Dissociation: [tex]\( \text{H}_2\text{SO}_3 \rightleftharpoons \text{H}^+ + \text{HSO}_3^- \rightleftharpoons \text{H}^+ + \text{SO}_3^{2-} \)[/tex]
- Species present:
- H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex]
- H[tex]\(^+\)[/tex]
- HSO[tex]\(_3^-\)[/tex]
- SO[tex]\(_3^{2-}\)[/tex]
4. HI (Hydroiodic acid)
- Strong or Weak?: Strong Acid
- Explanation: Strong acids dissociate completely in water.
- Dissociation: [tex]\( \text{HI} \rightarrow \text{H}^+ + \text{I}^- \)[/tex]
- Species present:
- HI (remaining undissociated)
- H[tex]\(^+\)[/tex]
- I[tex]\(^{-}\)[/tex]
Now, we can fill in the table:
\begin{tabular}{|c|c|c|}
\hline
acid & \begin{tabular}{c}
strong or \\
weak?
\end{tabular} & \begin{tabular}{c}
species present at [tex]$10^{-6}$[/tex] mol/L or greater \\
when dissolved in water
\end{tabular} \\
\hline
HIO[tex]\(_3\)[/tex] & strong & HIO[tex]\(_3\)[/tex], H[tex]\(^+\)[/tex], IO[tex]\(_3^{-}\)[/tex] \\
\hline
H[tex]\(_2\)[/tex]S & weak & H[tex]\(_2\)[/tex]S, H[tex]\(^+\)[/tex], HS[tex]\(^-\)[/tex], S[tex]\(^2{}^{-}\)[/tex] \\
\hline
H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex] & weak & H[tex]\(_2\)[/tex]SO[tex]\(_3\)[/tex], H[tex]\(^+\)[/tex], HSO[tex]\(_3^{-}\)[/tex], SO[tex]\(_3^{2-}\)[/tex] \\
\hline
HI & strong & HI, H[tex]\(^+\)[/tex], I[tex]\(^{-}\)[/tex] \\
\hline
\end{tabular}
This table now correctly lists each acid as strong or weak and enumerates the species present at significant concentrations when dissolved in water.
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