Questions: Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already: Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1 M aqueous solution ------ H2S 4 C6H5NH3+ (Choose one) HCOO- (Choose one) HS- (Choose one) HCOOH- H3O+ (Choose one) C6H5NH2 H2O 7

Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already: Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1 M aqueous solution ------ H2S 4 C6H5NH3+ (Choose one) HCOO- (Choose one) HS- (Choose one) HCOOH- H3O+ (Choose one) C6H5NH2 H2O 7
Transcript text: Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH . Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already: Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. \begin{tabular}{|c|c|} \hline species & \begin{tabular}{c} relative pH of \\ 0.1 M aqueous solution \end{tabular} \\ \hline $\mathrm{H}_{2} \mathrm{~S}$ & 4 \\ \hline $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}$ & (Choose one) $\mathbf{~}$ \\ \hline $\mathrm{HCOO}^{-}$ & (Choose one) $\mathbf{~}$ \\ \hline $\mathrm{HS}^{-}$ & (Choose one) $\mathbf{~}$ \\ \hline $\mathrm{HCOOH}^{-}$ & \\ \hline $\mathrm{H}_{3} \mathrm{O}^{+}$ & (Choose one) $\mathbf{~}$ \\ \hline $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$ & \\ \hline $\mathrm{H}_{2} \mathrm{O}$ & 7 \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Identify the pH of each species

To order the species by increasing pH, we need to determine whether each species is an acid, base, or neutral in water.

  • $\mathrm{H}_{2} \mathrm{~S}$: This is a weak acid. Given pH = 4.
  • $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}$: This is the conjugate acid of aniline, a weak base. Therefore, it is a weak acid.
  • $\mathrm{HCOO}^{-}$: This is the conjugate base of formic acid, a weak acid. Therefore, it is a weak base.
  • $\mathrm{HS}^{-}$: This is the conjugate base of $\mathrm{H}_{2} \mathrm{~S}$, a weak acid. Therefore, it is a weak base.
  • $\mathrm{HCOOH}$: This is formic acid, a weak acid.
  • $\mathrm{H}_{3} \mathrm{O}^{+}$: This is the hydronium ion, a strong acid.
  • $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$: This is aniline, a weak base.
  • $\mathrm{H}_{2} \mathrm{O}$: This is neutral with pH = 7.
Step 2: Rank the species by pH
  • $\mathrm{H}_{3} \mathrm{O}^{+}$: Strong acid, lowest pH.
  • $\mathrm{HCOOH}$: Weak acid, lower pH.
  • $\mathrm{H}_{2} \mathrm{~S}$: Weak acid, pH = 4.
  • $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}$: Weak acid, higher pH than $\mathrm{H}_{2} \mathrm{~S}$.
  • $\mathrm{H}_{2} \mathrm{O}$: Neutral, pH = 7.
  • $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$: Weak base, higher pH than water.
  • $\mathrm{HCOO}^{-}$: Weak base, higher pH than $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}$.
  • $\mathrm{HS}^{-}$: Weak base, highest pH.

Final Answer

\[ \begin{array}{|c|c|} \hline \text{species} & \text{relative pH of 0.1 M aqueous solution} \\ \hline \mathrm{H}_{3} \mathrm{O}^{+} & 1 \\ \hline \mathrm{HCOOH} & 2 \\ \hline \mathrm{H}_{2} \mathrm{~S} & 4 \\ \hline \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+} & 3 \\ \hline \mathrm{HCOO}^{-} & 7 \\ \hline \mathrm{HS}^{-} & 8 \\ \hline \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} & 6 \\ \hline \mathrm{H}_{2} \mathrm{O} & 5 \\ \hline \end{array} \]

\[ \boxed{ \begin{array}{|c|c|} \hline \mathrm{H}_{3} \mathrm{O}^{+} & 1 \\ \hline \mathrm{HCOOH} & 2 \\ \hline \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+} & 3 \\ \hline \mathrm{H}_{2} \mathrm{~S} & 4 \\ \hline \mathrm{H}_{2} \mathrm{O} & 5 \\ \hline \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2} & 6 \\ \hline \mathrm{HCOO}^{-} & 7 \\ \hline \mathrm{HS}^{-} & 8 \\ \hline \end{array} } \]

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