Questions: dissolved in a liter of water. acid strong or weak? species present at (10^-6 mol/L) or greater when dissolved in water --- --- --- (mathrmH2 mathrmCO3) weak (mathrmH2 mathrm~S) weak (mathrmHClO2) weak HI strong

dissolved in a liter of water. acid strong or weak? species present at (10^-6 mol/L) or greater when dissolved in water --- --- --- (mathrmH2 mathrmCO3) weak (mathrmH2 mathrm~S) weak (mathrmHClO2) weak HI strong
Transcript text: dissolved in a liter of water. \begin{tabular}{|c|c|cc|} \hline acid & \begin{tabular}{c} strong or \\ weak? \end{tabular} & \begin{tabular}{c} species present at $\mathbf{1 0}^{-6} \mathbf{~ m o l / L}$ or greater \\ when dissolved in water \end{tabular} \\ \hline $\mathrm{H}_{2} \mathrm{CO}_{3}$ & weak & $\square$ \\ \hline $\mathrm{H}_{2} \mathrm{~S}$ & weak & $\square$ \\ \hline $\mathrm{HClO}_{2}$ & weak & $\square$ \\ \hline HI & strong & $\square$ \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Identify the Nature of Each Acid
  • Determine whether each acid is strong or weak based on the given information.
Step 2: Analyze Dissociation of Weak Acids
  • For weak acids (\(\mathrm{H}_{2} \mathrm{CO}_{3}\), \(\mathrm{H}_{2} \mathrm{S}\), \(\mathrm{HClO}_{2}\)), consider partial dissociation in water.
  • Identify the species present at concentrations of \(10^{-6} \, \text{mol/L}\) or greater, including the undissociated acid and its dissociation products.
Step 3: Analyze Dissociation of Strong Acids
  • For the strong acid (\(\mathrm{HI}\)), assume complete dissociation in water.
  • Identify the species present at concentrations of \(10^{-6} \, \text{mol/L}\) or greater, which will include the dissociated ions.

Final Answer

  • For \(\mathrm{H}_{2} \mathrm{CO}_{3}\): \(\text{HCO}_3^-, \text{CO}_3^{2-}\)
  • For \(\mathrm{H}_{2} \mathrm{S}\): \(\text{HS}^-, \text{S}^{2-}\)
  • For \(\mathrm{HClO}_{2}\): \(\text{ClO}_2^-, \text{HClO}_2\)
  • For \(\mathrm{HI}\): \(\text{H}^+, \text{I}^-\)
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