Questions: The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10^(-6) mol / L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10^(-6) mol/L or greater when dissolved in water HBrO3 strong HBr strong H3PO4 weak HNO2 weak

The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10^(-6) mol / L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10^(-6) mol/L or greater when dissolved in water HBrO3 strong HBr strong H3PO4 weak HNO2 weak
Transcript text: The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about $10^{-6} \mathrm{~mol} / \mathrm{L}$ when about a tenth of a mole of the acid is dissolved in a liter of water. \begin{tabular}{|c|c|c|} \hline acid & strong or weak? & \begin{tabular}{c} species present at $10^{-6}$ mol/L or greater \\ when dissolved in water \end{tabular} \\ \hline $\mathrm{HBrO}_{3}$ & strong & \\ \hline HBr & strong & \\ \hline $\mathrm{H}_{3} \mathrm{PO}_{4}$ & weak & \\ \hline $\mathrm{HNO}_{2}$ & weak & \\ \hline \end{tabular}
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Solution

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Solution Steps

Step 1: Understanding Strong and Weak Acids

Strong acids completely dissociate in water, meaning they break apart into their ions. Weak acids only partially dissociate, so both the acid and its ions are present in solution.

Step 2: Analyzing Strong Acids

For strong acids, the primary species present in solution are the ions resulting from complete dissociation.

  • HBrO\(_3\): As a strong acid, it dissociates completely into \(\text{H}^+\) and \(\text{BrO}_3^-\).
  • HBr: As a strong acid, it dissociates completely into \(\text{H}^+\) and \(\text{Br}^-\).
Step 3: Analyzing Weak Acids

For weak acids, both the undissociated acid and the ions from partial dissociation are present.

  • H\(_3\)PO\(_4\): As a weak acid, it partially dissociates. The species present are \(\text{H}_3\text{PO}_4\), \(\text{H}_2\text{PO}_4^-\), and \(\text{H}^+\).
  • HNO\(_2\): As a weak acid, it partially dissociates. The species present are \(\text{HNO}_2\), \(\text{NO}_2^-\), and \(\text{H}^+\).

Final Answer

\[ \begin{array}{|c|c|c|} \hline \text{acid} & \text{strong or weak?} & \text{species present at } 10^{-6} \text{ mol/L or greater} \\ \hline \mathrm{HBrO}_{3} & \text{strong} & \boxed{\text{H}^+, \text{BrO}_3^-} \\ \hline \mathrm{HBr} & \text{strong} & \boxed{\text{H}^+, \text{Br}^-} \\ \hline \mathrm{H}_{3} \mathrm{PO}_{4} & \text{weak} & \boxed{\text{H}_3\text{PO}_4, \text{H}_2\text{PO}_4^-, \text{H}^+} \\ \hline \mathrm{HNO}_{2} & \text{weak} & \boxed{\text{HNO}_2, \text{NO}_2^-, \text{H}^+} \\ \hline \end{array} \]

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