Question

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 hclo_2 weak hi strong hbro_4 strong h_2s weak

Explanation:

Step1: Analyze weak acid \(HClO_{2}\)

Weak acids partially dissociate in water. The dissociation equation for \(HClO_{2}\) is \(HClO_{2}(aq)
ightleftharpoons H^{+}(aq)+ClO_{2}^{-}(aq)\), and water is also present (\(H_{2}O(l)\)). So the species are \(HClO_{2},H^{+},ClO_{2}^{-},H_{2}O\).

Step2: Analyze strong acid \(HI\)

Strong acids completely dissociate in water. The dissociation equation for \(HI\) is \(HI(aq)
ightarrow H^{+}(aq)+I^{-}(aq)\), and water is present (\(H_{2}O(l)\)). So the species are \(H^{+},I^{-},H_{2}O\).

Step3: Analyze strong acid \(HBrO_{4}\)

Strong acids completely dissociate in water. The dissociation equation for \(HBrO_{4}\) is \(HBrO_{4}(aq)
ightarrow H^{+}(aq)+BrO_{4}^{-}(aq)\), and water is present (\(H_{2}O(l)\)). So the species are \(H^{+},BrO_{4}^{-},H_{2}O\).

Step4: Analyze weak acid \(H_{2}S\)

Weak acids partially dissociate in water. The first - stage dissociation equation for \(H_{2}S\) is \(H_{2}S(aq)
ightleftharpoons H^{+}(aq)+HS^{-}(aq)\), and water is present (\(H_{2}O(l)\)). So the species are \(H_{2}S,H^{+},HS^{-},H_{2}O\).

Answer:

acid	strong or weak?	species present at \(10^{-6}\ mol/L\) or greater when dissolved in water
\(HI\)	strong	\(H^{+},I^{-},H_{2}O\)
\(HBrO_{4}\)	strong	\(H^{+},BrO_{4}^{-},H_{2}O\)
\(H_{2}S\)	weak	\(H_{2}S,H^{+},HS^{-},H_{2}O\)