Question

some chemical compounds are listed in the first column of the table below. each compound is soluble in water.
imagine that a few tenths of a mole of each compound is dissolved in a liter of water. the important chemical species that would be present in this solution are
written in the second column of the table. use the checkboxes to classify each compound

Explanation:

• For \(CH_3NH_2\):
• It is a molecular compound.
• It is a weak base as it partially dissociates in water (\(CH_3NH_2 + H_2O

ightleftharpoons CH_3NH_3^++OH^-\)) and the important species present (\(CH_3NH_3^+\), \(OH^-\), \(CH_3NH_2\), \(H_2O\)) show partial ionization.

• For \(HC_2H_3O_2\):
• It is a molecular compound.
• It is a weak acid as it partially dissociates in water (\(HC_2H_3O_2 + H_2O

ightleftharpoons H_3O^++C_2H_3O_2^-\)) and the important species present (\(H_3O^+\), \(C_2H_3O_2^-\), \(HC_2H_3O_2\), \(H_2O\)) show partial ionization.

• For \(HBrO_3\):
• It is a molecular compound.
• It is a strong acid as it completely dissociates in water (\(HBrO_3 + H_2O = H_3O^++BrO_3^-\)) and the important species present (\(H_3O^+\), \(BrO_3^-\), \(H_2O\)) show complete ionization.
• For \(NaBrO_3\):
• It is an ionic compound (composed of \(Na^+\) and \(BrO_3^-\) ions).
• It is neither an acid nor a base in terms of the given acid - base categories. It is a salt that dissociates completely in water (\(NaBrO_3=Na^++BrO_3^-\)).

Answer:

• \(CH_3NH_2\): molecular, weak base
• \(HC_2H_3O_2\): molecular, weak acid
• \(HBrO_3\): molecular, strong acid
• \(NaBrO_3\): ionic