Chemistry, 08.07.2019 11:00 nhristov

If you have an aqueous solution that contains 1.5 moles of hcl, how many moles of ions are in the solution? (a) 1.0, (b) 1.5, (c) 2.0, (d) 2.5, (e) 3.if you have an aqueous solution that contains 1.5 moles of hcl, how many moles of ions are in the solution? (a) 1.0, (b) 1.5, (c) 2.0, (d) 2.5, (e) 3.

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The correct option is $\boxed{\left( {\text{e}} \right)}$ . The number of moles of ion in the solution is $\boxed{3\;{\text{moles}}}$

Further Explanation:

An acid is a substance that has the ability to donate ${{\text{H}}^+}$ ions or can accept electrons from the electron-rich species. The acids can be classified into two types as follows:

1. Strong acids

2. Weak acids

1. Strong acids:

The acids that undergo complete dissociation into its constituent ions when dissolved in water are known as strong acids. The pH value of strong acids is lower than pH value of weak acids. Examples of strong acids include HCl, ${\text{HN}}{{\text{O}}_3}$ and ${{\text{H}}_2}{\text{S}}{{\text{O}}_4}$ . The general dissociation reaction of a strong acid is as follows:

${\text{HA}}+{{\text{H}}_2}{\text{O}}\to {{\text{H}}_3}{{\text{O}}^+}+{{\text{A}}^-}$

Here, HA is a strong acid.

2. Weak acids:

The acids that undergo partial dissociation into its constituent ions when dissolved in water are known as weak acids. pH value of weak acids is higher than pH value of strong acids. Examples of weak acids include , ${\text{C}}{{\text{H}}_3}{\text{COOH}}$ , HCOOH and HCN. The general dissociation reaction of a weak acid is as follows:

${\text{HB}} + {{\text{H}}_2}{\text{O}} \rightleftharpoons {{\text{H}}_3}{{\text{O}}^+} + {{\text{B}}^ -}$

Here, HB is a weak acid.

HCl is a strong acid and therefore it dissociates completely into ${{\mathbf{H}}_{\mathbf{3}}}{{\mathbf{O}}^{\mathbf{+}}}$ and ${\mathbf{C}}{{\mathbf{l}}^-}$ ions. The dissociation reaction of HCl is as follows:

${\text{HCl}}\left( g \right) + {{\text{H}}_2}{\text{O}}\left( l \right) \to {{\text{H}}_3}{{\text{O}}^+}\left( {aq} \right) + {\text{C}}{{\text{l}}^-}\left( {aq} \right)$

The above chemical equation depicts that one mole of HCl dissociates to give one mole of ${{\text{H}}_{\text{3}}}{{\text{O}}^+}$ ion and one ${\text{C}}{{\text{l}}^-}$ mole of ion. Therefore 1.5 mol of HCl will dissociate to give 1.5 mol of ${{\text{H}}_{\text{3}}}{{\text{O}}^+}$ ions and 1.5 mol of ${\text{C}}{{\text{l}}^-}$ ions.

The total number of moles of ions released from 1.5 mol of HCl in the aqueous solution is the sum of ${{\text{H}}_{\text{3}}}{{\text{O}}^+}$ ions and ${\text{C}}{{\text{l}}^-}$ ions.

$\begin{gathered}{\text{Total moles of ions}} = {\text{ions of }}{{\text{H}}_{\text{3}}}{{\text{O}}^+} + {\text{ions of C}}{{\text{l}}^ - }\\= 1.5\;{\text{moles}} +1.5\;{\text{moles}} \\= {\text{3 moles}} \\ \end{gathered}$