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.

Answers: 1

Show answers

Answers

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.

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

Hence, the correct option is (e).

Learn more:

1. The reason for the acidity of water

2. Reason for the acidic and basic nature of amino acid.

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Acids, bases, and salts

Keywords: Acid, bases, strong acids, pH , weak acids, electron-rich species, dissociation, moles of ions, HCl, H3O+, Cl-.

If you have an aqueous solution that contains 1.5 moles of hcl, how many moles of ions are in the so

Answer from: Quest

Ireally don’t know this

Answer from: Quest

Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbf₂(s) ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is $k_{sp} = [\text{pb}^{2+}][\text{f}^- ]^2 = 4 \times 10^{-8}$ (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as $q = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}}$ then, we can interpret q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product: $\begin{aligned} q & = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}} \\ & = (1.9 \times 10^{-3} ) (3.8\times 10^{3})^2 \\ & = 2.7 \times 10^{-8} \end{aligned}$ since q = 2.7 × 10⁻⁸ < ksp = 4 × 10⁻⁸, a precipitate will not form.

Another question on Chemistry

Chemistry, 21.06.2019 18:20

Part of molten rock at mid-ocean ridges

Answers: 1

Answer

Chemistry, 21.06.2019 20:30

In which layer of earth do most earthauakes occur a_ inner core b_outer core c_mantle d_crust

Answers: 1

Answer

Chemistry, 22.06.2019 02:30

Which element forms an ionic bond with flourine? 1) fluorine 2) carbon 3) potassium 4) oxygen

Answers: 1

Answer

Chemistry, 22.06.2019 16:50

Assuming complete dissociation of the solute, how many grams of kno3 must be added to 275 ml of water to produce a solution that freezes at -14.5 c? the freezing point for pure water is 0.0 c and k_f is equal to 1.86 c/m

Answers: 3

Answer

You know the right answer?

If you have an aqueous solution that contains 1.5 moles of hcl, how many moles of ions are in the so...

Questions