Chemistry, 13.01.2020 12:31 mayachojnicki

Including all coefficients, charges, and phases, what is the correct net ionic equation for the following set of reactants? assume that the contribution of protons from h2so4 is near 100% . ba(oh)2(aq)+h2so4(aq)
express your answer as a chemical equation.

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Answer from: sydthekid25

The correct ionic equation that includes all the charges, phases, and coefficients is as follows:

$\boxed{{\text{B}}{{\text{a}}^{2+}}\left({aq}\right)+2{\text{O}}{{\text{H}}^-}\left({aq}\right)+2{{\text{H}}^+}\left({aq}\right)+{\text{S}}{{\text{O}}_4}^{2-}\left({aq}\right)\to{\text{BaS}}{{\text{O}}_4}\left(s\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(s\right)}$

Further explanation:

Double displacement reaction is defined as the reaction in which ions of two compound interchange with each other to form the product. For example, the general double displacement reaction between two compounds ${\text{AX}}$ and ${\text{BY}}$ is as follows:

${\text{AX}}+{\text{BY}}\to{\text{AY}}+{\text{BX}}$

The three types of equations that are employed to represent the chemical reaction are as follows:

1. Molecular equation

2. Total ionic equation

3. Net ionic equation

The molecular equation represents the reactants and products of the ionic reaction in dissociated form. In total ionic reaction, all the dissociated ions that are present in the reaction mixture are represented and in net ionic reaction, the useful ions that participate in the reaction are represented.

In first step, write the molecular equation for the reaction with the phases in bracket.

${\text{Ba}}{\left({{\text{OH}}}\right)_2}\left({aq}\right)+{{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_4}\left({aq}\right)\to{\text{BaS}}{{\text{O}}_4}\left(s\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(l\right)$

Note that parentheses indicate the state or the phase of the compound.

In second step, dissociate all the compounds with aqueous phase to write the total ionic equation and then cancel out the common ions on both sides to get the net ionic equation. The compounds with solid phase remain same.

The ionic species present in ${\text{Ba}}{\left({{\text{OH}}}\right)_2}$ is ${\text{B}}{{\text{a}}^{2+}}$ and ${\text{O}}{{\text{H}}^-}$ respectively. Similarly, the ionic species in ${{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_4}$ is $2{{\text{H}}^+}$ and ${\text{S}}{{\text{O}}_4}^{2-}$ respectively. Hence the net ionic equation can be represented as follows:

${\text{B}}{{\text{a}}^{2+}}\left({aq}\right)+2{\text{O}}{{\text{H}}^-}\left({aq}\right)+2{{\text{H}}^+}\left({aq}\right)+{\text{S}}{{\text{O}}_4}^{2-}\left({aq}\right)\to{\text{BaS}}{{\text{O}}_4}\left(s\right)+2{{\text{H}}_{\text{2}}}{\text{O}}\left(l\right)$

Learn more:

1. Component of John Dalton’s atomic theory:

2. Identification of all of the phases of the reaction:

Answer details:

Grade: High school

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: Chemical equation, Law of conservation of mass, phase, double displacement reactions, ionic equation, BaSO4, H2SO4.

Answer from: Quest

1. o2(g)as a product

Answer from: Quest

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