The equation that shows [tex]{\text{M}}{{\text{n}}^{3 + }}[/tex] acts as the acid is
[tex]\boxed{{{\left[{{\text{Mn}}{{\left({{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]}^{3 + }}+{{\text{H}}_2}{\text{O}}\to{{\left[ {{\text{MnOH}}{{\left({{{\text{H}}_2}{\text{O}}} \right)}_5}}\right]}^{2 + }}{{\text{H}}_3}{{\text{O}}^ + }}[/tex]
Further Explanation:
Acids and bases can be defined in many ways based on different theories, which are as follows:
1. Arrhenius theory: According to this theory, acid is defined as the one which produces hydrogen or hydronium ions in a solution, while the base is defined as the one which produces hydroxide ions in a solution. Examples of Arrhenius acids include HBr, [tex]{\text{HN}}{{\text{O}}_3}[/tex] and [tex]{{\text{H}}_2}{\text{S}}{{\text{O}}_4}[/tex] while NaOH and KOH are examples of Arrhenius bases.
2. Bronsted-Lowry theory: According to this theory, the acid in the reaction donates a proton while a base is one that accepts a proton. HCl acts as Bronsted acid while [tex]{\text{N}}{{\text{H}}_3}[/tex] is a Bronsted base.
3. Lewis theory: According to this theory, an acid accepts a pair of electrons to electron-rich species while a base donates electrons to electron-deficient species in the reaction. Examples of Lewis acids are [tex]{\text{B}}{{\text{F}}_3}[/tex] , [tex]{\text{S}}{{\text{O}}_3}[/tex] while [tex]{{\text{H}}_2}{\text{O}}[/tex] and ROH are the examples of Lewis base.
The equation to show the acidic nature of [tex]{\mathbf{M}}{{\mathbf{n}}^{{\mathbf{3 + }}}}[/tex] is as follows:
[tex]{\left[ {{\text{Mn}}{{\left({{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]^{3 + }}+{{\text{H}}_2}{\text{O}}\to {\left[{{\text{MnOH}}{{\left( {{{\text{H}}_2}{\text{O}}}\right)}_5}} \right]^{2+}}+{{\text{H}}_3}{{\text{O}}^+}[/tex]
Here, [tex]{\text{M}}{{\text{n}}^{3 + }}[/tex] exists as [tex]{\left[{{\text{Mn}}{{\left( {{{\text{H}}_2}{\text{O}}}\right)}_6}}\right]^{3 + }}[/tex] in the aqueous medium. It reacts with water molecule to form [tex]{\left[{{\mathbf{MnOH}}{{\left( {{{\mathbf{H}}_{\mathbf{2}}}{\mathbf{O}}} \right)}_{\mathbf{5}}}} \right]^{{\mathbf{2 + }}}}[/tex] and [tex]{{\mathbf{H}}_{\mathbf{3}}}{{\mathbf{O}}^{\mathbf{ + }}}[/tex] is also released during the reaction.
Learn more:
1. The reason for the acidity of water https://brainly.com/question/1550328
2. Reason for the acidic and basic nature of amino acid https://brainly.com/question/5050077
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Chemical reaction and equation
Keywords: acid, Mn3+, Arrhenius theory, Bronsted-Lowry theory, Lewis theory, H3O+, HCl, NH3, BF3, SO3, hydrogen ions, hydronium ions, hydroxide ions, aqueous, water, Mn(H20)63+, MnOH(H2O)63+, H2O, accepts, donates, electrons, reaction, proton.
The equation that depicts Mn3+ as an acid is shown is; Mn3+(aq) + 6NH3(aq) ------->[Mn(NH3)]^3+(aq)
There are several ways of defining acids and bases such as;
Lewis definition of acids an bases extends beyond aqueous phase reactions. According to this reaction, acids accept lone pairs of electrons while bases donate lone pair of electrons. In this sense, Mn3+ acts as an acid.
An equation that depicts Mn3+ as an acid is shown below;
Mn3+(aq) + 6NH3(aq) ------->[Mn(NH3)]^3+(aq)
In this case NH3 is the Lewis base that donates six lone pairs of electrons to form the six-coordinate complex as shown in the equation.
Learn more: https://brainly.com/question/11969651
