Question

What is the net ionic equation of the reaction of mgso4 with sr(no3)2?

Answer 1

The net ionic equation for the reaction is as follows:$\boxed{{\text{SO}}_4^{2 - }\left( {aq} \right) + {\text{S}}{{\text{r}}^{2 + }}\left( {aq} \right) \to {\text{SrS}}{{\text{O}}_4}\left( s \right)}$

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 compound AX and BY is as follows:

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

The three types of equations that are used 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 undissociated form. In total ionic equation, 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.

The steps to write the net ionic reaction are as follows:

Step 1: Write the molecular equation for the reaction with the phases in the bracket.

In the reaction, ${\text{MgS}}{{\text{O}}_4}$ reacts with ${\text{Sr}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2}$ to form ${\text{SrS}}{{\text{O}}_4}$ and ${\text{Mg}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2}$. The balanced molecular equation of the reaction is as follows:

${\text{MgS}}{{\text{O}}_4}\left( {aq} \right) + {\text{Sr}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2}\left( {aq} \right) \to {\text{SrS}}{{\text{O}}_4}\left( s \right) + {\text{Mg}}{\left( {{\text{N}}{{\text{O}}_{\text{3}}}} \right)_2}\left( {aq} \right)$

Step 2: Dissociate all the compounds with the aqueous phase to write the total ionic equation. The compounds with solid phase remain same. The total ionic equation is as follows:

${\text{M}}{{\text{g}}^{2 + }}\left( {aq} \right) + {\text{SO}}_4^{2 - }\left( {aq} \right) + {\text{S}}{{\text{r}}^{2 + }}\left( {aq} \right) + 2{\text{NO}}_3^ - \left( {aq} \right) \to {\text{SrS}}{{\text{O}}_4}\left( s \right) + {\text{M}}{{\text{g}}^{2 + }}\left( {aq} \right) + 2{\text{NO}}_3^ - \left( {aq} \right)$

Step 3: The common ions on both the sides of the reaction get cancelled out to get the net ionic equation.

$\boxed{{\text{M}}{{\text{g}}^{2 + }}\left( {aq} \right)} + {\text{SO}}_4^{2 - }\left( {aq} \right) + {\text{S}}{{\text{r}}^{2 + }}\left( {aq} \right) + \boxed{2{\text{NO}}_3^ - \left( {aq} \right)} \to {\text{SrS}}{{\text{O}}_4}\left( s \right) + \boxed{{\text{M}}{{\text{g}}^{2 + }}\left( {aq} \right)} + \boxed{2{\text{NO}}_3^ - \left( {aq} \right)}$

Therefore, the net ionic equation obtained is as follows:

${\text{SO}}_4^{2 - }\left( {aq} \right) + {\text{S}}{{\text{r}}^{2 + }}\left( {aq} \right) \to {\text{SrS}}{{\text{O}}_4}\left( s \right)$

Learn more:

1. Balanced chemical equation: brainly.com/question/1405182

2. Oxidation and reduction reaction: brainly.com/question/2973661

Answer details:  

Grade: High School  

Subject: Chemistry  

Chapter: Chemical reaction and equation

Keywords: Double displacement reaction, types of equation, molecular equation, total ionic equation, net ionic equation, MgSO4, Sr(NO3)2, SrSO4,  Mg(NO3)2.

Answer 2

Balanced chemical reaction:  

MgSO₄(aq) + Sr(NO₃)₂(aq) → Mg(NO₃)₂(aq) + SrSO₄(s).

Ionic reaction:  

Mg²⁺(aq) + SO₄²⁻(aq) + Sr²⁺(aq) + 2NO₃⁻(aq) → Mg²⁺(aq) + 2NO₃⁻(aq) + SrSO₄(s).

Net ionic reaction:

Sr²⁺(aq) + SO₄²⁻(aq) → SrSO₄(s).

Magnesium sulfate (MgSO₄), strontium nitrate (Sr(NO₃)₂ and magnesium nitrate (Mg(NO₃)₂) are soluble in water. Strontium sulfate (SrSO₄) is not soluble in water.

This chemical reaction is double displacement reaction - cations and anions of the two reactants switch places and form two new compounds.