HCl and Mn_{2}(SO_{4})_{3} are both inorganic compounds wherein HCl is a corrosive powerful acid and Mn_{2}(SO_{4})_{3} is a metal sulfate. Let us analyze the reaction between HCl and Mn_{2}(SO_{4})_{3} in detail.

**Hydrochloric acid (HCl) is found in both liquid and gaseous forms and is typically prepared by dissolving hydrogen chloride in water. It is an odorless, colorless, acidic chemical that is highly reactive. Manganese (III) sulfate, Mn _{2}(SO_{4})_{3}, is a white transition metal sulfate and has a molar mass of 398.06 g/mol.**

This article shall focus on the many aspects of the HCl + Mn_{2}(SO_{4})_{3} reaction, such as the product, reaction type, intermolecular forces, and so on.

**What is the product of HCl + Mn**_{2}(SO_{4})_{3}

_{2}(SO

_{4})

_{3}

**Manganese (III) sulfate reacts with HCl to form manganese (II) sulfate, chlorine, and sulfuric acid.**

**Mn _{2}(SO_{4})_{3} + 2HCl**

**—> 2MnSO**

_{4}+ Cl_{2}+ H_{2}SO_{4}**What type of reaction is HCl + Mn**_{2}(SO_{4})_{3}

_{2}(SO

_{4})

_{3}

**The reaction of HCl with Mn _{2}(SO_{4})_{3} is a single displacement reaction.**

**How to balance HCl + Mn**_{2}(SO_{4})_{3 }

_{2}(SO

_{4})

_{3 }

**Following are the steps to balance HCl + Mn _{2}(SO_{4})_{3} reaction:**

**The chemical equation to be balanced: Mn _{2}(SO_{4})_{3} + HCl =**

**MnSO**

_{4}+ Cl_{2}+ H_{2}SO_{4}**The count of the total number of atoms of each element on the reactant side must equal the total number of atoms on the product side for the reaction to be balanced.**

Atoms | Reactant Side | Product Side |

Manganese | 2 | 1 |

Sulfur | 3 | 2 |

Chlorine | 1 | 2 |

Oxygen | 12 | 8 |

Hydrogen | 1 | 2 |

**Table representing the count of atoms**

**In order to equate Manganese and Chlorine, MnSO**_{4}and HCl are each multiplied by coefficient 2, as a result balancing the remaining unbalanced atoms (S, O and H) on both sides of the reaction.**Thus, the overall balanced chemical equation is:**

**Mn _{2}(SO_{4})_{3} + 2HCl = 2MnSO_{4} + Cl_{2} + H_{2}SO_{4}**

**HCl + Mn**_{2}(SO_{4})_{3 }Titration

_{2}(SO

_{4})

_{3 }Titration

**Titration of HCl with Mn**_{2}(SO_{4})_{3}cannot be conducted to determine the volume of the analyte.**The reactant Mn**_{2}(SO_{4})_{3}acts as a salt in this reaction, yielding no significant results and besides, it is not an acid-base type of reaction.

**HCl + Mn**_{2}(SO_{4})_{3 }Net Ionic Equation

_{2}(SO

_{4})

_{3 }Net Ionic Equation

**The net ionic equation of HCl +** **Mn _{2}(SO_{4})_{3}**

**is: 2H**

^{+}+ 2Cl^{–}+ 2Mn^{3+}+ SO_{4}^{2-}= 2Mn^{2+}+ 2SO_{4}^{2-}+ Cl_{2}+ 2H^{+}+ SO_{4}^{2-}**The steps to derive the net ionic equation are as follows:**

**Firstly, the complete balanced equation is written.**

**Mn _{2}(SO_{4})_{3} + 2HCl**

**—> 2MnSO**

_{4}+ Cl_{2}+ H_{2}SO_{4}**The atoms are then split into ions followed by elimination of the spectator ions. Thus, the overall net ionic equation between HCl and Mn**_{2}(SO_{4})_{3}is:

**2H ^{+} + 2Cl^{–} + 2Mn^{3+} + SO_{4}^{2-} = 2Mn^{2+} + 2SO_{4}^{2-} + Cl_{2} + 2H^{+} + SO_{4}^{2-}**

**HCl + Mn**_{2}(SO_{4})_{3 }Conjugate Pairs

_{2}(SO

_{4})

_{3 }Conjugate Pairs

**The conjugate pairs formed during the reaction between HCl + Mn_{2}(SO_{4})_{3 }are:**

**Conjugate base of HCl = Cl**^{–}**Conjugate base of H**_{2}SO_{4}= HSO_{4}^{–}

**HCl + Mn**_{2}(SO_{4})_{3 }Intermolecular Forces

_{2}(SO

_{4})

_{3 }Intermolecular Forces

**Hydrogen bonding, dipole-dipole interactions and London dispersion forces are the intermolecular forces of attraction experienced by the HCl molecule.****Dipole-dipole (dipole exists between sulfur and oxygen), London dispersion and Ionic forces are the intermolecular forces that keep the molecules of Mn**_{2}(SO_{4})_{3 }together.

**Is HCl + Mn**_{2}(SO_{4})_{3 }a Buffer Solution

_{2}(SO

_{4})

_{3 }a Buffer Solution

**HCl + Mn _{2}(SO_{4})_{3 }is not a buffer solution as the solution contains strong Hydrochloric acid and a manganese salt.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }a Complete Reaction

_{2}(SO

_{4})

_{3 }a Complete Reaction

**HCl + Mn _{2}(SO_{4})_{3 }is a complete reaction as the reactants are totally consumed to yield complete products.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }an Exothermic or Endothermic Reaction

_{2}(SO

_{4})

_{3 }an Exothermic or Endothermic Reaction

**The reaction HCl + Mn _{2}(SO_{4})_{3 }is an exothermic reaction as heat is released to the surroundings during the course of the reaction.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }a Redox Reaction

_{2}(SO

_{4})

_{3 }a Redox Reaction

**HCl + Mn _{2}(SO_{4})_{3 }is a redox reaction where a change in oxidation state is observed for various elements in this reaction. For instance,**

**Mn**_{2}(SO_{4})_{3}functions as an oxidizing agent, reducing Mn from a +3 oxidation state on the reactant side to a +2 oxidation state on the product side.**HCl acts as a reducing agent, oxidizing Cl from a -1 oxidation state on the reactant side to a +0 oxidation state on the product side.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }a Precipitation Reaction

_{2}(SO

_{4})

_{3 }a Precipitation Reaction

**HCl + Mn _{2}(SO_{4})_{3 }is not a precipitation reaction, as no insoluble product is formed during the reaction.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }a Reversible or Irreversible Reaction

_{2}(SO

_{4})

_{3 }a Reversible or Irreversible Reaction

**HCl + Mn _{2}(SO_{4})_{3 }is an irreversible reaction since MnSO_{4} and H_{2}SO_{4} produced in this reaction are stable and cannot be utilized to recover the reactants under the same reaction parameters.**

**Is HCl + Mn**_{2}(SO_{4})_{3 }Displacement Reaction

_{2}(SO

_{4})

_{3 }Displacement Reaction

**HCl + Mn _{2}(SO_{4})_{3 }is a displacement reaction as hydrogen ion displaces the sulfate ion from Mn_{2}(SO_{4})_{3 }to form H_{2}SO_{4}.**

**Conclusion**

Manganese (III) sulfate reacts with hydrochloric acid to produce Manganese (II) sulfate and sulfuric acid in a single displacement reaction. During the reaction process, yellowish-green Chlorine gas evolved is an excellent oxidizing agent with biological applications.

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