Sulphuric acid or H_{2}SO_{4} appears as a colorless oily liquid, and MnS is a sulfide salt of manganese. Let us explore the several facets of the reaction between these two compounds.

**Sulphuric acid is also known as the king of acids because of its huge application in manufacturing different chemicals. Manganese sulfide appears as a brown, green or red-colored powder. The crystals of MnS have a rock salt type of structure.**

As we continue, all the essential features of the reaction between H_{2}SO_{4} and MnS will come to light.

**What is the product of H**_{2}SO_{4} and MnS

_{2}SO

_{4}and MnS

**Manganese sulfate (MnSO _{4}) and hydrogen sulfide (H_{2}S) gas are the products of the reaction H_{2}SO_{4} + MnS. **

**H _{2}SO_{4} (aq) + MnS (s) = MnSO_{4} (aq) + H_{2}S (g)**

**What type of reaction is H**_{2}SO_{4} and MnS

_{2}SO

_{4}and MnS

**H _{2}SO_{4} + MnS**

**belongs to the category of displacement reaction.**

**How to balance H**_{2}SO_{4} and MnS

_{2}SO

_{4}and MnS

**The reaction H_{2}SO_{4} + MnS**

**is balanced using the following steps-**

**H _{2}SO_{4} + MnS = MnSO_{4} + H_{2}S**

**The reaction is already balanced as the number of atoms of H, S, O, and Mn are intact after the reaction.**

Element | Before reaction | After reaction |
---|---|---|

H | 2 | 2 |

S | 2 | 2 |

O | 4 | 4 |

Mn | 1 | 1 |

**Number of atoms before and after the reaction**

**H**_{2}SO_{4} and MnS titration

_{2}SO

_{4}and MnS titration

**Titration between H _{2}SO_{4} and MnS is not possible as this is a reaction between an acid with a sulfide salt producing a sulfate salt and an acid.**

**H**_{2}SO_{4} and MnS net ionic equation

_{2}SO

_{4}and MnS net ionic equation

**The net ionic equation for H _{2}SO_{4} + MnS**

**is**

**2H ^{+} (aq) + MnS (s) = Mn^{2+} (aq) + H_{2}S(g)**

**These are the steps to be followed to derive the net ionic equation.**

**Write the respective ions only for soluble ionic compounds.****H**_{2}SO_{4}and MnSO_{4}being ionic, dissociate into cations and anions.**The complete ionic equation is****2H**^{+}(aq) + SO_{4}^{2}_{–}**(aq) + MnS (s) = Mn**^{2+}(aq) + SO_{4}^{2-}(aq) + H_{2}S (g)**SO**_{4}^{2-}ion being the spectator ion here, will be canceled from both sides.**Thus the net ionic equation is****2H**^{+}(aq) + MnS (s) = Mn^{2+}(aq) + H_{2}S(g)

**H**_{2}SO_{4} and MnS conjugate pairs

_{2}SO

_{4}and MnS conjugate pairs

**Sulfate ion (SO**_{4}^{2-}) is the conjugate base of the acid H_{2}SO_{4}.**MnS does not have****a conjugate pair**as it is a metal sulfide.

**H**_{2}SO_{4} and MnS intermolecular forces

_{2}SO

_{4}and MnS intermolecular forces

**H-bonding****and****dipole-dipole these two intermolecular forces are present in H**_{2}SO_{4}molecule where the first one is more significant.**Electrostatic force of attraction will be there in MnS as it is ionic in nature.**

**H**_{2}SO_{4} and MnS reaction enthalpy

_{2}SO

_{4}and MnS reaction enthalpy

**For H _{2}SO_{4} + MnS**,

**the reaction enthalpy value is -27.2 kJ/mole.**

Compounds | Enthalpy of formation (ΔH_{f}°) in kJ/mole |
---|---|

H_{2}SO_{4} (aq) | -909.3 |

MnS (s) | -214.2 |

MnSO_{4} (aq) | -1130.1 |

H_{2}S(g) | -20.6 |

**Table representing enthalpy of formation values of all compounds**

**Reaction Enthalpy = ΣΔH**_{f}°(products) – ΣΔH_{f}° (reactants)**= [(-1130.2) + (-20.6)] – [(-909.3) + (-214.2)]****KJ/mol****= -27.2 KJ/mol**

**Is H**_{2}SO_{4} and MnS a buffer solution

_{2}SO

_{4}and MnS a buffer solution

**H _{2}SO_{4} + MnS cannot be a buffer solution as H_{2}SO_{4 }is a strong acid.**

**Is H**_{2}SO_{4} and MnS a complete reaction

_{2}SO

_{4}and MnS a complete reaction

**H _{2}SO_{4} + MnS is a complete reaction, as there is no further reaction once MnSO_{4} and H_{2}S are formed.**

**Is H**_{2}SO_{4} and MnS an exothermic or endothermic reaction

_{2}SO

_{4}and MnS an exothermic or endothermic reaction

**H _{2}SO_{4} + MnS is exothermic in nature as -27.2 kJ/mole heat is released.**

**Is H**_{2}SO_{4} and MnS a redox reaction

_{2}SO

_{4}and MnS a redox reaction

**H _{2}SO_{4} + MnS is not a redox reaction as oxidation states are the same for the atoms H, S, O, and Mn before and after the reaction.**

**Is H**_{2}SO_{4} and MnS a precipitation reaction

_{2}SO

_{4}and MnS a precipitation reaction

**H _{2}SO_{4} + MnS is not a precipitation reaction as the product MnSO_{4 }is a water-soluble compound, and the other product is a gas.**

**Is H**_{2}SO_{4} and MnS reversible or irreversible reaction

_{2}SO

_{4}and MnS reversible or irreversible reaction

**H _{2}SO_{4} + MnS is an irreversible reaction as it is a unidirectional reaction.**

**Is H**_{2}SO_{4} and MnS displacement reaction

_{2}SO

_{4}and MnS displacement reaction

**H _{2}SO_{4} + MnS is a displacement reaction as SO_{4}^{2-} and S^{2-} ions are interchanged between two reactant molecules, H_{2}SO_{4} and MnS.**

#### Conclusion

In conclusion, the product MnSO_{4} can form a variety of hydrates, all of which can dissolve in water producing a faint pink-colored solution. The other product, H_{2}S, is a colorless, pungent-odoured gas.

Hello, I am Tuluma Das, Completed my Ph.D. in Organic Chemistry from the Indian Association for the Cultivation of Science. I have a total of 9 years of research experience including a Ph.D. and Postdoc and 3 years of teaching experience. I have published 7 papers so far in international journals. Let’s connect through Linkedin :