KMnO_{4} is a strong oxidizing agent and can react with molecules having higher reduction potential. Let us see in detail the mechanism of its reaction with H2SO4.

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**Potassium permanganate is a purple violate solid molecule and it is a powerful reagent as the central metal Mn presents a +7 oxidation state. It can react with a cold and concentrated khuông of sulfuric acid and khuông different oxidized products. In this reaction, KMnO _{4} acts as a self catalyst. **

Let us discuss the mechanism of the reaction between sulfuric acid and iron, the reaction enthalpy, the type of reaction, product formation, etc in the following part of the article.

## 1. What is the product of H_{2}SO_{4} and KMnO_{4}?

**Manganese sulfate and Potassium sulfate are formed as major products when H _{2}SO_{4} and KMnO4 are reacted together. Water molecules and oxygen gas are also evolved due đồ sộ their reaction.**

## 2. What type of reaction is H_{2}SO_{4} + KMnO4?

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

**+ KMnO4 reaction is an example of a double displacement reaction along with redox and precipitation reactions. It is also oxygen evolved reaction along with a hydrolysis reaction.**

## 3. How đồ sộ balance H_{2}SO_{4} + KMnO4?

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

**+ KMnO4 = MnSO**:

_{4}+ K_{2}SO_{4}+ H_{2}O + O_{2}We have đồ sộ balance the equation in the following way

**Step 1 – Labelling all the reactants and products by the required number of alphabets****First, we labeled all the reactants and products by A, B, C, D, and E as there are only five different atoms obtained for this reaction and the reaction looks like**:**A H**_{2}SO_{4}+ B KMnO4 = C MnSO_{4}+ D K_{2}SO_{4}+ E H_{2}O + F O_{2}**Step 2 – Equating all the Coefficients for all the same type of elements by rearranging them****After the rearrangement of all the coefficients of the same elements by their stoichiometric proportion we get, H = 2A = 2E, S = A = C = D, O = 4A = 4B = 4C = 4 chiều = E =2F, Mn = B = C, K = B = 2d****Step 3 – Using Gaussian elimination đồ sộ determine the coefficient values****Using the Gaussian elimination and equating all the equations we get, A = 6, B = 4, C = 4, D = 2, E = 6, and F= 5,****Step 4- now write the whole equation in the balanced form****The overall balanced equation will be,****6 H**_{2}SO_{4}+ 4 KMnO4 = 4 MnSO_{4}+ 2 K_{2}SO_{4}+ 6 H_{2}O + 5 O_{2}

## 4. H_{2}SO_{4} + KMnO_{4} titration

**To estimate the quantity of potassium or manganese we can perform a titration between KMnO _{4} and **

**H**

_{2}SO_{4}

### Apparatus used

**We need a burette, conical flask, burette holder, volumetric flask, and beakers for this titration.**

### Titre and titrant

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

**versus KMnO**

_{4},**H**

_{2}SO_{4}acts**as a titrant which is taken in the burette and the molecule đồ sộ be analyzed is KMnO**

_{4}which is taken in a conical flask.

### Indicator

**The whole titration is done in acidic pH as the concentration of H _{2}SO_{4} is high and for this reaction, KMnO_{4} acts as a self-indicator because it is a colored solution and in different pH, it changes color.**

### Procedure

**The burette was filled with standardized ****H _{2}SO_{4}**

**and KMnO**

_{4}was taken in a conical flask along with the respective indicator.**H**

_{2}SO_{4}**is added dropwise đồ sộ the conical flask and the flask was shaking constantly. After a certain time when the endpoint arrived KMnO**

_{4}changes its color.

We repeat the titration several times for better results and then we estimate the potassium as well as manganese quantity by the formula V_{1}S_{1 }= V_{2}S_{2}.

## 5. H_{2}SO_{4}+ KMnO_{4} net ionic equation

**The net ionic equation between ****H _{2}SO_{4}**

**+ KMnO**

_{4}is as follows,

**2H**^{+}** + SO _{4}^{2-} + **

**K**

^{+}+ MnO_{4}^{–}**= Mn**

^{2+}+**K**

^{+}+**SO**

_{4}^{2-}+ H^{+}+ OH^{–}+ O_{2}

**To derive the net ionic equation the following steps are required,****First H**_{2}SO_{4}**will be ionized in proton and sulfate ions as it is a strong electrolyte****After that KMnO4 also dissociated đồ sộ K**^{+}ion and SO_{4}^{2-}.**After that, the product MnSO**_{4}also dissociated đồ sộ Mn^{2+}which is d^{5}stable configuration and corresponding SO_{4}^{2-}.**Water is also ionized đồ sộ H**^{+}and OH^{-.}**O**_{2}remains undissociated.

## 6. H_{2}SO_{4}+ KMnO_{4} conjugate pairs

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**In the reaction, H _{2}SO_{4}**

**+ KMnO**

_{4}conjugate pairs will be the corresponding de-protonated and protonated khuông of that particular species which are listed below-

**Conjugate pair of****H**_{2}SO_{4}**= SO**_{4}^{2-}**Conjugate pair of OH**^{–}=**H**_{2}O

## 7. H_{2}SO_{4} and KMnO_{4} intermolecular forces

**The intermolecular force between H _{2}SO_{4} is an electrostatic, covalent force. For the KMnO_{4} it is ionic interaction and for MnSO_{4} and K_{2}SO_{4} the ionic interaction is along with the coulombic force. H-bonding is present in water and cầu xin der waal’s force acts in O_{2} molecules.**

Molecule | Actingforce |

H_{2}SO_{4} | Electrostatic, van der waal’s Dipole interaction |

KMnO_{4} | Ionic, metallic, and electrostatic |

K_{2}SO_{4} / MnSO_{4} | Coulombic force, strong ionic interaction |

H_{2}O | Covalent, H-bonding |

O_{2} | Van der Waal’s force, London force |

**Intermolecular Forces**

## 8. H_{2}SO_{4} + KMnO_{4} reaction enthalpy

**In the reaction, H _{2}SO_{4}**

**+ KMnO**

_{4}**reaction enthalpy**

**is,-4400.4 KJ/mol which can be obtained by the formula enthalpy of products – enthalpy of reactants, and here the change in enthalpy is positive.**

Molecule | Enthalpy(KJ/mol) |

KMnO4 | -813 |

H_{2}SO_{4} | -814 |

MnSO_{4} | -1130 |

K_{2}SO_{4} | -1437.8 |

H_{2}O | -68 |

O_{2} | 0 |

**Enthalpy of Reactants**

**and Products**

## 9. Is H_{2}SO_{4} + KMnO_{4} a buffer solution?

**The reaction between ****H _{2}SO_{4}**

**+ KMnO4 gives a buffer solution and they can control the pH of the solution.**

## 10. Is H_{2}SO_{4} + KMnO_{4} a complete reaction?

**The reaction between ****H _{2}SO_{4}**

**+ KMnO**

_{4 }is the complete reaction because it gives two complete products MnSO_{4}and K_{2}SO_{4 }along with O_{2}gas.

**11. **Is H_{2}SO_{4} + KMnO_{4} an exothermic or endothermic reaction?

**The reaction ****H _{2}SO_{4}**

**+ KMnO4 is exothermic in terms of thermodynamics first law. So, the reaction releases more energy and temperature đồ sộ the surrounding ví we have đồ sộ be more**

**cautious**

**, Where δH is always negative.**

## 12. Is H_{2}SO_{4} + KMnO_{4} a redox reaction?

**The reaction between H _{2}SO_{4} + KMnO_{4} is a **

**redox reaction**

**because in this reaction many elements get reduced and oxidized.**

## 13. Is H_{2}SO_{4} + KMnO_{4} a precipitation reaction

**The reaction H _{2}SO_{4} + KMnO_{4} is a precipitation reaction because it gets precipitated in the solution and is not soluble in the reaction mixture.**

## 14. Is H_{2}SO_{4} + KMnO_{4} reversible or irreversible reaction?

**The reaction between H _{2}SO_{4}+ KMnO4 is irreversible because we get O_{2} gas as a product. When gas is formed during the reaction, the entropy of the reaction increases and the equilibrium of the reaction shifts towards the right-hand side only.**

## 15. Is H_{2}SO_{4} + KMnO_{4} displacement reaction?

**The reaction between H _{2}SO_{4}+ KMnO_{4} is an example of **

**single displacement**

**reaction because in the above reaction Mn and K are displaced by H**

^{+}in H_{2}SO_{4}and O_{2}gas becomes không tính tiền from the reaction.

#### Conclusion

H_{2}SO_{4} and KMnO_{4} reaction mainly gives us K_{2}SO_{4} and MnSO_{4} along with oxygen gas ví it is a commercially important reaction for the production of oxygen gas. Also, the quantitative analysis of the H_{2}SO_{4} and KMnO_{4} give the amount of Mn and K in the respective sample.

Read more about 11 Facts on H2SO4 + Al(OH)3.

Read more facts on H2SO4:

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H2SO4 + KClO3 H2SO4 + NaH H2SO4 + NaOCl H2SO4 + K2S H2SO4 + MnO2 H2SO4 + HCOOH H2SO4 + Mn2O7 H2SO4 + Mg H2SO4 + Na2CO3 H2SO4 + Sr(NO3)2 H2SO4 + MnS H2SO4 + NaHSO3 H2SO4 + CaCO3 H2SO4 + CH3COONa H2SO4 + Sn H2SO4 + Al2O3 H2SO4 + SO3 H2SO4 + H2O H2SO4 + Fe2S3 H2SO4 + NH4OH H2SO4 + Li3PO4 H2SO4 + Na2HPO4 H2SO4 + Zn(OH)2 H2SO4 + BeO | H2SO4 + KOH H2SO4 + CH3CH2OH H2SO4 + Li2O H2SO4 + K2Cr2O7 H2SO4 + NaOH H2SO4+ Ag H2SO4 + Mn3O4 H2SO4 + NaH2PO4 H2SO4 + Sr H2SO4 + Zn H2SO4-HG2(NO3)2 H2SO4 + Pb(NO3)2 H2SO4 + Na H2SO4 + Ag2S H2SO4 + BaCO3 H2SO4 + PbCO3 H2SO4 + Sr(OH)2 H2SO4 +Mg3N2 H2SO4 + LiOH H2SO4 + Cl2 H2SO4 + Be H2SO4 + Na2S H2SO4 + Na2S2O3 H2SO4 + As2S3 | H2SO4 + Fe(OH)3 H2SO4 + Al(OH)3 H2SO4 + NaI H2SO4 + K2CO3 H2SO4 + NaNO3 H2SO4 + CuO H2SO4 + Fe2O3 H2SO4 + AgNO3 H2SO4 + Al H2SO4 + K2SO4 H2SO4-HGO H2SO4 + Ba H2SO4 + MnCO3 H2SO4 + K2SO3 H2SO4 + PbCl2 H2SO4 + P4O10 H2SO4 + NaHCO3 H2SO4 + O3 H2SO4 + Ca(OH)2 H2SO4 + Be(OH)2 HCl + H2SO4 H2SO4 + FeCl2 H2SO4 + ZnCl2 H2SO4 + Al2(SO3)3 | H2SO4 + KMnO4 H2SO4 + CH3NH2 H2SO4 + CH3COOH H2SO4 + Pb H2SO4 + CH3OH H2SO4 + Fe2(CO3)3 H2SO4 + Li2CO3 H2SO4 + MgO H2SO4 + Na2O H2SO4 + F2 H2SO4 + Zn(NO3)2 H2SO4 + Ca H2SO4 + K2O H2SO4 + Mg(OH)2 H2SO4+NaF H2SO4 + Sb2S3 H2SO4 + NH4NO3 H2SO4 + AlBr3 H2SO4 + CsOH H2SO4 + BaSO3 H2SO4 + AlCl3 H2SO4 + AlPO4 H2SO4 + Li2SO3 | H2SO4 + Fe H2SO4 + HCOONa H2SO4 + Cu H2SO4 + PbS H2SO4 + P2O5 H2SO4 + CuCO3 H2SO4 + Li H2SO4 + K2CrO4 H2SO4 + NaCl H2SO4 + Ag2O H2SO4 +Mg2Si H2SO4 + Mn(OH)2 H2SO4+ NACLO2 H2SO4 + K H2SO4 + CaCl2 H2SO4 + Li2S H2SO4 + SrCO3 H2SO4 + H2O2 H2SO4 + CuS H2SO4 + KBr H2SO4 + Fe3O4 H2SO4 + Fe3O4 H2SO4 + KI |

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