H_{2}SO_{4} is a strong acid, and Pb(NO_{3})_{2} is a base. Let us see the reaction of H_{2}SO_{4} +Pb(NO_{3})_{2}.

**H _{2}SO_{4} is a clear and colorless liquid that reacts with Pb(NO_{3})_{2}, a white colorless solid. Pure sulfuric acid does not exist naturally on Earth due to its strong affinity to water vapor and Lead(II) nitrate must be handled with care to prevent inhalation and skin contact.**

Here, in this article, we will discuss some facts about the reaction, like net ionic reaction and enthalpy of the reaction.

**What is the product of H**_{2}SO_{4} and Pb(NO_{3})_{2}

_{2}SO

_{4}and Pb(NO

_{3})

_{2}

**Lead Sulfate and Nitric Acid** **are** **produced** **in** **the** **H _{2}SO_{4} + Pb(NO_{3})_{2}**

**reaction.**

**H _{2}SO_{4}+Pb(NO_{3})_{2}= Pb(SO_{4})+ HNO_{3}**

**What type of reaction is ****H**_{2}SO_{4} and Pb(NO_{3})_{2}

**H**

_{2}SO_{4}and Pb(NO_{3})_{2}**H _{2}SO_{4} + Pb(NO_{3})_{2} is a precipitation reaction**.

**How to balance ****H**_{2}SO_{4} and Pb(NO_{3})_{2}

**H**

_{2}SO_{4}and Pb(NO_{3})_{2}**The reaction** **H _{2}SO_{4} + Pb(NO_{3})_{2}**

**is**

**balanced**

**using**

**the**

**following**

**steps:**

**H _{2}SO_{4}+Pb(NO_{3})_{2} = Pb(SO_{4})+ HNO_{3}**

**The first thing we check is the number of atoms on the reactant and product sides.****After that, if the number of atoms is not the same, then we have done multiplication of the smallest figure according to the formula**.**In the above equation, the H atom and NO**_{3}atoms number are not the same

**So, in this next step, we should multiply HNO**_{3}by 2.

**Thus the balance equation is****H**_{2}SO_{4 }+ Pb(NO_{3})_{2}= Pb(SO_{4}) + 2 HNO_{3}

**H**_{2}SO_{4} and Pb(NO_{3})_{2} titration

**H**titration

_{2}SO_{4}and Pb(NO_{3})_{2}**Titration is not possible in the reaction H _{2}SO_{4 }+ Pb(NO_{3})_{2} because H_{2}SO_{4} is an acid, and when it reacts with Pb(NO_{3})_{2}, it forms precipitate of Pb(SO_{4}).**

**H**_{2}SO_{4} and Pb(NO_{3})_{2} **net ionic equation**

**H**

_{2}SO_{4}and Pb(NO_{3})_{2}**The net ionic equation for the reaction H_{2}SO_{4 }+ Pb(NO_{3})_{2} is **

**Pb² ^{+}(aq)+SO₄²^{–}(aq)⇒ PbSO₄(s).**

**To derive the net ionic equation, following steps are followed **

**First, the soluble ionic compounds can dissociated into ions.****Pb²**^{+}(aq)+ 2NO₃^{–}(aq) + 2H^{+}(aq)+SO₄²^{–}(aq) ⇒ PbSO₄(s) + 2H^{+}(aq)+2NO₃^{–}(aq).**Spector ions****2NO₃**^{–}and 2H^{+}**are cancelled out.****The Spector ion is 2NO₃**^{–}and 2H^{+}.**Thus the net ionic equation****is****Pb²**^{+}(aq)+SO₄²^{–}(aq)⇒ PbSO₄(s).

**H**_{2}SO_{4} and Pb(NO_{3})_{2} **conjugate pairs**

**H**

_{2}SO_{4}and Pb(NO_{3})_{2}**H**_{2}SO_{4 }+ Pb(NO_{3})_{2}**doesn’t form conjugate pairs because PbSO**_{4}is in precipitate form.

**conjugated****base of****H**is HSO_{2}SO_{4}_{4}^{–}.

**H**_{2}SO_{4} and Pb(NO_{3})_{2} **intermolecular forces**

**H**

_{2}SO_{4}and Pb(NO_{3})_{2}**Dipole-dipole interactions and strong hydrogen bonding are present as intermolecular forces****in**.**H**_{2}SO_{4}

**Both ionic and covalent bonds are present in Pb(NO**_{3})_{2}, as nitrogen and oxygen are non-metals, whereas lead is a metal.

**H**_{2}SO_{4} and Pb(NO_{3})_{2} **reaction enthalpy**

_{2}SO

_{4}and Pb(NO

_{3})

_{2}

**The reaction enthalpy of H_{2}SO_{4 }+ Pb(NO_{3})_{2} reaction is -8.97 KJ/mol.**

**Is ****H**_{2}SO_{4} and Pb(NO_{3})_{2} a buffer solution?

**H**a buffer solution?

_{2}SO_{4}and Pb(NO_{3})_{2}** H_{2}SO_{4 }+ Pb(NO_{3})_{2}** reaction can not form a buffer solution because

**is a strong acid.**

**H**_{2}SO_{4}**Is ****H**_{2}SO_{4} and Pb(NO_{3})_{2} a complete reaction?

**a complete reaction?**

**H**_{2}SO_{4}and Pb(NO_{3})_{2} **H_{2}SO_{4 }+ Pb(NO_{3})_{2} ** is a complete reaction because

**lead sulfate and nitric acid**are formed in reaction .

**Is ****H**_{2}SO_{4} and Pb(NO_{3})_{2} an exothermic or endothermic reaction?

**an exothermic or endothermic reaction?**

**H**_{2}SO_{4}and Pb(NO_{3})_{2}** H_{2}SO_{4 }+ Pb(NO_{3})_{2} is an exothermic reaction, because the enthalpy of the reaction that it is negative. **

**Is H**_{2}SO_{4} + Pb(NO_{3})_{2} a redox reaction?

_{2}SO

_{4}+ Pb(NO

_{3})

_{2}a redox reaction?

** H_{2}SO_{4 }+ Pb(NO_{3})_{2}** reaction is not a redox reaction because the oxidation state of Pb(NO

_{3})

_{2 }is not changed during the reaction.

**Is H**_{2}SO_{4} + Pb(NO_{3})_{2} a precipitation reaction?

_{2}SO

_{4}+ Pb(NO

_{3})

_{2}a precipitation reaction?

**H_{2}SO_{4 }+ Pb(NO_{3})_{2}** is a precipitation reaction as PbSO

_{4}formed produces precipitate.

**Is H**_{2}SO_{4} + Pb(NO_{3})_{2} reversible or irreversible reaction?

_{2}SO

_{4}+ Pb(NO

_{3})

_{2}reversible or irreversible reaction?

**H _{2}SO_{4 }+ Pb(NO_{3})_{2}**

**product of the reaction is a residue, so it is an irreversible reaction.**

**Is H**_{2}SO_{4} + Pb(NO_{3})_{2} displacement reaction?

_{2}SO

_{4}+ Pb(NO

_{3})

_{2}displacement reaction?

**H_{2}SO_{4 }+ Pb(NO_{3})_{2} is a double displacement reaction because H replaces Pb from Pb(NO_{3})_{2} and Pb replaces H from H_{2}SO_{4}** .

**Conclusion**

This reaction of Sulfuric acid and Lead nitrate gives Lead sulfate and Nitric acid. This is a precipitation reaction and irreversible. We use this reaction to form Nitric acid.

Hi……I am Mrinmoyee Pal, I have completed my Bachelor’s degree in Chemistry from The University of Burdwan and currently I am doing my Master’s Degree in Chemistry from Rani Rashmoni Green University.

My LinkedIn profile is http://www.linkedin.com/in/mrinmoyee-pal-828410254