Rearranging molecules or ions of substance, into distinct form is called chemical reaction. Let us see, how chemical reaction takes place in case of H_{2}SO_{4} + Ag_{2}O.

**Silver (1) oxide is dark brown powder used for preparation of silver compounds. It is used in silver oxide batteries and also acts as an oxidizing agent. H _{2}SO_{4} being strong acid undergoes reaction with Ag_{2}O giving insoluble salt.**

The study on the effects of adding H_{2}SO_{4}_{ }to Ag_{2}O will be described throughout this article with a chemical equation, in its balanced form.

## What is the product of H_{2}SO_{4 }and Ag_{2}O

** Silver (1) sulphate and water molecule are the product of reaction H _{2}SO_{4} + Ag_{2}O.**

**Ag _{2}O + H_{2}SO_{4} → Ag_{2}SO_{4} + H_{2}O**

## What type of reaction is H_{2}SO_{4} + Ag_{2}O

**H _{2}SO_{4} + Ag_{2}O is double displacement reaction. **

## How to balance H_{2}SO_{4}+ Ag_{2}O

**The reaction is balanced using the following steps.**

**Ag _{2}O + H_{2}SO_{4} → Ag_{2}SO_{4} + H_{2}O**

**Firstly, we have to tag both side of reaction with alphabetical coefficients.****A Ag**_{2}O + B H_{2}SO_{4}→ C Ag_{2}SO_{4}+ D H_{2}O**Expressed coefficient are used to represent alphabetical reactants and products.****Ag = 2A+2C, O = A+4B+4C+D, S = B+C, H = 2B+2D.****Enter the coefficient values into the elimination method for estimation.****Get the smallest, whole integer values from the result by simplifying it.****A = 1, B = 1, C =1, D=1****Thus, the balanced equation is-****Ag**_{2}O + H_{2}SO_{4}→ Ag_{2}SO_{4}+ H_{2}O

## H_{2}SO_{4 }+ Ag_{2}O titration

**Titration between H _{2}SO_{4} and Ag_{2}O is not possible to predict because both are oxidizing agent, so they cannot undergo acid base reaction. However, it**

**shows possibility of redox titration with some irregularities.**

## H_{2}SO_{4}+ Ag_{2}O net ionic equation

**Net ionic equation, for given reaction is**

**2H ^{+} + O^{-2} → H_{2}O**

**For deriving net ionic equation, following steps are used:**

**A molecular equation should be balanced and include the phase of every compound.****H**_{2}SO_{4}(Aq) + Ag_{2}O(S) → Ag_{2}SO_{4 }(S) + H_{2}O(l)**The aqueous salts or chemicals in the equation must be transformed into ions.****Only the strong electrolytes should be broken down because they can completely dissociate.****2H**^{+}+ SO_{4}^{-2}+ 2Ag^{+}+ O^{-2}→ 2Ag^{+}+ SO_{4}^{-2}+ H_{2}O**In order to display the species that are actually involved in the reaction, the spectator ions must be cancelled out.****Thus, the net ionic equation is****2H**^{+}+ O^{-2}→ H_{2}O

## H_{2}SO_{4}and Ag_{2}O conjugate pair

**H**_{2}SO_{4}[Conjugate base] =HSO_{4}^{–}**H**_{2}O [Conjugate acid] = H_{3}O^{+}**Ag**_{2}O does not have any conjugate pairs because it is mild oxidizing agent.

## H_{2}SO_{4}and Ag_{2}O intermolecular forces

**H**_{2}SO_{4}shows London dispersion forces because of presence of non-planarity in its molecule**Van der Waals forces are present in Ag**_{2}O because of general tendency of oxides to show covalent character.

## H_{2}SO_{4} + Ag_{2}O reaction enthalpy

**The reaction enthalpy of H _{2}SO_{4} + Ag_{2}O is -151.2 kJ/mol. **

Numbers | Compounds | ΔH( kJ/mol) |
---|---|---|

1 | H_{2}SO_{4} | -814.4 kJ/mol |

2 | Ag_{2}O | -31 kJ/mol |

3 | Ag_{2}SO_{4} | -715.9 kJ/mol |

4 | H_{2}O | -280.7 kJ/mol |

**Tabular representation of compounds with their enthalpies.**

**The enthalpy is calculated using the formula**:**Change in enthalpy = addition of enthalpies of formation of product – addition of enthalpies of formation of reactant.****Enthalpy change = [(-715.9) + (-280.7)] – [(-814.4) + (-31)]**

**= (-996.6) + (-845.4) kJ/mol**

**= -151.2 kJ/mol**

## Is H_{2}SO_{4}+ Ag_{2}O a buffer solution

**H _{2}SO_{4} + Ag_{2}O does not give buffer solution due to presence of strong H_{2}SO_{4}.**

## Is H_{2}SO_{4} + Ag_{2}O a complete reaction

**H _{2}SO_{4} + Ag_{2}O is complete reaction because the reactants get completely converted to silver (1) sulphate and water molecules.**

## Is H_{2}SO_{4} + Ag_{2}O an exothermic or endothermic reaction

**H _{2}SO_{4} + Ag_{2}O is exothermic in nature, as enthalpy change for this reaction is negative, indicating that heat is released.**

## H_{2}SO_{4} + Ag_{2}O a redox reaction

**H _{2}SO_{4} + Ag_{2}O is not a redox reaction**

**because the reaction does not involve any electron transfer and the oxidation states of every reacting species does not change from the reactant side to the product side**.

## Is H_{2}SO_{4} + Ag_{2}O a precipitation reaction

**H _{2}SO_{4} + Ag_{2}O is a precipitation reaction because silver (1) sulphate has low solubility, it is insoluble in nature, leads to formation of precipitate.**

## Is H_{2}SO_{4} and Ag_{2}O reversible or irreversible reaction.

**H _{2}SO_{4} + Ag_{2}O is irreversible reaction.**

**The formation of white solid precipitate of Ag**

_{2}SO_{4}, makes reaction impossible to revert back.## Is H_{2}SO_{4} + Ag_{2}O displacement reaction

**H _{2}SO_{4} + Ag_{2}O is a double displacement reaction, because both ions of reactants displace their place, resulting in new compound.**

#### Conclusion

Ag_{2}O is used for photocatalytic degradation of organic pollutants and dyes, when reacts with H_{2}SO_{4} leads to formation of white solid precipitate silver (1) sulphate. Ag_{2}SO_{4} is having antimicrobial property and acts as biocide. Displacement of both ions takes place during reaction, results in liberation of heat.

Hello ….I am Sana Khan. A master’s student in organic chemistry from Nagpur University. I want to share my knowledge by publishing articles.