Sulphuric acid (H_{2}SO_{4}) is a strong acid, and silver sulphide (Ag_{2}S) is a dense black solid. Let’s study the various aspects of the H_{2}SO_{4} + Ag_{2}S reaction in detail.

**Sulphuric acid is a corrosive liquid that is dense, colourless, and oily. It completely ionizes in water as it’s a strong acid. Silver sulphide is an inorganic compound which is the only sulphide of silver. It is helpful in photography as a photosensitizer.**

In this article, we will focus on several characteristics of the H_{2}SO_{4} + Ag_{2}S reaction in depth.

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

**Ag _{2}S reacts with H_{2}SO_{4 }to form **

**H**

_{2}S (hydrogen sulphide) and Ag_{2}SO_{4 }(silver sulphate).**Ag _{2}S(s) + H_{2}SO_{4}(aq) **

**→**

**Ag**

_{2}SO_{4}(s) + H_{2}S(s)**What type of reaction is ****H**_{2}SO_{4}+Ag_{2}S?

_{2}SO

_{4}+Ag

_{2}S?

**H _{2}SO_{4} and Ag_{2}S belong to the category of double displacement reaction.**

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

**The general equation of the H**_{2}SO_{4}+ Ag_{2}S reaction is as follows:**Ag**_{2}S + H_{2}SO_{4}→ Ag_{2}SO_{4}+ H_{2}S**The reaction is said to be balanced when the moles of reactant are equal to the moles of product.****The above reaction is already balanced. Hence, the balanced reaction is given by:****Ag**_{2}S + H_{2}SO_{4}→ Ag_{2}SO_{4}+ H_{2}S

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

**H _{2}SO_{4 }+ Ag_{2}S can be titrated to determine the quantity of Ag. However, because the reaction produces a precipitate, it should be carried out carefully.**

**Apparatus used**

**Pipette, Erlenmeyer flask, burette holder, burette, wash bottle, dropper, volumetric flask and beakers.**

**Titre and titrant**

**In ****H _{2}SO_{4 }+Ag_{2}S **

**titration,**

**H**

_{2}SO_{4}**is**

**titrant,**

**and the titre is AgNO**

_{3}.**Indicator**

**Phenolphthalein****, an acid-base indicator, is employed to detect the end point of the titration.**

**Procedure**

**A burette was used to take standardized****H**_{2}SO_{4}**, and an Erlenmeyer flask was used to take AgNO**_{3}.**1-2 drops of phenolphthalein indicator were added.****H**_{2}SO_{4 }from the burette was added dropwise into the conical flask until the solution changed from colourless to light pink.**To obtain three concordant readings the process was repeated.**

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

**The balanced net ionic equation of H _{2}SO_{4}+Ag_{2}S is as follows:**

**Ag _{2}S**

**(s)**

**+ 2H**

^{+}**(aq)**

**+ SO**

_{4}^{2-}**(aq)**

**→**

**Ag**

_{2}SO_{4}**(s)**

**+ H**

_{2}S**(s)**

## H_{2}SO_{4}_{ }+Ag_{2}S conjugate pairs

**H _{2}SO_{4 }+Ag_{2}S reaction don’t form**

**conjugate pairs**

**because they do not conjugate to produce the products.**

## H_{2}SO_{4}_{ } and Ag_{2}S intermolecular forces

**H _{2}SO_{4 } and Ag_{2}S have the following intermolecular forces**,

**The intermolecular forces in H**_{2}SO_{4}are**Van der Waal’s dispersion****, Dipole-dipole interactions and****hydrogen bonding****.****Being an ionic compound,****Ag**_{2}S has**ion-dipole interactions.**

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

**The standard reaction enthalpy of the H _{2}SO_{4 }+Ag_{2}S reaction is negative.**

## Is H_{2}SO_{4}_{ }+Ag_{2}S a buffer solution?

**H _{2}SO_{4 }+Ag_{2}S don’t form a buffer solution because of the strong acid H_{2}SO_{4.}**

## Is H_{2}SO_{4}_{ }+Ag_{2}S a complete reaction?

**H _{2}SO_{4 }+Ag_{2}S reaction is complete because **

**hydrogen sulphide and silver sulphate are formed in the same amount and don’t undergo further reaction.**

## Is H_{2}SO_{4}_{ }+Ag_{2}S an exothermic or endothermic reaction?

**The reaction between H _{2}SO_{4 }+Ag_{2}S is an exothermic reaction and the heat released is used to complete the reaction.**

## Is H_{2}SO_{4}_{ }+Ag_{2}S a redox reaction?

**Redox reaction doesn’t occur when H _{2}SO_{4 }+Ag_{2}S react because the oxidation state of reactants and products remains the same.**

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

**H _{2}SO_{4} + Ag_{2}S is a precipitation reaction as it leads to the formation of precipitates like **

**Ag**

_{2}SO_{4}and H_{2}S.## Is H_{2}SO_{4} + Ag_{2}S reversible or irreversible reaction?

**The reaction between H _{2}SO_{4 }+Ag_{2}S is irreversible as the reactants do not combine with products to reform them.**

## Is H_{2}SO_{4} + Ag_{2}S displacement reaction?

**H _{2}SO_{4} + Ag_{2}S is a**

**double displacement reaction cations and anions exchange their position resulting in the formation of a new product.**

**Conclusion**

In conclusion, the reaction between H_{2}SO_{4} + Ag_{2}S has a high synthetic application and can be categorized as a double displacement and precipitation reaction with a negative enthalpy. The reaction is irreversible. Heat is liberated during the process.