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The Chemistry Behind Ag2CrO4 and H2SO4: Reactions and Properties Explored

Ag2CrO4 and H2SO4: Understanding Their Chemical Properties and Reaction

Have you ever wondered about the chemistry behind the substances and materials that we encounter in our daily lives? Two such substances are Ag2CrO4 and H2SO4.

In this article, we will delve into the chemical properties of these compounds, the reaction that occurs between them, and the resultant product.

Composition and Characteristics of Ag2CrO4

Ag2CrO4 is a ternary ionic solid composed of silver, chromium, and oxygen. It takes the form of red crystals that are insoluble in water.

The compound is commonly referred to as silver chromate and is mainly used as a pigment in paints and dyes. It has a high refractive index and is capable of absorbing ultraviolet rays, making it useful in photography.

Interestingly, its chromate transition shifts as its particle size decreases.

Characteristics and Reactivity of H2SO4

H2SO4, also known as sulfuric acid or oil of vitriol, is a highly corrosive and strong mineral acid. It appears as a colorless, oily liquid with sp3 hybridization.

It is widely used in industries such as agriculture, chemical manufacturing, and petroleum refining. Battery acid is also a dilute form of sulfuric acid.

Due to its highly reactive nature, it can cause severe burns on contact with the skin and needs to be handled with care. It works as an oxidizing agent and reacts violently with metals, producing hydrogen gas.

Reaction Between H2SO4 and Ag2CrO4

When Ag2CrO4 is mixed with H2SO4, a double displacement reaction takes place. The hydrogen ions (H+) from the sulfuric acid displace the silver ions (Ag+) in Ag2CrO4, resulting in the formation of silver sulfate (Ag2SO4) and chromic acid (H2CrO4).

Ag2CrO4 + H2SO4 Ag2SO4 + H2CrO4

This reaction is exothermic and releases energy in the form of heat. It involves a redox reaction, where one substance is reduced (Ag2CrO4) while the other is oxidized (H2SO4).

In the process, the sulfuric acid is reduced to sulfur dioxide, while the chromate ion in H2CrO4 is oxidized to yield dichromate.

Balancing the Equation

The molecular equation for the reaction between Ag2CrO4 and H2SO4 can be represented as:

Ag2CrO4 + H2SO4 Ag2SO4 + H2CrO4

When the equation is balanced, the ionic equation becomes:

2Ag+ + CrO4 2 + 2H+ + SO4 2 Ag2SO4 + H2CrO4


Ag2CrO4 and H2SO4 are two fascinating compounds that exhibit unique properties and reactions. Through their composition, characteristics, and reactions, we can gain a better understanding of the world around us.

The ability to balance chemical equations and identify the products of the reactions can bring about advancements in chemistry and improve our daily lives.

Titration of H2SO4 and Ag2CrO4

Titration is a process that determines the concentration and strength of a given solution by reacting it with another solution of known concentration. In this section, we will look at the titration of H2SO4 and Ag2CrO4 and calculate the strength of the former.

Apparatus and Procedure

To conduct the titration, we will need a burette, a conical flask, a beaker, and a methyl orange indicator. The procedure is as follows:


Measure 25 ml of Ag2CrO4 into the conical flask. 2.

Add a few drops of methyl orange indicator to the conical flask. 3.

Fill the burette with H2SO4 of known concentration. 4.

Slowly add H2SO4 to the Ag2CrO4 solution until the color of the mixture changes. 5.

Record the volume of H2SO4 required to trigger the color change.

Calculation of H2SO4 Strength

Using the balanced equation: Ag2CrO4 + H2SO4 Ag2SO4 + H2CrO4

We can deduce that one mole of H2SO4 will react with one mole of Ag2CrO4. Therefore, we can calculate the number of moles of H2SO4 used in the reaction.

Moles of H2SO4 = [Volume of H2SO4 (in liters) x Concentration of H2SO4 (in moles / liter)]

Once we have calculated the number of moles of H2SO4 used, we can find the concentration of H2SO4. Concentration of H2SO4 = Moles of H2SO4 / Volume of Ag2CrO4 (in liters)

Net Ionic Equation and Conjugate Pairs

A net ionic equation is a reaction equation that eliminates spectator ions. In this section, we will write the net ionic equation for Ag2CrO4 and H2SO4 and examine the conjugate pairs of H2SO4 and H2CrO4.

Writing the Net Ionic Equation

Ag2CrO4 is an insoluble salt, and when it reacts with H2SO4, it becomes soluble. Therefore, the net ionic equation will show only the dissolved ions.

The solubility equation for Ag2CrO4 is: Ag2CrO4 2Ag+ + CrO4 2

The complete equation for the reaction is: Ag2CrO4 + H2SO4 Ag2SO4 + H2CrO4

Breaking down the equation based on solubility, we get:

CrO4 2 (aq) + H+ (aq) HCrO4 (aq)

Ag2CrO4 (s) + H2SO4 (aq) Ag2SO4 (aq) + HCrO4 (aq)

Eliminating the spectator ions, we get the net ionic equation:

Ag2CrO4 (s) + 2H+ (aq) Ag2SO4 (aq) + HCrO4 (aq)

Conjugate Pairs of H2SO4 and H2CrO4

In the reaction equation, H2SO4 acts as an acid, donating a proton to H2CrO4, which acts as a base. The resulting conjugate pairs are:

HSO4 / SO42-

– HSO4 is the acid, and SO42- is its conjugate base.

– HSO4 donates a proton to water, forming H3O+, making it an acidic oxo-acid. CrO42- / HCrO4-

– CrO42- is the base, and HCrO4- is its conjugate acid.

– CrO42- accepts a proton from water, forming OH-, making it a basic oxo-anion.

Intermolecular Forces

A molecule’s intermolecular forces determine its physical properties and behavior. In this section, we will examine the three types of intermolecular forces: dipole-dipole force, London dispersion force, and hydrogen bonding.

Dipole-Dipole Force

The dipole-dipole force occurs between polar molecules and is the result of the attractive force between the partial positive and negative charges of two molecules. H2CrO4’s molecule is polar due to the electronegativity difference between oxygen and hydrogen atoms.

London Dispersion Force

London dispersion force is also known as Van der Waal’s force and occurs between all atoms or molecules, regardless of their polarity. It is the result of uneven electron distribution, which creates temporary dipoles.

Both H2SO4 and Ag2CrO4 exhibit London dispersion force.

Hydrogen Bonding

Hydrogen bonding occurs in polar molecules containing hydrogen atoms bonded to highly electronegative atoms such as oxygen, nitrogen, or fluorine. H2CrO4 exhibits hydrogen bonding due to its polar nature and the presence of two hydrogen atoms bonded to the highly electronegative oxygen atom.


In summary, the titration of H2SO4 and Ag2CrO4 helps us to determine the concentration and strength of H2SO4. The net ionic equation of Ag2CrO4 and H2SO4 showcases the removal of spectator ions.

Lastly, the intermolecular forces present in H2SO4 and H2CrO4 have interesting implications on their respective behavior.

Reaction Enthalpy and Other Characteristics

In this section, we will explore the reaction enthalpy and other characteristics of the reaction between H2SO4 and Ag2CrO4. We will discuss the calculation of enthalpy change, buffer solutions, completeness of reaction, and endothermic or exothermic reaction.

Calculation of Enthalpy Change

The enthalpy change is a measure of the heat transferred between a system and its surroundings during a chemical reaction. It can be calculated using the enthalpy of formation (Hf) of the reactants and products.

The enthalpy change is given by:

H = sum of [products enthalpy of formation – reactants enthalpy of formation]

The enthalpy of formation is the energy change that occurs when one mole of a substance is formed from its constituent elements in their standard states at 25C and 1 atm pressure. The following values can be used to calculate the enthalpy change:

Ag2CrO4 (s) 2Ag+ + CrO42- Enthalpy of formation = -719 kJ/mol

H2SO4 (aq) H+ + HSO4- Enthalpy of formation = -814 kJ/mol

Ag2SO4 (s) + H2CrO4 (aq)

Using enthalpy of formation, we get:

H = (-1398 kJ/mol) – (-1629 kJ/mol) = 231 kJ/mol

Buffer Solution and Completeness of Reaction

Buffer solutions resist changes in pH when small amounts of an acid or base are added to them. A buffer solution contains a weak acid and its conjugate base.

In this reaction, H2SO4 acts as a strong acid, while HCrO4 acts as a weak acid. HCrO4’s conjugate base, CrO42-, acts as a buffer.

Hence, the reaction is not able to maintain a constant pH. The completeness of the reaction depends on various factors, including the concentration of reactants, duration of reaction, and temperature.

When the reaction proceeds to completion, it means that all reactants have been consumed to form the products. In this reaction, the formation of Ag2SO4 and HCrO4 indicates the completeness of the reaction.

Endothermic or Exothermic Reaction

The net change of enthalpy (H) in a reaction indicates whether it is endothermic or exothermic. In an endothermic reaction, heat is absorbed, while in an exothermic reaction, heat is released.

To determine if the reaction between H2SO4 and Ag2CrO4 is endothermic or exothermic, we calculate the H, as shown above, and note that it is a positive value. Therefore, the reaction is endothermic.

Redox and Precipitation Reactions

Redox reactions are reactions in which there is a transfer of electrons between two reactants. In the reaction between H2SO4 and Ag2CrO4, Ag2CrO4 is oxidized to form Ag2SO4, while H2SO4 is reduced to form H2CrO4.

Ag2CrO4 + H2SO4 Ag2SO4 + HCrO4

In the above equation, Ag2CrO4 donates electrons, while H2SO4 accepts them. This exchange of electrons causes a change in the oxidation states of Ag and Cr in Ag2CrO4.

Precipitation reactions involve the formation of an insoluble solid when two aqueous solutions combine. In this reaction, the formation of Ag2SO4 is a precipitation reaction.

Ag2SO4 is insoluble in water, and its formation causes it to precipitate out of the solution.

Reversibility and Displacement of Reaction

The reversibility of a reaction depends on the stability and energy of the reactants, products, and intermediate species. An irreversible reaction proceeds in only one direction and cannot return to its original condition.

In the reaction between H2SO4 and Ag2CrO4, the formation of Ag2SO4 and HCrO4 is irreversible. Ag2SO4 and HCrO4 are both stable compounds, and their formation is favorable due to the high energy of the reactants.

The displacement of a reaction involves the exchange of ions between two compounds. In this reaction, we have a double displacement reaction, where the ions Ag+ and H+ are exchanged between the reactants H2SO4 and Ag2CrO4, forming the products Ag2SO4 and HCrO4.


In conclusion, the reaction between H2SO4 and Ag2CrO4 has several characteristics, including the calculation of enthalpy change, buffer solutions, and completeness of reaction. The reaction is endothermic and involves a redox reaction that results in a precipitation of Ag2SO4.

The reaction is irreversible, and its products’ stability favors the formation of Ag2SO4 and HCrO4, resulting in a double displacement reaction. Understanding these characteristics of the reaction helps us understand the chemical nature of the reactants and products.

In conclusion, the article has explored the chemical properties and reactions of Ag2CrO4 and H2SO4. Ag2CrO4 is a red ternary ionic solid, while H2SO4 is a strong acid commonly known as oil of vitriol.

When these two substances react, they undergo a double displacement reaction, forming silver sulfate (Ag2SO4) and chromic acid (H2CrO4). The reaction is exothermic and involves a redox process.

The article also discussed the calculation of enthalpy change, the use of buffer solutions, and the irreversibility of the reaction. Understanding these concepts helps deepen our knowledge of chemical reactions and their properties, highlighting the importance of chemistry in our daily lives.


Q: What are the products formed when H2SO4 and Ag2CrO4 react? A: The products formed are silver sulfate (Ag2SO4) and chromic acid (H2CrO4).

Q: Is the reaction between H2SO4 and Ag2CrO4 exothermic or endothermic? A: The reaction is endothermic, meaning it absorbs heat.

Q: Can the reaction between H2SO4 and Ag2CrO4 be reversed? A: No, the reaction is irreversible due to the stability of the products formed.

Q: Does the reaction between H2SO4 and Ag2CrO4 involve a precipitation reaction? A: Yes, the formation of Ag2SO4 is a precipitation reaction as it forms an insoluble solid.

Q: What is the importance of understanding the properties of Ag2CrO4 and H2SO4? A: Understanding these properties helps us comprehend chemical reactions and their role in various industrial processes and daily life applications.

Closing thought: Chemistry’s intricate world offers captivating insights into the properties and reactions of substances like Ag2CrO4 and H2SO4, enhancing our understanding of the fundamental principles governing the composition and behavior of matter. By unraveling these intricate details, we unlock the potential for advancements in various sectors and foster an appreciation for the wonders of the chemical world.

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