Hydrogen iodide(HI) is a yellow gas while copper sulfate (CuSO_{4}), a blue crystalline solid liquifies in water to form copper sulfate solutions. Let us see some of their properties.

**HI being very volatile reacts with numerous organic compounds. CuSO _{4} is a very vital compound in the industrial sector since it is utilized in an extensive variety of applications including agriculture, manufacturing, and construction.**

This article will deliver thorough facts about the various characteristics of the interaction between HI and CuSO_{4}.

**What is the product of ****HI and CuSO**_{4} ?

**HI and CuSO**

_{4}?**The product of the interaction between HI and CuSO _{4} is copper(I) iodide (CuI) along with sulfuric acid (H_{2}SO_{4}).**

**HI + CuSO _{4 }→ CuI + H_{2}SO_{4}**

**What type of reaction is HI and CuSO**_{4}

_{4}

**HI and CuSO _{4} lie under a double displacement reaction, also identified as a metathesis reaction.**

**How to balance HI and CuSO**_{4}?

_{4}?

**HI + CuSO _{4}**

**reaction is balanced in the following underneath steps,**

**Count both the left and right sides of the equation to determine how many atoms there are for each element.****Equalize the number of atoms for each element so that they are evenly distributed on both sides.****For the elements HI and H**_{2}SO_{4}, add coefficients (numbers in front of the element symbols) of 2 and 1, respectively, to bring them to the corresponding values on the right, which are 2 and 1.**To make the CuSO**._{4}and CuI elements’ respective coefficients on the right side equal to those on the left, add 1 and 2 there, respectively**Now that the equation is balanced:****2HI + CuSO**_{4}→ 2CuI + H_{2}SO_{4}

**HI and CuSO**_{4} **titration**

_{4}

**HI + CuSO _{4} titration is accomplished to determine the amount of HI in a solution. By identifying the concentration of CuSO_{4} utilized in the titration, the amount of HI available in the solution can be found**.

__Apparatus__

__Apparatus__

**Pipette, different-sized beakers (250 ml-1, 100 ml-3), grease stand with pencil, burette clamp, and a 250 ml flask**

__Indicator__

__Indicator__

**The end-point of the titration is identified using the acid-base reagent ****Phenolphthalein****.**

__Procedur__e

__Procedur__

**Pour a volumetric flask with a known amount of HI solution.****Fill the flask with a few drops of phenolphthalein indicator.****Using a burette, add the****CuSO**solution to the flask._{4}**Stir the flask vigorously to achieve complete mixing.****Pay attention to how the indicator’s color changes. The endpoint is attained when the solution takes on a faint pink hue.****Note the quantity of****CuSO**solution that was used._{4}**Employ the titration equation(S**_{1}V_{1}=S_{2}V_{2}) to determine the amount of HI present in the solution.**For better outcomes replicate the procedure 2-3 times.**

**HI + ****CuSO**_{4} net ionic equation

**CuSO**net ionic equation

_{4}**The net ionic equation for the reaction:**

**2H ^{+} + Cu^{2+} + SO_{4}^{2- }→ 2Cu^{+} + H_{2}SO_{4}**

**Dividing the chemical equation into its individual ions is the first step. This can be decomposed into****2H**^{+}+ I^{–}+ Cu^{2+}+ SO_{4}^{2-}→ 2Cu^{+}+ I^{–}+ H_{2}SO_{4}

**Equilibrating the equation is the next step. To accomplish this, multiply the reactants and products until they are all equal to one another. By multiplying the reactants and products by two, the equation in this instance can be made to balance.**

**2H**^{+}+ 2I^{–}+ 2Cu^{2+}+ 2SO_{4}^{2-}→ 2Cu^{+}+ 2I^{–}+ H_{2}SO_{4 }is the balanced equation.

**Eliminating the spectator ions is step three. The iodide ions are the spectator ions in this instance. By removing the iodide ions from the equation, we are left with**

**2H**^{+}+ Cu^{2+}+ SO_{4}^{2- }→ 2Cu+ + H_{2}SO_{4}

**The net ionic equation must be written as the fourth and last step. The ions that are present on both the reactant and product sides of the equation are eliminated to achieve this. The net ionic equation in this instance is**

**2H**^{+}+ Cu^{2+}+ SO_{4}^{2- }→ 2Cu^{+}+ H_{2}SO_{4}

**HI + ****CuSO**_{4} conjugate pairs

**CuSO**conjugate pairs

_{4}** HI + CuSO_{4}** has the following conjugate pairs, differing by one proton:

**The conjugate acid-base pair of HI =****H**_{3}O**The conjugate acid-base pair of****CuSO**= Cu_{4}^{2+}.

**HI + ****CuSO**_{4} intermolecular forces

**CuSO**intermolecular forces

_{4}**HI + CuSO _{4} has the following intermolecular forces,**

**Hydrogen****bonds****and interactions between dipoles are the intermolecular forces that hold HI and****CuSO**together._{4}

**When the hydrogen atom of HI is drawn to the oxygen atom of****CuSO**, hydrogen bonds are created. This is because the oxygen atom in_{4}**CuSO**is slightly negative and the hydrogen atom in HI is slightly positive._{4}

**HI and****CuSO**also interact via dipole-dipole interactions. This is because HI is slightly polar, which means that its electrons are distributed unevenly, and_{4}**CuSO**is similarly polar, which means that its electrons are distributed unevenly._{4}

**HI + ****CuSO**_{4} reaction enthalpy

**CuSO**reaction enthalpy

_{4}**The reaction enthalpy of HI + CuSO_{4} is -80.14 kJ/mol. This reaction can be stated as follows:**

**HI (g) +****CuSO**(s) → CuI (s) + H_{4}_{2}SO_{4 }(g)

**The reaction enthalpy of this reaction can be considered using the subsequent equation:**

**ΔH = ΣHf (products) – ΣHf (reactants)**

**Where ΣHf is the sum of the standard enthalpies of the formation of the reactants and products.**

**Therefore, the reaction enthalpy can be calculated as follows:**

**ΔH = (-890.1 kJ/mol) + (-41.7 kJ/mol) – (-100.7 kJ/mol)**

**ΔH = -80.14 kJ/mol.**

**Is HI + ****CuSO**_{4} a buffer solution?

**CuSO**a buffer solution?

_{4}**HI + CuSO_{4} cannot be referred to as a **

**buffer solution**

**.**

**As the modest amounts of acid or base are added, the pH of a buffer solution does not change. This definition is not met by HI +**

**CuSO**._{4}**Is HI + ****CuSO**_{4} a complete reaction?

**CuSO**a complete reaction?

_{4}**HI + CuSO_{4} is not really a complete reaction since the reactants and products can change back and forth into one another in constant dynamic equilibrium.**

**Is HI + ****CuSO**_{4} an exothermic or endothermic reaction?

**CuSO**an exothermic or endothermic reaction?

_{4}**HI + CuSO_{4} is exothermic and generates a sizable amount of heat energy.**

**Is HI + ****CuSO**_{4} a redox reaction?

**CuSO**a redox reaction?

_{4}**HI + CuSO_{4} is stated to as a **

**redox process**

**.**

**.**

**CuSO**undergoes oxidation in this process, to produce CuI. Reduced H_{4}_{2}gets electrons to create H_{2}SO_{4}**Is HI + ****CuSO**_{4} a precipitation reaction?

**CuSO**a precipitation reaction?

_{4}**HI + CuSO_{4} is stated to as a **

**precipitation**

**reaction because**

**two ions (Cu**

^{2+}and SO_{4}^{2-}) in the reactants interact to produce a new molecule, a solid precipitate (CuI) is formed. The sulphate ions (SO_{4}^{2-}) and hydronium ions (H_{3}O^{+}) are still in solution.**Is HI + ****CuSO**_{4} a reversible or irreversible reaction?

**CuSO**a reversible or irreversible reaction?

_{4}**HI + CuSO_{4} is stated to as a **

**reversible reaction**

**.**

**As the left-side reactants (2HI and**

**CuSO**) can become the products (2CuI and H_{4}_{2}SO_{4}), and the products (2CuI and H_{2}SO_{4}) can be transformed back into reactants through the reaction 2HI +**CuSO**= 2CuI + H_{4}_{2}SO_{4}(2HI and**CuSO**)._{4}**Is HI + CuSO**_{4} a displacement reaction?

_{4}a displacement reaction?

**HI + CuSO_{4} is stated to as a displacement reaction**.

**As iodine (I) in this reaction displaces copper (Cu) from copper sulphate (**

**CuSO**) (I)._{4}**Copper iodide (CuI) and sulfuric acid (H**

_{2}SO_{4}), are the byproducts of the process**Conclusion**

To broad HI + CuSO4 is a reversible reaction which forms yellow colored precipitate resulting into release of energy. Interaction between both results into formation of displaced product copper iodide (CuI) and sulfuric acid (H_{2}SO_{4}) respectively.

Hello…I’m Ritika Vaishnav, a Chemistry Subject Matter Expert with a passion for creating educational and engaging content on a wide range of topics related to chemistry. With a master’s degree in Chemistry, I have written for a variety of publications, including research papers. My writing is concise and well-researched, and I strive to make complex topics easily understandable for readers.

“I’m interested in everything related to Chemistry and its aligned fields!”

Connect me via LinkedIn: