What is the $pH$ value of $M H _{2} SO _{4}$ ?
- 0
- -0.213
- -2
- -0.301
The Correct Option is D
Approach Solution - 1
The correct answer is Option is D) -0.301
\(M H _{2} SO _{4} =2 N H _{2} SO _{4}\)
\(\left[ H ^{+}\right] =N \cdot \alpha\)
\(=2 \times 1=2\)
\(pH =-\log \left[ H ^{+}\right]\)
\(=-\log 2\)
\(=-0.3010\)
Read more from chapter: Equilibrium
Approach Solution -2
The correct answer is Option is D) -0.301
Real Life Applications
- A range of chemical compounds, including active medicinal components, are synthesized using it as a solvent. Alkylating agents, which are frequently used in chemotherapy (cancer treatment), are one type of active medicinal component produced utilizing sulphuric acid.
- Phosphoric acid, which is required to prepare phosphate fertilizers, is made from sulfuric acid, which is utilized in enormous quantities in this process.
- It is employed in the production of Lead-Acid batteries. Lead-acid sealed-unit batteries are utilized in the automobile sector for vehicles and trucks.
- Gas samples for CEMS also include sulfuric acid. Batteries for automobiles. Sulfuric acid is used in the pulp and paper industry to produce chlorine dioxide on-site, which is a crucial bleaching component of the ecologically friendly ECF chemical pulping process. .Sulfuric acid is also used to produce cellulose fibers like rayon fiber.
- Steel production: Today, petroleum refining successfully cleans petrol and other refinery products of contaminants.
- It serves as a colouring agent in the creation of colours, medications, and disinfectants.
Question can also be asked as
- What is the pH of a 1 M solution of H2SO4?
- What is the pH of a 0.005 M solution of H2SO4?
- What is the pH of a solution of H2SO4 with a concentration of 2.5 x 10^-3 M?
- What is the pH of a solution of H2SO4 with a [H+] concentration of 0.01 M?
- What is the pH of a solution of H2SO4 that is 0.1% acidic?
Approach Solution -3
pH is the measurement of the alkalinity and acidity of the solution. It is measured by the amount of H+ ions in the solution. pH is a unitless quantity. pH is a concept given by Soren Sorensen. The full form of pH is the power of Hydrogen. pH scale ranges from 0 to 14.
- pH< 7: Acidic
- pH> 7: Basic
- pH= Neutral
pH formula
- When an acid is added to the water, it can release H+ ions and that will form H30+ ions.
- Strong acids will have lower pH, since they can easily release hydrogen ions.
- Acidic solutions have a concentration of hydrogen ions of [H+] > 10-7 M.
pH= -log [H]+
pH = - log[ H30+]
- For acidic solutions, the pH is [H3O+] > [OH–].
- For neutral solutions, the pH is [H3O+] = [OH–].
- For basic solutions, the pH is [H3O+] < [OH–].
pH Value Equation:
The equilibrium equation of weak acids are as follows:
HA= H⁺ + A⁻
Where,
- [H3O+] is Hydronium Concentration.
- [A-] is Conjugate Base Concentration.
- HA is the Weak Acid Concentration.
Application of pH Scale
Some of the applications of pH scale are as follows:
- It is used in industries like pharmacy
- pH of the medicine so that it is not harmful for the body
- Buffer solutions are made for maintaining the pH of the solution
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Concepts Used:
Equilibrium
An equilibrium represents a state in a process when the observable properties such as color, temperature, pressure, concentration etc do not show any change.
The word equilibrium means ‘balance’ which indicates that a chemical reaction represents a balance between the reactants and products taking part in the reaction. The equilibrium state is also noticed in certain physical processes such as the melting point of ice at 0℃, both ice and water are present at equilibrium.
In the case of physical processes such as the melting of solid, dissolution of salt in water etc., the equilibrium is called physical equilibrium while the equilibrium associated with chemical reaction is known as chemical equilibrium.
Equilibrium in Chemical changes
The chemical equilibrium in a reversible reaction is the state at which both forward and backward reactions occur at the same speed.
The stage of the reversible reaction at which the concentration of the reactants and products do not change with time is called the equilibrium state.
Read More: Calculating Equilibrium Concentration
Types of Chemical Equilibrium
There are two types of chemical equilibrium:
- Homogeneous Equilibrium
- Heterogeneous Equilibrium
Homogenous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are all in the same phase. Homogenous equilibrium can be further divided into two types: Reactions in which the number of molecules of the products is equal to the number of molecules of the reactants. For example,
- H2 (g) + I2 (g) ⇌ 2HI (g)
- N2 (g) + O2 (g) ⇌ 2NO (g)
Reactions in which the number of molecules of the products is not equal to the total number of reactant molecules. For example,
- 2SO2 (g) + O2 (g) ⇌ 2SO3 (g)
- COCl2 (g) ⇌ CO (g) + Cl2 (g)
Heterogeneous Chemical Equilibrium
In this type, the reactants and the products of chemical equilibrium are present in different phases. A few examples of heterogeneous equilibrium are listed below.
- CO2 (g) + C (s) ⇌ 2CO (g)
- CaCO3 (s) ⇌ CaO (s) + CO2 (g)
Thus, the different types of chemical equilibrium are based on the phase of the reactants and products.
Check Out: Equilibrium Important Questions