The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is
[Given pKa of CH3COOH = 4.57]
[Given pKa of CH3COOH = 4.57]
- 5.57
- 3.57
- 4.57
- 2.57
The Correct Option is A
Approach Solution - 1
To find the pH of the given solution, we will use the Henderson-Hasselbalch equation, which is applicable for buffer solutions containing a weak acid and its conjugate base. The formula is:
pH = pKa + log10([A-]/[HA])
Where:
- pH is the hydrogen ion concentration.
- pKa is the acid dissociation constant. For acetic acid (CH3COOH), pKa = 4.57.
- [A-] is the molarity of the conjugate base, sodium acetate (CH3COONa).
- [HA] is the molarity of the weak acid, acetic acid (CH3COOH).
Given:
- Volume of sodium acetate solution = Volume of acetic acid solution = 50 mL
- [CH3COONa] = 0.10 M
- [CH3COOH] = 0.01 M
50mL each, the concentrations remain as:
- [A-] = 0.10 M
- [HA] = 0.01 M
Now, apply these values to the Henderson-Hasselbalch equation:
pH = 4.57 + log10(0.10/0.01)
Compute the logarithm:
- [0.10/0.01 = 10]
- log10(10) = 1
Substitute in the equation:
pH = 4.57 + 1
pH = 5.57
Thus, the pH of the solution is 5.57.
Approach Solution -2
- pKa = 4.57 (given)
- [A-] = concentration of the acetate ion, which is equal to the concentration of sodium acetate = 0.10 M
- [HA] = concentration of acetic acid = 0.01 M
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NEET Notification
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