Which will make basic buffer?
- $100\, mL \,of\, 0.1\, M \,HCI\, + \,100\, mL\, of\, 0.1\, M\, NaOH$
- $100\, mL \,of\, 0.1\, M \,HCI \,+ \,100\, mL\, of\, 0.1\, M \,NaOH$
- $50 \,mL \,of\, 0 .1\, M \,NaOH\, + \,25 \,mL\, of \,0.1 M \,CH_3COOH$
- $100\, mL\, of\, 0.1 \,M \,CH_3COOH + 100\, mL 0.1\, MNaOH$
The Correct Option is A
Approach Solution - 1
Approach Solution -2
A basic buffer solution contains a weak base and its salt. To determine which of the options (A, B, C, or D) is the correct basic buffer solution:
- Calculate the number of moles of reactants and products in each option.
- Check if the solution contains a weak base (NH4OH) and its salt (NH4Cl).
- Compare the moles of reactants and products to determine if the solution is a buffer solution.
Option A (100 mL of 0.1 M HCl + 200 mL of 0.1 M NH4OH) contains a weak base (NH4OH) and its salt (NH4Cl), and has a larger amount of base compared to acid, making it the correct basic buffer solution.
Approach Solution -3
The reaction between acetic acid (CH3COOH) and sodium hydroxide (NaOH) is:
CH3COOH + NaOH -> CH3COONa + H2O.
For the mixture 50 ml of 0.1M NaOH + 25 ml of 0.1M CH3COOH, the initial moles are:
moles of CH3COOH = 0.1 M * 25 ml = 2.5 mol moles of NaOH = 0.1 M * 50 ml = 5.0 mol
The mole ratio of CH3COOH and NaOH is 1:1. So 2.5 mol of CH3COOH reacts with 2.5 mol of NaOH, giving 2.5 mmol of CH3COONa. The solution contains 2.5 mmol of unreacted NaOH, 0 mol of CH3COOH and 2.5 mmol of CH3COONa. The solution is basic, but not a buffer solution as it does not contain CH3COOH.
For the mixture 100 ml of 0.1M CH3COOH + 100 ml of 0.1M NaOH, the initial moles are:
moles of CH3COOH = 0.1 M * 100 ml = 10 mol
moles of NaOH = 0.1 M * 100 ml = 10 mol
The mole ratio of CH3COOH and NaOH is 1:1. So 10 mol of CH3COOH reacts with 10 mol of NaOH, giving 10 mmol of CH3COONa. The solution contains 0 mol of unreacted NaOH and CH3COOH, and 10mmol of CH3COONa. The solution is neutral, not a basic buffer solution.
Hence, the correct answer is (1) 100 ml of 0.1M CH3COOH + 100 ml of 0.1M NaOH.
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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