Which of the following does not form a buffer solution?
Which of the following does not form a buffer solution?
NH3+HCL (2:1 mole ratio)
CH3CO2H + NaOH (2:1 mole ratio)
NaOH + CH3COOH (1:1 mole ratio)
NH4Cl + NH3 (1:1 mole ratio)
The Correct Option is C
Solution and Explanation
The correct option is: (C): NaOH + CH3COOH (1:1 mole ratio).
The solution of NaOH (sodium hydroxide) and CH3COOH (acetic acid) in a 1:1 mole ratio does not form a buffer solution. A buffer solution consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. This combination helps the solution resist changes in pH when an acid or base is added.
In the case of NaOH and CH3COOH, you have a strong base (NaOH) and a weak acid (CH3COOH), but they are not a conjugate acid-base pair. Buffer solutions require a weak acid and its conjugate base (or vice versa) to effectively maintain a stable pH. The weak acid in the buffer system donates protons (H+) to counteract any added base, while its conjugate base absorbs protons to counteract any added acid.
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Concepts Used:
Law of Chemical Equilibrium
Law of Chemical Equilibrium states that at a constant temperature, the rate of a chemical reaction is directly proportional to the product of the molar concentrations of the reactants each raised to a power equal to the corresponding stoichiometric coefficients as represented by the balanced chemical equation.
Let us consider a general reversible reaction;
A+B ↔ C+D
After some time, there is a reduction in reactants A and B and an accumulation of the products C and D. As a result, the rate of the forward reaction decreases and that of backward reaction increases.
Eventually, the two reactions occur at the same rate and a state of equilibrium is attained.
By applying the Law of Mass Action;
The rate of forward reaction;
Rf = Kf [A]a [B]b
The rate of backward reaction;
Rb = Kb [C]c [D]d
Where,
[A], [B], [C] and [D] are the concentrations of A, B, C and D at equilibrium respectively.
a, b, c, and d are the stoichiometric coefficients of A, B, C and D respectively.
Kf and Kb are the rate constants of forward and backward reactions.
However, at equilibrium,
Rate of forward reaction = Rate of backward reaction.
Kc is called the equilibrium constant expressed in terms of molar concentrations.
The above equation is known as the equation of Law of Chemical Equilibrium.