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For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10–5)
- a)1 : 10
- b)10 : 1
- c)100 : 1
- d)1 : 100
Correct answer is option 'B'. Can you explain this answer?
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Buffer Solution:
A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. It is composed of a weak acid and its conjugate base (or a weak base and its conjugate acid) in approximately equal concentrations.
Acetic Acid and Sodium Acetate:
Acetic acid (CH3COOH) is a weak acid and sodium acetate (CH3COONa) is its conjugate base. When acetic acid dissolves in water, it donates a proton (H+) to water to form the acetate ion (CH3COO-) and hydronium ion (H3O+).
CH3COOH + H2O ⇌ CH3COO- + H3O+
On the other hand, sodium acetate dissociates in water to release acetate ions and sodium ions.
CH3COONa ⇌ CH3COO- + Na+
pH of Buffer Solution:
The pH of a buffer solution is determined by the equilibrium between the weak acid and its conjugate base. In this case, the equilibrium can be represented as:
CH3COOH + H2O ⇌ CH3COO- + H3O+
The Ka value (acid dissociation constant) for acetic acid is given as 10^-5. The Ka expression for this equilibrium is:
Ka = [CH3COO-][H3O+] / [CH3COOH]
Since the pH of the buffer solution is 6, the concentration of hydronium ions ([H3O+]) is 10^-6 M.
Now, let's consider the ratio of the concentration of sodium acetate ([CH3COO-]) to acetic acid ([CH3COOH]) in the buffer solution.
Calculation:
Using the Ka expression, we can rearrange it to find the ratio of salt to acid:
Ka = [CH3COO-][H3O+] / [CH3COOH]
10^-5 = [CH3COO-] * 10^-6 / [CH3COOH]
Cross-multiplying and rearranging, we get:
[CH3COO-] / [CH3COOH] = 10^-5 * 10^6
[CH3COO-] / [CH3COOH] = 10
Therefore, the ratio of the concentration of sodium acetate to acetic acid should be 10:1. This means that for every 10 moles of sodium acetate, there should be 1 mole of acetic acid in the buffer solution.
Conclusion:
To prepare a buffer solution of pH 6 using sodium acetate and acetic acid, the ratio of the concentration of salt to acid should be 10:1. This ensures the presence of sufficient amounts of the weak acid and its conjugate base to resist changes in pH when small amounts of acid or base are added to the solution.
A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. It is composed of a weak acid and its conjugate base (or a weak base and its conjugate acid) in approximately equal concentrations.
Acetic Acid and Sodium Acetate:
Acetic acid (CH3COOH) is a weak acid and sodium acetate (CH3COONa) is its conjugate base. When acetic acid dissolves in water, it donates a proton (H+) to water to form the acetate ion (CH3COO-) and hydronium ion (H3O+).
CH3COOH + H2O ⇌ CH3COO- + H3O+
On the other hand, sodium acetate dissociates in water to release acetate ions and sodium ions.
CH3COONa ⇌ CH3COO- + Na+
pH of Buffer Solution:
The pH of a buffer solution is determined by the equilibrium between the weak acid and its conjugate base. In this case, the equilibrium can be represented as:
CH3COOH + H2O ⇌ CH3COO- + H3O+
The Ka value (acid dissociation constant) for acetic acid is given as 10^-5. The Ka expression for this equilibrium is:
Ka = [CH3COO-][H3O+] / [CH3COOH]
Since the pH of the buffer solution is 6, the concentration of hydronium ions ([H3O+]) is 10^-6 M.
Now, let's consider the ratio of the concentration of sodium acetate ([CH3COO-]) to acetic acid ([CH3COOH]) in the buffer solution.
Calculation:
Using the Ka expression, we can rearrange it to find the ratio of salt to acid:
Ka = [CH3COO-][H3O+] / [CH3COOH]
10^-5 = [CH3COO-] * 10^-6 / [CH3COOH]
Cross-multiplying and rearranging, we get:
[CH3COO-] / [CH3COOH] = 10^-5 * 10^6
[CH3COO-] / [CH3COOH] = 10
Therefore, the ratio of the concentration of sodium acetate to acetic acid should be 10:1. This means that for every 10 moles of sodium acetate, there should be 1 mole of acetic acid in the buffer solution.
Conclusion:
To prepare a buffer solution of pH 6 using sodium acetate and acetic acid, the ratio of the concentration of salt to acid should be 10:1. This ensures the presence of sufficient amounts of the weak acid and its conjugate base to resist changes in pH when small amounts of acid or base are added to the solution.
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For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10–5)a)1 : 10b)10 : 1c)100 : 1d)1 : 100Correct answer is option 'B'. Can you explain this answer?
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For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10–5)a)1 : 10b)10 : 1c)100 : 1d)1 : 100Correct answer is option 'B'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10–5)a)1 : 10b)10 : 1c)100 : 1d)1 : 100Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10–5)a)1 : 10b)10 : 1c)100 : 1d)1 : 100Correct answer is option 'B'. Can you explain this answer?.
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