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Which of the following is an example of basic buffer?
- a)A mixture of HCl and NaOH
- b)A mixture of NH4Cl and NH4OH
- c)A mixture of CH3COOH and OH3COONa
- d)1M solution of NaOH
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
Which of the following is an example of basic buffer?a)A mixture of HC...
Acidic buffer solution contains equimolar quantities of a weak acid and its salt with strong base. For example: an acetic acid, CH3COOH and sodium acetate I.e. CH3COONa. Basic buffer solution contains equimolar quantities of a weak base and its salt with strong acid.
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Which of the following is an example of basic buffer?a)A mixture of HC...
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 the given options, option B is an example of a basic buffer. Let's understand why.
Explanation:
Buffer Solution
- A buffer solution is made up of a weak acid and its conjugate base or a weak base and its conjugate acid.
- It helps maintain the pH of a solution by neutralizing the added acid or base.
Mixture of NH4Cl and NH4OH
- In option B, the mixture of NH4Cl (ammonium chloride) and NH4OH (ammonium hydroxide) is a basic buffer solution.
- NH4Cl is the salt of a weak base (NH4OH) and a strong acid (HCl).
- NH4OH is a weak base that can donate OH- ions.
- NH4Cl can dissociate into NH4+ and Cl- ions.
- When NH4Cl and NH4OH are mixed, NH4+ ions from the salt react with OH- ions from NH4OH to form NH4OH.
- NH4OH acts as a weak base and NH4Cl acts as a weak acid in the solution.
- This reaction helps maintain the pH of the solution when acid or base is added.
Other Options
- Option A, a mixture of HCl and NaOH, is not a buffer solution. It is a neutralization reaction where HCl (strong acid) reacts with NaOH (strong base) to form water and a salt.
- Option C, a mixture of CH3COOH (acetic acid) and OH3COONa (sodium acetate), is a buffer solution. It is an example of an acidic buffer.
- Option D, a 1M solution of NaOH, is not a buffer solution. It is a strong base solution.
In conclusion, option B, a mixture of NH4Cl and NH4OH, is an example of a basic buffer solution because it contains a weak acid (NH4Cl) and its conjugate base (NH4OH).
In the given options, option B is an example of a basic buffer. Let's understand why.
Explanation:
Buffer Solution
- A buffer solution is made up of a weak acid and its conjugate base or a weak base and its conjugate acid.
- It helps maintain the pH of a solution by neutralizing the added acid or base.
Mixture of NH4Cl and NH4OH
- In option B, the mixture of NH4Cl (ammonium chloride) and NH4OH (ammonium hydroxide) is a basic buffer solution.
- NH4Cl is the salt of a weak base (NH4OH) and a strong acid (HCl).
- NH4OH is a weak base that can donate OH- ions.
- NH4Cl can dissociate into NH4+ and Cl- ions.
- When NH4Cl and NH4OH are mixed, NH4+ ions from the salt react with OH- ions from NH4OH to form NH4OH.
- NH4OH acts as a weak base and NH4Cl acts as a weak acid in the solution.
- This reaction helps maintain the pH of the solution when acid or base is added.
Other Options
- Option A, a mixture of HCl and NaOH, is not a buffer solution. It is a neutralization reaction where HCl (strong acid) reacts with NaOH (strong base) to form water and a salt.
- Option C, a mixture of CH3COOH (acetic acid) and OH3COONa (sodium acetate), is a buffer solution. It is an example of an acidic buffer.
- Option D, a 1M solution of NaOH, is not a buffer solution. It is a strong base solution.
In conclusion, option B, a mixture of NH4Cl and NH4OH, is an example of a basic buffer solution because it contains a weak acid (NH4Cl) and its conjugate base (NH4OH).
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Which of the following is an example of basic buffer?a)A mixture of HCl and NaOHb)A mixture of NH4Cl and NH4OHc)A mixture of CH3COOH and OH3COONad)1M solution of NaOHCorrect answer is option 'B'. Can you explain this answer?
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