Which of the following solution cannot act as a buffer?
(a) NaH₂PO₄ + H₃PO₄
(b) CH₃COOH+CH₃COONa
(c) HCl + NH₄Cl
(d) H₃PO4 + NaH₂PO₄
Answers
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Among the given combinations, the following solution cannot act as a buffer:
(c) HCl + NH₄Cl
1. Buffer solution has to be a weak acid / base with its salt is a strong base/ acid respectively.
2. In this case the acid HCl is strong and the salt NH₄Cl is strong as well.
3. Thus, this combination cannot form a buffer.
Answered by
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HCl + NH₄Cl is the correct combination.
Explanation:
- A buffer solution is defined as the solution which prevents a change in pH of the solution and restricts the pH within a narrow margin.
- A buffer solution is formed of a weak acid and its salt with strong base.
- This is called acid buffer.
- Or it can be formed of a weak base and its salt with strong acid.
- This is a basic buffer.
- Here among the options, NaH₂PO₄ + H₃PO₄, CH₃COOH + CH₃COONa and H₃PO4 + NaH₂PO₄ are weak acids and their salt with strong bases.
- But HCl + NH₄Cl is a strong acid and its salt with weak base.
- So its not a buffer.
For more information about buffer,
https://brainly.in/question/2190431
State the role of buffer solution in the given titration - Brainly.in
https://brainly.in/question/5671386
define buffer solution . explain buffer action - Brainly.in
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