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Question
Write any four applications of buffer solution.
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Solution
Buffer solution finds extensive applications in a variety of fields. Some of its applications are given.
- In a biochemical system: pH of blood in our body is maintained at 7.36 - 7.42 due to \[\ce{(HCO^-3 + H2CO3)}\] buffer. A mere change of 0.2 pH units can cause death. The saline solution used for intravenous injection must contain a buffer system to maintain the proper pH of the blood.
- Agriculture: The soils get buffered due to the presence of salts such as carbonate, bicarbonate, phosphates, and organic acids. The choice of fertilizers depends upon the pH of the soil.
- Industry: Buffers play an important role in the paper, dye, ink, paint, and drug industries.
- Medicine: Penicillin preparations are stabilized by the addition of sodium citrate as a buffer. When citric acid is added to milk of magnesia (Mg(OH)2), magnesium citrate is formed, which is a buffer.
- Analytical chemistry: In qualitative analysis, a pH of 8 to 10 is required for precipitation of cations IIIA group. It is maintained with the use of (NH4OH + NH4Cl) buffer.
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RELATED QUESTIONS
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Which of the Na following is a buffer solution?
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CH3COOH + CH3COONa
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NH4OH + NH4Cl
In biochemical system, pH of blood in our body is maintained due to the following buffer:
The pKb of weak base BOH [Kb(BOH) = 1 × 10-5] will be ______.
Name the buffer which is used to maintained pH of 8 to 10 for precipitation of cations III A group in qualitative analysis.
Write the formula to calculate pH of buffer solution.
Define buffer solution.
Write one application of the following buffer:
Citrate buffer
Write one application of the following buffer:
NH4OH + NH4Cl
A buffer solution contains 0.3 mol dm–3 NH4OH (Kb = 1.8 × 10–5) and 0.4 mol dm–3 NH4Cl. Calculate pOH of the solution.
Veronal is used as a/an ______.
What is the pH of 0.5 litre buffer solution containing 0.01 mole of CH3COOH and 0.01 mole of CH3COONa?
[pKa of acid = 4.74]
Which will make basic buffer?
The dissociation constant of a weak acid is 1 × 10−3. In order to prepare a buffer solution with a pH = 4, the `(["Acid"])/(["Salt"])` ratio should be ____________.
The hydrogen ion concentration of a buffer solution consisting of a weak acid and its salts is given by ____________.
Which of the following will produce a buffer solution when mixed in equal volumes?
Assertion (A): A solution containing a mixture of acetic acid and sodium acetate maintains a constant value of \[\ce{pH}\] on addition of small amounts of acid or alkali.
Reason (R): A solution containing a mixture of acetic acid and sodium acetate acts as a buffer solution around \[\ce{pH}\] 4.75.
Which of the following combinations will constitute a buffer solution?
Define Acidic buffer solution.
