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प्रश्न
Write any four applications of buffer solution.
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उत्तर
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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The ionization constant of benzoic acid is 6.46 × 10–5 and Ksp for silver benzoate is 2.5 × 10–13. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?
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In biochemical system, pH of blood in our body is maintained due to the following buffer:
Write the formula to calculate pH of buffer solution.
Define buffer solution.
Explain the types of buffer solutions.
Write one application of the following buffer:
`"HCO"_3^- + "H"_2"CO"_3`
Veronal is used as a/an ______.
Which will make basic buffer?
On the basis of the equation \[\ce{pH}\] = – log \[\ce{[H+]}\], the \[\ce{pH}\] of 10–8 mol dm–3 solution of \[\ce{HCl}\] should be 8. However, it is observed to be less than 7.0. Explain the reason.
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.
Assertion (A): An aqueous solution of ammonium acetate can act as a buffer.
Reason (R): Acetic acid is a weak acid and \[\ce{NH4OH}\] is a weak base.
Which of the following combinations will constitute a buffer solution?
What are buffer solutions?
Calculate pKa of HF if Ka= 7.2 x 10-4.
What is the pH of buffer solution formed by mixing 0.01 M acetic acid and 0.05 M sodium acetate? (pKa = 4.7447)
Calculate the pOH of a buffer solution formed from 0.3 M weak base and 0.45 M of its salt with strong acid [pKb = 4.7447].
