Advertisements
Advertisements
प्रश्न
Explain the types of buffer solutions.
Advertisements
उत्तर
There are two types of buffer solutions:
- Acidic buffer:
A solution containing a weak acid and its salts with strong base is called an acidic buffer solution. It maintains an acidic pH.
e.g. A solution containing weak acid such as CH3COOH and its salt such as CH3COONa is an acidic buffer solution. - Basic buffer:
A solution containing a weak base and its salt with strong acid is the basic buffer solution. It maintains an alkaline pH.
e.g. A solution containing a weak base such as NH4OH and its salt such as NH4Cl is a basic buffer solution.
संबंधित प्रश्न
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?
When NH4 Cl and NH4OH are added to a solution containing both, Fe3+ and Ca2+ ions, which ion is precipitated first and why?
A solution of NH4Cl and NH4OH acts as a buffer.
Cu is precipitated as CuS while Zn is not precipitated when H2S is passed through an acidic solution of Cu(NO3 )2 and Zn(NO3)2 respectively.
Choose the most correct answer:
Which of the Na following is a buffer solution?
Answer the following in one sentence :
How are basic buffer solutions prepared?
Answer the following in one sentence :
Write one property of a buffer solution.
In biochemical system, pH of blood in our body is maintained due to the following buffer:
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 ______.
Which will make basic buffer?
Ksp of Al(OH)3 is 1 × 10−15 M. At what pH does 1.0 × 10−3 M Al3+ precipitate on the addition of buffer of NH4Cl and NH4OH solution?
Which of the following will produce a buffer solution when mixed in equal volumes?
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.
Calculate the pH of buffer solution composed of 0.01 M weak base BOH and 0.02 M of its salt BA. [Kb = 1.8 × 10–5 for weak base]
Explain the types of buffers with example.
Explain buffer action of sodium acetate-acetic acid buffer.
What is the pH of buffer solution prepared by mixing \[\text{0.2MNH4OHand0.4MNH4Cl}\] solution. \[(\mathrm{pK_{b}~of~NH_{4}OH=4.620})\]
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].
A buffer solution is prepared by mixing 0.01 М HCN and 0.02 M sodium cyanide. If pKa for HCN is 5.20, what is the pH of solution?
