Advertisements
Advertisements
प्रश्न
Define Acidic buffer solution.
Advertisements
उत्तर
A solution containing a weak acid and its salts with strong base is called an acidic buffer solution.
APPEARS IN
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?
A solution of NH4Cl and NH4OH acts as a buffer.
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.
Answer the following in one sentence :
Classify the following buffers into different types :
NH4OH + NH4Cl
Answer the following in one sentence :
Classify the following buffers into different types :
Sodium benzoate + benzoic acid
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.
Write one application of the following buffer:
Citrate buffer
Write one application of the following buffer:
`"HCO"_3^- + "H"_2"CO"_3`
Write one application of the following buffer:
NH4OH + NH4Cl
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 ____________.
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?
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.
Explain buffer action of sodium acetate-acetic acid buffer.
A buffer solution is prepared by mixing 0.1 M ammonia solution and 0.25 M solution of NH4CI. What is the value of pKb to maintain its pOH at 6?
