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प्रश्न
Write one application of the following buffer:
NH4OH + NH4Cl
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उत्तर
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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संबंधित प्रश्न
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.
Answer the following in one sentence :
How are basic buffer solutions prepared?
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
Answer the following in one sentence :
Classify the following buffers into different types :
Cu(OH)2 + CuCl2
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.
Explain the types of buffer solutions.
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.
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]
____________ forms a basic buffer solution.
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 ____________.
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.
Define Acidic buffer solution.
Write any four applications of buffer solution.
What are buffer solutions?
Explain the types of buffers with example.
