Advertisements
Advertisements
प्रश्न
Choose the most correct answer:
Which of the Na following is a buffer solution?
विकल्प
CH3COONa + NaCl in water
CH3COOH + HCl in water
CH3COOH + CH3COONa in water
HCl + NH4Cl in water
Advertisements
उत्तर
CH3COOH + CH3COONa in water
Explanation:
A buffer solution is a water-based mixture of a weak acid and its conjugate base. It could potentially be a combination of a weak base and its conjugate base.
In the given, only option C has weak acid CH3COOH and its conjugate base CH3COONa
Option A has a strong base and its conjugate base.
Options D and B are not buffer solutions as they contain strong acids HCl.
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.
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
The pKb of weak base BOH [Kb(BOH) = 1 × 10-5] will be ______.
Define buffer solution.
Write one application of the following buffer:
Citrate buffer
Write one application of the following buffer:
`"HCO"_3^- + "H"_2"CO"_3`
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]
____________ forms a basic buffer solution.
Which will make basic buffer?
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?
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.
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 0.1 M ammonia solution and 0.25 M solution of NH4CI. What is the value of pKb to maintain its pOH at 6?
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?
