Advertisements
Advertisements
Question
Which of the following will produce a buffer solution when mixed in equal volumes?
Options
0.1 mol dm–3 \[\ce{NH4OH}\] and 0.1 mol dm–3 \[\ce{HCl}\]
0.05 mol dm–3 \[\ce{NH4OH}\] and 0.1 mol dm–3 \[\ce{HCl}\]
0.1 mol dm–3 \[\ce{NH4OH}\] and 0.05 mol dm–3 \[\ce{HCl}\]
0.1 mol dm–3 \[\ce{CH4COONa}\] and 0.1 mol dm–3 \[\ce{NaOH}\]
Advertisements
Solution
0.1 mol dm–3 \[\ce{NH4OH}\] and 0.05 mol dm–3 \[\ce{HCl}\]
Explanation:
When 0.1 mol dm–3 \[\ce{NH4OH}\] and 0.05 mol dm–3 \[\ce{HCl}\] react total amount of \[\ce{HCl}\] reacts with \[\ce{NH4OH}\] to form \[\ce{NH4Cl}\] and some \[\ce{NH4OH}\] will be left unreacted. Thus, the resultant solution contains \[\ce{NH4Cl}\] and \[\ce{NH4OH}\] which will produce a buffer solution.
APPEARS IN
RELATED QUESTIONS
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.
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 :
Classify the following buffers into different types :
CH3COOH + CH3COONa
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:
Name the buffer which is used to maintained pH of 8 to 10 for precipitation of cations III A group in qualitative analysis.
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 ______.
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): 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.
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]
Define Acidic buffer solution.
Write any four applications of buffer solution.
What are buffer solutions?
Explain the types of buffers with example.
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?
